Multiple Choice
Consider the industrial conversion of ammonia to nitrogen monoxide: 2 N2H4(g) + 1 N2O4(g) → 3 N2(g) + 4 H2O(g). If H2O is produced at the rate of 0.66 mol/s, what is the rate of production of N2?
3. Chemical Reactions
Stoichiometry
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Determine the number of grams of H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 x 10^23 atoms of Fe according to the following reaction: 2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq).
A
0.050 grams
B
0.100 grams
C
0.025 grams
D
0.075 grams
Verified step by step guidance1
Calculate the moles of HCl in the solution using the formula: \( \text{moles of HCl} = \text{Molarity} \times \text{Volume in Liters} \). Convert 250.0 mL to liters by dividing by 1000.
Determine the moles of Fe using Avogadro's number: \( \text{moles of Fe} = \frac{3.41 \times 10^{23} \text{ atoms}}{6.022 \times 10^{23} \text{ atoms/mol}} \).
Use the stoichiometry of the balanced chemical equation \( 2 \text{HCl} + \text{Fe} \rightarrow \text{H}_2 + \text{FeCl}_2 \) to find the limiting reactant. Compare the mole ratio of HCl to Fe.
Calculate the moles of \( \text{H}_2 \) produced using the stoichiometry of the reaction. For every 2 moles of HCl, 1 mole of \( \text{H}_2 \) is produced.
Convert the moles of \( \text{H}_2 \) to grams using the molar mass of hydrogen gas \( \text{H}_2 \), which is approximately 2.02 g/mol. Use the formula: \( \text{grams of } \text{H}_2 = \text{moles of } \text{H}_2 \times 2.02 \text{ g/mol} \).
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