Multiple Choice
According to the following reaction, 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(l), how many grams of sulfur are formed when 37.4 g of water are produced?
3. Chemical Reactions
Stoichiometry
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Ammonia gas decomposes according to the equation: 2NH3(g) → N2(g) + 3H2(g). If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (also measured at STP)?
A
30.0 L
B
10.0 L
C
22.5 L
D
15.0 L
Verified step by step guidance1
Identify the balanced chemical equation for the decomposition of ammonia: 2NH₃(g) → N₂(g) + 3H₂(g). This equation tells us that 2 moles of NH₃ produce 1 mole of N₂ and 3 moles of H₂.
Recognize that at Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies 22.4 liters. This is a key concept for solving gas-related stoichiometry problems.
Determine the mole ratio between nitrogen and hydrogen from the balanced equation. For every 1 mole of N₂ produced, 3 moles of H₂ are produced.
Calculate the moles of nitrogen gas produced using the volume given: 15.0 L of N₂ at STP. Use the relationship: \( \text{moles of N}_2 = \frac{\text{volume of N}_2}{22.4 \text{ L/mol}} \).
Use the mole ratio to find the volume of hydrogen gas produced. Since 3 moles of H₂ are produced for every 1 mole of N₂, multiply the moles of N₂ by 3 to find the moles of H₂, then convert this to volume using the same STP conversion: \( \text{volume of H}_2 = \text{moles of H}_2 \times 22.4 \text{ L/mol} \).
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