We're being asked to determine how could the result of the reaction be checked without changing the given procedure. We're given the following balanced reaction:
Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g) (Cu does not react with HCl.)
First, we need to calculate the amount of zinc needed to produce 0.0985 g ZnCl2.
From the balanced reaction: 1 mole of Zn produces 1 mole of ZnCl2.
mass ZnCl2 (molar mass ZnCl2) → moles ZnCl2 (mole-to-mole comparison) → moles Zn (molar mass Zn) → mass Zn
molar mass of Zn = 65.39 g/mol
molar mass of ZnCl2:
Commercial brass, an alloy of Zn and Cu, reacts with hydrochloric acid as follows:
Zn (s) + 2 HCl (aq) → ZnCl 2 (aq) + H2 (g) (Cu does not react with HCl.)
When 0.5065 g of a certain brass alloy is reacted with excess HCl, 0.0985 g ZnCl2 is eventually isolated. How could this result be checked without changing the above procedure?
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.