Question

question 5 (2 points)
what is the theoretical yield in grams of hydrogen gas when 7.36 g zn reacts with 12.0 g of h₂so₄? report your answer to 3 decimal places but do not include the unit of grams in your response.
zn (s) + h₂so₄ (aq) → h₂ (g) + znso₄
your answer:
answer

Explanation:

Step1: Calculate moles of Zn

Molar mass of Zn is 65.38 g/mol. Moles of Zn = mass / molar mass = \( \frac{7.36}{65.38} \approx 0.1126 \) mol.

Step2: Calculate moles of \( H_2SO_4 \)

Molar mass of \( H_2SO_4 \) is \( 2(1.008) + 32.07 + 4(16.00) = 98.09 \) g/mol. Moles of \( H_2SO_4 = \frac{12.0}{98.09} \approx 0.1223 \) mol.

Step3: Determine limiting reactant

From the reaction \( Zn + H_2SO_4
ightarrow H_2 + ZnSO_4 \), the mole ratio of Zn to \( H_2SO_4 \) is 1:1. Zn has fewer moles (0.1126 < 0.1223), so Zn is the limiting reactant.

Step4: Calculate moles of \( H_2 \)

Mole ratio of Zn to \( H_2 \) is 1:1, so moles of \( H_2 = 0.1126 \) mol.

Step5: Calculate mass of \( H_2 \)

Molar mass of \( H_2 \) is 2.016 g/mol. Mass = \( 0.1126 \times 2.016 \approx 0.227 \) g.

Answer:

0.227