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Ch.3 - Chemical Reactions and Reaction Stoichiometry
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All textbooksBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblem 112

Chapter 3, Problem 112

A 3.50 g of an alloy which contains only lead and tin is dissolved in hot HNO3. Excess sulfuric acid is added to this solution and 1.57g of PbSO4(s) is obtained. (b) Assuming all the lead in the alloy reacted to form PbSO4, what was the amount, in grams, of lead and tin in the alloy respectively?

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Hi everyone. So we have a 5.37 g of an alloy containing nickel and copper. And it's placed in hcl liquid And were asked if 6.72 g of copper chloride is acquired. We need to determine the mass of nickel and copper in the alloy. And we assume that all hcl reacts with copper. So we're gonna have copper which is C. U plus H C. L. And it's gonna be your age too plus C. U C. L. And if you balance this we're gonna put a two in front of hcl And the two in front of c. u. c. So to find the mask of copper in the alloy, I need to convert from grams of copper chloride to malls of copper chloride into malls copper and then grams of copper. We have 6.72 g of copper chloride. And in one mole of copper chloride we have the molar mass And this is 63.546 grams plus 35 .453 grams. And this will give us Only have two moles of copper chloride and the reaction and one more of copper. And in one mall of copper we have the mass of copper Which is 63 .546. We're gonna get 2.16 g of copper. So now that we have the mass of copper we need to subtract the mass of copper from the mass of the alloy. To find the mask of nickel, We have 5.37 g of the alloy -2.16 g of copper. And this will give us 3.21 g of nickel. Thanks for watching my video, and I hope it was helpful.
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