To determine the maximum number of moles and grams of iodic acid (HIO\u2083) that can form when iodine trichloride (ICl\u2083) reacts with water, follow these steps:<\/p>\n\n\n\n
Step 1: Write the Balanced Chemical Equation<\/strong><\/h3>\n\n\n\n[
ICl_3 + H_2O \\rightarrow HIO_3 + HCl
]
From this equation, 1 mole<\/strong> of ICl\u2083<\/strong> reacts with 1 mole<\/strong> of H\u2082O<\/strong> to form 1 mole<\/strong> of HIO\u2083<\/strong> and 3 moles<\/strong> of HCl<\/strong>.<\/p>\n\n\n\nStep 2: Determine the Molar Mass of Each Substance<\/strong><\/h3>\n\n\n\n\n- ICl\u2083:<\/strong><\/li>\n\n\n\n
- Iodine (I) = 126.90 g\/mol<\/li>\n\n\n\n
- Chlorine (Cl) = 35.45 g\/mol \u00d7 3 = 106.35 g\/mol<\/li>\n\n\n\n
- Molar mass of ICl\u2083 = 126.90 + 106.35 = 233.25 g\/mol<\/strong><\/li>\n\n\n\n
- H\u2082O:<\/strong><\/li>\n\n\n\n
- Hydrogen (H) = 1.008 g\/mol \u00d7 2 = 2.016 g\/mol<\/li>\n\n\n\n
- Oxygen (O) = 16.00 g\/mol<\/li>\n\n\n\n
- Molar mass of H\u2082O = 18.016 g\/mol<\/strong><\/li>\n\n\n\n
- HIO\u2083:<\/strong><\/li>\n\n\n\n
- Hydrogen (H) = 1.008 g\/mol<\/li>\n\n\n\n
- Iodine (I) = 126.90 g\/mol<\/li>\n\n\n\n
- Oxygen (O) = 16.00 g\/mol \u00d7 3 = 48.00 g\/mol<\/li>\n\n\n\n
- Molar mass of HIO\u2083 = 1.008 + 126.90 + 48.00 = 175.91 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
Step 3: Determine the Moles of Reactants<\/strong><\/h3>\n\n\n\n\n- Moles of ICl\u2083:<\/strong>
[
\\frac{632 \\text{ g}}{233.25 \\text{ g\/mol}} = 2.71 \\text{ moles}
]<\/li>\n\n\n\n- Moles of H\u2082O:<\/strong>
[
\\frac{117.6 \\text{ g}}{18.016 \\text{ g\/mol}} = 6.53 \\text{ moles}
]<\/li>\n<\/ul>\n\n\n\nStep 4: Identify the Limiting Reactant<\/strong><\/h3>\n\n\n\nSince the reaction follows a 1:1 mole ratio<\/strong>, compare the available moles:<\/p>\n\n\n\n\n- ICl\u2083 available = 2.71 moles<\/strong><\/li>\n\n\n\n
- H\u2082O available = 6.53 moles<\/strong><\/li>\n<\/ul>\n\n\n\n
Since ICl\u2083 is present in fewer moles, it is the limiting reactant<\/strong>.<\/p>\n\n\n\nStep 5: Determine the Maximum Amount of HIO\u2083 Produced<\/strong><\/h3>\n\n\n\nBecause 1 mole of ICl\u2083 produces 1 mole of HIO\u2083<\/strong>, the moles of HIO\u2083 formed are equal to the moles of ICl\u2083 reacted:
[
\\text{Moles of HIO\u2083} = 2.71 \\text{ moles}
]<\/p>\n\n\n\nConvert to grams:
[
2.71 \\text{ moles} \\times 175.91 \\text{ g\/mol} = 477.0 \\text{ g of HIO\u2083}
]<\/p>\n\n\n\n
Final Answer<\/strong><\/h3>\n\n\n\n\n- Maximum moles of HIO\u2083 formed = 2.71 moles<\/strong><\/li>\n\n\n\n
- Maximum mass of HIO\u2083 formed = 477.0 g<\/strong><\/li>\n<\/ul>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-740.png\")
<\/figure>\n\n\n\nHere is an image visually summarizing the reaction of iodine trichloride (ICl\u2083) with water (H\u2082O) to form iodic acid (HIO\u2083) and hydrochloric acid (HCl). The diagram includes molecular structures, the balanced equation, and a depiction of ICl\u2083 as the limiting reactant.<\/p>\n","protected":false},"excerpt":{"rendered":"
Calculate the maximum number of moles and grams of iodic acid (HIO3) that can form when 632 g iodine trichloride reacts with 117.6 g of water. The correct answer and explanation is : To determine the maximum number of moles and grams of iodic acid (HIO\u2083) that can form when iodine trichloride (ICl\u2083) reacts with […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-198611","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=198611"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198611"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198611"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198611"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
