{"id":210072,"date":"2025-04-29T17:50:12","date_gmt":"2025-04-29T17:50:12","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=210072"},"modified":"2025-04-29T17:50:15","modified_gmt":"2025-04-29T17:50:15","slug":"how-many-grams-of-silver-iodide","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/29\/how-many-grams-of-silver-iodide\/","title":{"rendered":"how many grams of silver iodide"},"content":{"rendered":"\n

how many grams of silver iodide, AgI, are produced from 24.7 g of calcium iodide, CaI2<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

To determine how many grams of silver iodide (AgI) are produced from 24.7 g of calcium iodide (CaI2), we can use the stoichiometric method, which involves a series of steps: converting grams to moles, using the balanced chemical equation to find the mole ratio, and then converting moles back to grams.<\/p>\n\n\n\n

Step 1: Write the balanced chemical equation.<\/h3>\n\n\n\n

The reaction between calcium iodide (CaI2) and silver nitrate (AgNO3) to form silver iodide (AgI) and calcium nitrate (Ca(NO3)2) is as follows:<\/p>\n\n\n\n

[
\\text{CaI}_2 (aq) + 2 \\text{AgNO}_3 (aq) \\rightarrow 2 \\text{AgI} (s) + \\text{Ca(NO}_3)_2 (aq)
]<\/p>\n\n\n\n

This equation shows that 1 mole of CaI2 produces 2 moles of AgI.<\/p>\n\n\n\n

Step 2: Calculate the molar mass of calcium iodide (CaI2).<\/h3>\n\n\n\n

The molar mass of CaI2 is calculated by adding the atomic masses of calcium (Ca) and iodine (I):<\/p>\n\n\n\n

    \n
  • Molar mass of Ca = 40.08 g\/mol<\/li>\n\n\n\n
  • Molar mass of I = 126.90 g\/mol<\/li>\n<\/ul>\n\n\n\n

    So, the molar mass of CaI2 is:<\/p>\n\n\n\n

    [
    \\text{Molar mass of CaI}_2 = 40.08 \\, \\text{g\/mol} + (2 \\times 126.90 \\, \\text{g\/mol}) = 293.88 \\, \\text{g\/mol}
    ]<\/p>\n\n\n\n

    Step 3: Convert grams of CaI2 to moles.<\/h3>\n\n\n\n

    We have 24.7 g of CaI2, so we can convert this to moles by dividing by the molar mass of CaI2:<\/p>\n\n\n\n

    [
    \\text{Moles of CaI}_2 = \\frac{24.7 \\, \\text{g}}{293.88 \\, \\text{g\/mol}} = 0.084 \\, \\text{mol}
    ]<\/p>\n\n\n\n

    Step 4: Use the mole ratio to find moles of AgI.<\/h3>\n\n\n\n

    From the balanced equation, we know that 1 mole of CaI2 produces 2 moles of AgI. Therefore, the moles of AgI produced will be:<\/p>\n\n\n\n

    [
    \\text{Moles of AgI} = 0.084 \\, \\text{mol} \\times 2 = 0.168 \\, \\text{mol}
    ]<\/p>\n\n\n\n

    Step 5: Calculate the molar mass of AgI.<\/h3>\n\n\n\n

    The molar mass of AgI is:<\/p>\n\n\n\n

      \n
    • Molar mass of Ag = 107.87 g\/mol<\/li>\n\n\n\n
    • Molar mass of I = 126.90 g\/mol<\/li>\n<\/ul>\n\n\n\n

      [
      \\text{Molar mass of AgI} = 107.87 \\, \\text{g\/mol} + 126.90 \\, \\text{g\/mol} = 234.77 \\, \\text{g\/mol}
      ]<\/p>\n\n\n\n

      Step 6: Convert moles of AgI to grams.<\/h3>\n\n\n\n

      Now, we can convert moles of AgI to grams:<\/p>\n\n\n\n

      [
      \\text{Grams of AgI} = 0.168 \\, \\text{mol} \\times 234.77 \\, \\text{g\/mol} = 39.4 \\, \\text{g}
      ]<\/p>\n\n\n\n

      Final Answer:<\/h3>\n\n\n\n

      Thus, 24.7 g of calcium iodide (CaI2) will produce 39.4 g of silver iodide (AgI).<\/p>\n","protected":false},"excerpt":{"rendered":"

      how many grams of silver iodide, AgI, are produced from 24.7 g of calcium iodide, CaI2 The correct answer and explanation is : To determine how many grams of silver iodide (AgI) are produced from 24.7 g of calcium iodide (CaI2), we can use the stoichiometric method, which involves a series of steps: converting grams […]<\/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-210072","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/210072","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=210072"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/210072\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=210072"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=210072"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=210072"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}