Chemistry - Stoichiometry Question with Solution | TestHub
ChemistryStoichiometryProblems Based on Mixtures, Percentage PurityHard2 minQB
ChemistryHardnumerical
A quantity of 2.7 g of an alloy of copper and silver was dissolved in moderately conc. HNO₃ and excess of HCl was added to this solution when 2.87 g of a dry precipitate is formed. Calculate the percentage of copper in the alloy. (Cu = 63.5, Ag = 108)
Answer:
20.00
Solution:
Only Ag precipitates as AgCl (CuCl₂ is soluble). Moles AgCl = 2.87/143.5 = 0.02 mol = moles of Ag. Mass Ag = 0.02×108 = 2.16 g. Mass Cu = 2.7-2.16 = 0.54 g. %Cu = 0.54/2.7×100 = 20%. Ans 0020.
Stream:JEESubject:ChemistryTopic:StoichiometrySubtopic:Problems Based on Mixtures, Percentage Purity
⏱ 2mℹ️ Source: QB
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