ICl_3 + H_2O \\rightarrow HIO_3 + HCl
]
From this equation, 1 mole<\/strong> of ICl\u2083<\/strong> reacts with 1 mole<\/strong> of H\u2082O<\/strong> to form 1 mole<\/strong> of HIO\u2083<\/strong> and 3 moles<\/strong> of HCl<\/strong>.<\/p>\n\n\n\n
Step 2: Determine the Molar Mass of Each Substance<\/strong><\/h3>\n\n\n\n\n- ICl\u2083:<\/strong><\/li>\n\n\n\n
- Iodine (I) = 126.90 g\/mol<\/li>\n\n\n\n
- Chlorine (Cl) = 35.45 g\/mol \u00d7 3 = 106.35 g\/mol<\/li>\n\n\n\n
- Molar mass of ICl\u2083 = 126.90 + 106.35 = 233.25 g\/mol<\/strong><\/li>\n\n\n\n
- H\u2082O:<\/strong><\/li>\n\n\n\n
- Hydrogen (H) = 1.008 g\/mol \u00d7 2 = 2.016 g\/mol<\/li>\n\n\n\n
- Oxygen (O) = 16.00 g\/mol<\/li>\n\n\n\n
- Molar mass of H\u2082O = 18.016 g\/mol<\/strong><\/li>\n\n\n\n
- HIO\u2083:<\/strong><\/li>\n\n\n\n
- Hydrogen (H) = 1.008 g\/mol<\/li>\n\n\n\n
- Iodine (I) = 126.90 g\/mol<\/li>\n\n\n\n
- Oxygen (O) = 16.00 g\/mol \u00d7 3 = 48.00 g\/mol<\/li>\n\n\n\n
- Molar mass of HIO\u2083 = 1.008 + 126.90 + 48.00 = 175.91 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n
Step 3: Determine the Moles of Reactants<\/strong><\/h3>\n\n\n\n\n- Moles of ICl\u2083:<\/strong>
[
\\frac{632 \\text{ g}}{233.25 \\text{ g\/mol}} = 2.71 \\text{ moles}
]<\/li>\n\n\n\n- Moles of H\u2082O:<\/strong>
[
\\frac{117.6 \\text{ g}}{18.016 \\text{ g\/mol}} = 6.53 \\text{ moles}
]<\/li>\n<\/ul>\n\n\n\nStep 4: Identify the Limiting Reactant<\/strong><\/h3>\n\n\n\nSince the reaction follows a 1:1 mole ratio<\/strong>, compare the available moles:<\/p>\n\n\n\n\n- ICl\u2083 available = 2.71 moles<\/strong><\/li>\n\n\n\n
- H\u2082O available = 6.53 moles<\/strong><\/li>\n<\/ul>\n\n\n\n
Since ICl\u2083 is present in fewer moles, it is the limiting reactant<\/strong>.<\/p>\n\n\n\nStep 5: Determine the Maximum Amount of HIO\u2083 Produced<\/strong><\/h3>\n\n\n\nBecause 1 mole of ICl\u2083 produces 1 mole of HIO\u2083<\/strong>, the moles of HIO\u2083 formed are equal to the moles of ICl\u2083 reacted:
[
\\text{Moles of HIO\u2083} = 2.71 \\text{ moles}
]<\/p>\n\n\n\nConvert to grams:
[
2.71 \\text{ moles} \\times 175.91 \\text{ g\/mol} = 477.0 \\text{ g of HIO\u2083}
]<\/p>\n\n\n\n
Final Answer<\/strong><\/h3>\n\n\n\n\n- Maximum moles of HIO\u2083 formed = 2.71 moles<\/strong><\/li>\n\n\n\n
- Maximum mass of HIO\u2083 formed = 477.0 g<\/strong><\/li>\n<\/ul>\n\n\n\n
<\/figure>\n\n\n\nHere is an image visually summarizing the reaction of iodine trichloride (ICl\u2083) with water (H\u2082O) to form iodic acid (HIO\u2083) and hydrochloric acid (HCl). The diagram includes molecular structures, the balanced equation, and a depiction of ICl\u2083 as the limiting reactant.<\/p>\n","protected":false},"excerpt":{"rendered":"
Calculate the maximum number of moles and grams of iodic acid (HIO3) that can form when 632 g iodine trichloride reacts with 117.6 g of water. The correct answer and explanation is : To determine the maximum number of moles and grams of iodic acid (HIO\u2083) that can form when iodine trichloride (ICl\u2083) reacts with […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-198611","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=198611"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198611"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198611"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198611"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Step 3: Determine the Moles of Reactants<\/strong><\/h3>\n\n\n\n\n- Moles of ICl\u2083:<\/strong>
