When 7.68 g of zinc react with hydrochloric acid, what volume of hydrogen gas will be collected at 20.00C and 740 mm Hg?

V ≈ 2.9 L H₂

General Formulas and Concepts:

Chemistry - Atomic Structure

Chemistry - Reactions

Chemistry - Gas Laws

Combined Gas Law: PV = nRT

Temperature Conversion: K = °C + 273.15

Explanation:

Step 1: Define

Unbalanced RxN:   Zn (s) + HCl (aq) → ZnCl₂ (aq) + H₂ (g)

Balanced RxN:   Zn (s) + 2HCl (aq) → ZnCl₂ (aq) + H₂ (g)

Given:   7.68 g Zn, 20.00 °C, 740 mmHg

Step 2: Identify Conversions

Kelvin Conversion

Molar Mass of Zn - 65.39 g/mol

Step 3: Convert

Stoichiometry:   = 0.117449 mol H₂

Temp Conversion:   20.00 + 273.15 = 293.15 K

Step 4: Find V

Step 5: Check

We are given 2 sig figs as our lowest. Follow sig fig rules and round.

2.9033 L H₂ ≈ 2.9 L H₂

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