Determine the theoretical yield of zinc chloride .4g zinc 6m hcl<\/p>\n\n\n\n
The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n To determine the theoretical yield of zinc chloride (ZnCl\u2082)<\/strong> from 0.4 g of zinc (Zn)<\/strong> reacting with 6 M hydrochloric acid (HCl)<\/strong>, we first need the balanced chemical equation<\/strong> and then apply stoichiometry<\/strong>.<\/p>\n\n\n\n Zn (s)+2HCl (aq)\u2192ZnCl2(aq)+H2(g)\\text{Zn (s)} + 2\\text{HCl (aq)} \\rightarrow \\text{ZnCl}_2\\text{(aq)} + \\text{H}_2\\text{(g)}<\/p>\n\n\n\n Atomic mass of Zn=65.38\u2009g\/mol\\text{Atomic mass of Zn} = 65.38 \\, \\text{g\/mol} Moles of Zn=0.4\u2009g65.38\u2009g\/mol\u22480.00612\u2009mol\\text{Moles of Zn} = \\frac{0.4 \\, \\text{g}}{65.38 \\, \\text{g\/mol}} \\approx 0.00612 \\, \\text{mol}<\/p>\n\n\n\n From the balanced equation: 1 mol Zn\u21921 mol ZnCl2\\text{1 mol Zn} \\rightarrow 1 \\text{ mol ZnCl}_2<\/p>\n\n\n\n So, Moles of ZnCl2=0.00612\u2009mol\\text{Moles of ZnCl}_2 = 0.00612 \\, \\text{mol}<\/p>\n\n\n\n Molar mass of ZnCl2=65.38+(35.45\u00d72)=136.28\u2009g\/mol\\text{Molar mass of ZnCl}_2 = 65.38 + (35.45 \u00d7 2) = 136.28 \\, \\text{g\/mol} Mass of ZnCl2=0.00612\u00d7136.28\u22480.834\u2009g\\text{Mass of ZnCl}_2 = 0.00612 \\times 136.28 \\approx 0.834 \\, \\text{g}<\/p>\n\n\n\n Theoretical yield of zinc chloride = 0.834 g<\/strong><\/p>\n\n\n\n The theoretical yield represents the maximum amount of product that can be formed from a given amount of reactants, assuming perfect conditions and complete reaction. In this case, we are calculating how much zinc chloride (ZnCl\u2082)<\/strong> can be produced from 0.4 grams of zinc<\/strong> using 6 M hydrochloric acid<\/strong>.<\/p>\n\n\n\n We begin with the balanced chemical equation<\/strong>: Zn+2HCl\u2192ZnCl2+H2\\text{Zn} + 2\\text{HCl} \\rightarrow \\text{ZnCl}_2 + \\text{H}_2<\/p>\n\n\n\n This shows that 1 mole of zinc<\/strong> reacts with 2 moles of hydrochloric acid<\/strong> to produce 1 mole of zinc chloride<\/strong>. Since we have an excess of HCl (as 6 M is highly concentrated), zinc is the limiting reactant<\/strong>\u2014it determines how much ZnCl\u2082 can be made.<\/p>\n\n\n\n Next, we convert 0.4 grams of zinc to moles using its atomic mass<\/strong> (65.38 g\/mol). This gives us approximately 0.00612 mol<\/strong> of zinc. Because the molar ratio of Zn to ZnCl\u2082 is 1:1, we expect to form 0.00612 mol of ZnCl\u2082<\/strong>.<\/p>\n\n\n\n To find the mass of zinc chloride produced<\/strong>, we multiply the moles of ZnCl\u2082 by its molar mass<\/strong>, which is 136.28 g\/mol. This results in a theoretical yield of about 0.834 grams<\/strong> of ZnCl\u2082.<\/p>\n\n\n\n This calculation is vital in chemistry labs to predict the efficiency of a reaction and compare it with the actual yield<\/strong> to determine percent yield<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":" Determine the theoretical yield of zinc chloride .4g zinc 6m hcl The correct answer and explanation is: To determine the theoretical yield of zinc chloride (ZnCl\u2082) from 0.4 g of zinc (Zn) reacting with 6 M hydrochloric acid (HCl), we first need the balanced chemical equation and then apply stoichiometry. \u2705 Balanced Chemical Equation: Zn (s)+2HCl (aq)\u2192ZnCl2(aq)+H2(g)\\text{Zn […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-16246","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16246","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=16246"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16246\/revisions"}],"predecessor-version":[{"id":16247,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16246\/revisions\/16247"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=16246"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=16246"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=16246"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\n\u2705 Balanced Chemical Equation<\/strong>:<\/h3>\n\n\n\n
\n\n\n\n\u2705 Step 1: Calculate moles of zinc used<\/strong><\/h3>\n\n\n\n
\n\n\n\n\u2705 Step 2: Use molar ratio to find moles of ZnCl\u2082<\/strong><\/h3>\n\n\n\n
\n\n\n\n\u2705 Step 3: Convert moles of ZnCl\u2082 to grams<\/strong><\/h3>\n\n\n\n
\n\n\n\n\u2705 Final Answer<\/strong>:<\/h3>\n\n\n\n
\n\n\n\n\u270d\ufe0f Explanation (Approx. 300 Words)<\/strong>:<\/h3>\n\n\n\n