[
\\frac{632 \\text{ g}}{233.25 \\text{ g\/mol}} = 2.71 \\text{ moles}
]<\/li>\n\n\n\n- Moles of H\u2082O:<\/strong>
[
\\frac{117.6 \\text{ g}}{18.016 \\text{ g\/mol}} = 6.53 \\text{ moles}
]<\/li>\n<\/ul>\n\n\n\nStep 4: Identify the Limiting Reactant<\/strong><\/h3>\n\n\n\nSince the reaction follows a 1:1 mole ratio<\/strong>, compare the available moles:<\/p>\n\n\n\n\n- ICl\u2083 available = 2.71 moles<\/strong><\/li>\n\n\n\n
- H\u2082O available = 6.53 moles<\/strong><\/li>\n<\/ul>\n\n\n\n
Since ICl\u2083 is present in fewer moles, it is the limiting reactant<\/strong>.<\/p>\n\n\n\nStep 5: Determine the Maximum Amount of HIO\u2083 Produced<\/strong><\/h3>\n\n\n\nBecause 1 mole of ICl\u2083 produces 1 mole of HIO\u2083<\/strong>, the moles of HIO\u2083 formed are equal to the moles of ICl\u2083 reacted:
[
\\text{Moles of HIO\u2083} = 2.71 \\text{ moles}
]<\/p>\n\n\n\nConvert to grams:
[
2.71 \\text{ moles} \\times 175.91 \\text{ g\/mol} = 477.0 \\text{ g of HIO\u2083}
]<\/p>\n\n\n\n
Final Answer<\/strong><\/h3>\n\n\n\n\n- Maximum moles of HIO\u2083 formed = 2.71 moles<\/strong><\/li>\n\n\n\n
- Maximum mass of HIO\u2083 formed = 477.0 g<\/strong><\/li>\n<\/ul>\n\n\n\n
<\/figure>\n\n\n\nHere is an image visually summarizing the reaction of iodine trichloride (ICl\u2083) with water (H\u2082O) to form iodic acid (HIO\u2083) and hydrochloric acid (HCl). The diagram includes molecular structures, the balanced equation, and a depiction of ICl\u2083 as the limiting reactant.<\/p>\n","protected":false},"excerpt":{"rendered":"
Calculate the maximum number of moles and grams of iodic acid (HIO3) that can form when 632 g iodine trichloride reacts with 117.6 g of water. The correct answer and explanation is : To determine the maximum number of moles and grams of iodic acid (HIO\u2083) that can form when iodine trichloride (ICl\u2083) reacts with […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-198611","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=198611"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198611"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198611"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198611"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
[
\\frac{632 \\text{ g}}{233.25 \\text{ g\/mol}} = 2.71 \\text{ moles}
]<\/li>\n\n\n\n
[
\\frac{117.6 \\text{ g}}{18.016 \\text{ g\/mol}} = 6.53 \\text{ moles}
]<\/li>\n<\/ul>\n\n\n\n
Step 4: Identify the Limiting Reactant<\/strong><\/h3>\n\n\n\nSince the reaction follows a 1:1 mole ratio<\/strong>, compare the available moles:<\/p>\n\n\n\n\n- ICl\u2083 available = 2.71 moles<\/strong><\/li>\n\n\n\n
- H\u2082O available = 6.53 moles<\/strong><\/li>\n<\/ul>\n\n\n\n
Since ICl\u2083 is present in fewer moles, it is the limiting reactant<\/strong>.<\/p>\n\n\n\nStep 5: Determine the Maximum Amount of HIO\u2083 Produced<\/strong><\/h3>\n\n\n\nBecause 1 mole of ICl\u2083 produces 1 mole of HIO\u2083<\/strong>, the moles of HIO\u2083 formed are equal to the moles of ICl\u2083 reacted:
[
\\text{Moles of HIO\u2083} = 2.71 \\text{ moles}
