Lead (IV) sulfate reacts with lithium nitrate, write a balanced equation to represent this reaction.
How many grams of lithium nitrate will be needed to make 250. grams of lithium sulfate. assuming that you have an adequate amount of lead (IV) sulfate?<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To start, let’s write the balanced chemical equation for the reaction between lead (IV) sulfate and lithium nitrate to form lithium sulfate and lead (IV) nitrate.<\/p>\n\n\n\n The reaction is:<\/p>\n\n\n\n [ In this equation, lead (IV) sulfate reacts with lithium nitrate to form lithium sulfate and lead (IV) nitrate.<\/p>\n\n\n\n To find the mass of lithium nitrate required to produce 250 g of lithium sulfate, we need to follow a few steps, beginning with determining the molar masses.<\/p>\n\n\n\n From the balanced equation, we know that 1 mole of Pb(SO\u2084)\u2082 produces 2 moles of Li\u2082SO\u2084. For every 1 mole of Li\u2082SO\u2084 produced, 4 moles of LiNO\u2083 are required.<\/p>\n\n\n\n We can use this information to set up a stoichiometric calculation.<\/p>\n\n\n\n To make 250.0 grams of lithium sulfate, 242.6 grams of lithium nitrate<\/strong> will be needed, assuming an adequate amount of lead (IV) sulfate is available.<\/p>\n","protected":false},"excerpt":{"rendered":" Lead (IV) sulfate reacts with lithium nitrate, write a balanced equation to represent this reaction.How many grams of lithium nitrate will be needed to make 250. grams of lithium sulfate. assuming that you have an adequate amount of lead (IV) sulfate? The Correct Answer and Explanation is : To start, let’s write the balanced chemical […]<\/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-185704","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185704","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=185704"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185704\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185704"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185704"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185704"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\\text{Pb(SO}_4\\text{)}_2 + 4 \\text{LiNO}_3 \\rightarrow 2 \\text{Li}_2\\text{SO}_4 + \\text{Pb(NO}_3\\text{)}_4
]<\/p>\n\n\n\nStep 1: Determining the Molar Masses<\/h3>\n\n\n\n
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Step 2: Using Stoichiometry to Calculate Required Mass of Lithium Nitrate<\/h3>\n\n\n\n
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Conclusion:<\/h3>\n\n\n\n