Question

Write a balanced equation for the chemical reaction, including states, using your calculated empirical formula. Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) Determine the theoretical yield of zinc chloride that can be produced from your reaction. Show work. Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) 1 mol of Zn produces 1 mol of ZnCl2 Molar mass of ZnCl2 = 65.38 g/mol Mass of Zn = 0.5 g Theoretical yield = (0.5 g / 65.38 g/mol) * 1 mol = 0.00765 mol Theoretical yield = 0.00765 mol * 65.38 g/mol = 0.5 g What is the limiting reactant? Which reactant is in excess? The limiting reactant is Zn. The reactant in excess is HCl. Calculate the percent yield of zinc chloride. Show work. Actual yield = 0.45 g Percent yield = (0.45 g / 0.5 g) * 100% = 90%

          Write a balanced equation for the chemical reaction, including states, using your calculated empirical formula.
Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)

Determine the theoretical yield of zinc chloride that can be produced from your reaction. Show work.
Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)
1 mol of Zn produces 1 mol of ZnCl2
Molar mass of ZnCl2 = 65.38 g/mol
Mass of Zn = 0.5 g
Theoretical yield = (0.5 g / 65.38 g/mol) * 1 mol = 0.00765 mol
Theoretical yield = 0.00765 mol * 65.38 g/mol = 0.5 g

What is the limiting reactant? Which reactant is in excess?
The limiting reactant is Zn.
The reactant in excess is HCl.

Calculate the percent yield of zinc chloride. Show work.
Actual yield = 0.45 g
Percent yield = (0.45 g / 0.5 g) * 100% = 90%

Show more…

Added by Katrina F.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Chareen Guzman

05/12/2023

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Step 1: Write the balanced equation for the chemical reaction: Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) Show more…

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Write a balanced equation for the chemical reaction, including states, using your calculated empirical formula. Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) Determine the theoretical yield of zinc chloride that can be produced from your reaction. Show work. Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) 1 mol of Zn produces 1 mol of ZnCl2 Molar mass of ZnCl2 = 65.38 g/mol Mass of Zn = 0.5 g Theoretical yield = (0.5 g / 65.38 g/mol) * 1 mol = 0.00765 mol Theoretical yield = 0.00765 mol * 65.38 g/mol = 0.5 g What is the limiting reactant? Which reactant is in excess? The limiting reactant is Zn. The reactant in excess is HCl. Calculate the percent yield of zinc chloride. Show work. Actual yield = 0.45 g Percent yield = (0.45 g / 0.5 g) * 100% = 90%

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Transcript

00:01 Hi, so we are to solve for the mass of the product and identify the limiting reactant in the given reaction.

00:08 So we have here the balance equation already.

00:10 We'll identify first the limiting reactant, convert the given mass of reactants to moles first, number of zinc, or number of moles of zinc is equivalent to 71 .24 grams of zinc, divide the atomic mass of zinc, which is equivalent to 65 .38 grams, and then we have moles in the numerator.

00:32 So that means we'll cancel grams and we'll get 1 .0896.

00:37 This is moles of zinc.

00:41 And then we have hydrochloric acid, hcl, 91 .53 grams divided by the molar mass of hcl.

00:49 That's 36 .46 grams here.

00:53 And then moles in the numerator, cancel grams, and we'll get 2 .504.

01:01 This is moles of hcl.

01:04 Now we will solve for the mole ratio.

01:09 So mole ratio in this case is the number of moles of the reactant divided by the coefficient of that reactant from the balance equation.

01:16 So for zinc, we have calculated 1 .0896 moles.

01:21 And then as per balance equation, the stoichiometric coefficient of zinc is 1.

01:27 So we'll get 1 .0896.

01:30 And then for hcl, we have calculated 2 .5104 divided by the coefficient of hcl from the balance equation, which is 2.

01:39 So we'll get 1 .2552.

01:44 Okay, so whichever gives the smallest mole ratio will be the limiting reactant.

01:50 So that means zinc is our limiting reactant...

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