]<\/p>\n\n\n\nConvert to grams:
[
2.71 \\text{ moles} \\times 175.91 \\text{ g\/mol} = 477.0 \\text{ g of HIO\u2083}
]<\/p>\n\n\n\n
Final Answer<\/strong><\/h3>\n\n\n\n\n- Maximum moles of HIO\u2083 formed = 2.71 moles<\/strong><\/li>\n\n\n\n
- Maximum mass of HIO\u2083 formed = 477.0 g<\/strong><\/li>\n<\/ul>\n\n\n\n
<\/figure>\n\n\n\nHere is an image visually summarizing the reaction of iodine trichloride (ICl\u2083) with water (H\u2082O) to form iodic acid (HIO\u2083) and hydrochloric acid (HCl). The diagram includes molecular structures, the balanced equation, and a depiction of ICl\u2083 as the limiting reactant.<\/p>\n","protected":false},"excerpt":{"rendered":"
Calculate the maximum number of moles and grams of iodic acid (HIO3) that can form when 632 g iodine trichloride reacts with 117.6 g of water. The correct answer and explanation is : To determine the maximum number of moles and grams of iodic acid (HIO\u2083) that can form when iodine trichloride (ICl\u2083) reacts with […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-198611","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=198611"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198611"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198611"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198611"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- \n
- ICl\u2083 available = 2.71 moles<\/strong><\/li>\n\n\n\n
- H\u2082O available = 6.53 moles<\/strong><\/li>\n<\/ul>\n\n\n\n
Since ICl\u2083 is present in fewer moles, it is the limiting reactant<\/strong>.<\/p>\n\n\n\n
Step 5: Determine the Maximum Amount of HIO\u2083 Produced<\/strong><\/h3>\n\n\n\n
Because 1 mole of ICl\u2083 produces 1 mole of HIO\u2083<\/strong>, the moles of HIO\u2083 formed are equal to the moles of ICl\u2083 reacted:
[
\\text{Moles of HIO\u2083} = 2.71 \\text{ moles}
]<\/p>\n\n\n\nConvert to grams:
[
2.71 \\text{ moles} \\times 175.91 \\text{ g\/mol} = 477.0 \\text{ g of HIO\u2083}
]<\/p>\n\n\n\nFinal Answer<\/strong><\/h3>\n\n\n\n
- \n
- Maximum moles of HIO\u2083 formed = 2.71 moles<\/strong><\/li>\n\n\n\n
- Maximum mass of HIO\u2083 formed = 477.0 g<\/strong><\/li>\n<\/ul>\n\n\n\n
<\/figure>\n\n\n\nHere is an image visually summarizing the reaction of iodine trichloride (ICl\u2083) with water (H\u2082O) to form iodic acid (HIO\u2083) and hydrochloric acid (HCl). The diagram includes molecular structures, the balanced equation, and a depiction of ICl\u2083 as the limiting reactant.<\/p>\n","protected":false},"excerpt":{"rendered":"
Calculate the maximum number of moles and grams of iodic acid (HIO3) that can form when 632 g iodine trichloride reacts with 117.6 g of water. The correct answer and explanation is : To determine the maximum number of moles and grams of iodic acid (HIO\u2083) that can form when iodine trichloride (ICl\u2083) reacts with […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-198611","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=198611"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198611\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198611"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198611"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198611"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- Maximum mass of HIO\u2083 formed = 477.0 g<\/strong><\/li>\n<\/ul>\n\n\n\n
- H\u2082O available = 6.53 moles<\/strong><\/li>\n<\/ul>\n\n\n\n