객관식
A reaction requires 0.50 mol of H2SO4. What is the minimum mass of H2SO4 (in grams) needed to provide this amount?
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3. Chemical Reactions
Stoichiometry
객관식
Based on the mole ratio you determined in part c, how many moles of H2O are produced when 2 moles of H2 react completely with excess O2 according to the equation: 2 H2 + O2 → 2 H2O?
A
4 moles
B
0.5 mole
C
1 mole
D
2 moles
검증된 단계별 안내1
Identify the balanced chemical equation: \(2\ \mathrm{H_2} + \mathrm{O_2} \rightarrow 2\ \mathrm{H_2O}\).
Determine the mole ratio between \(\mathrm{H_2}\) and \(\mathrm{H_2O}\) from the balanced equation. Here, 2 moles of \(\mathrm{H_2}\) produce 2 moles of \(\mathrm{H_2O}\), so the ratio is \(\frac{2\ \mathrm{mol}\ \mathrm{H_2O}}{2\ \mathrm{mol}\ \mathrm{H_2}} = 1\).
Use the mole ratio to calculate the moles of \(\mathrm{H_2O}\) produced from 2 moles of \(\mathrm{H_2}\). Multiply the given moles of \(\mathrm{H_2}\) by the mole ratio: \(2\ \mathrm{mol}\ \mathrm{H_2} \times 1 = 2\ \mathrm{mol}\ \mathrm{H_2O}\).
Confirm that oxygen (\(\mathrm{O_2}\)) is in excess, so it does not limit the reaction and all \(\mathrm{H_2}\) reacts completely.
Conclude that 2 moles of \(\mathrm{H_2}\) produce 2 moles of \(\mathrm{H_2O}\) according to the balanced equation and mole ratio.
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