Multiple Choice
How many liters of H2 gas, collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C, can be produced from 5.566 g of Zn reacting with excess HCl? The partial pressure of water vapor is 18.65 mm Hg.
3. Chemical Reactions
Stoichiometry
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How many grams of oxygen (O2) are needed to completely react with 1326.76 grams of ammonia (NH3) according to the balanced chemical equation: 4 NH3 + 5 O2 → 4 NO + 6 H2O?
A
1000 grams
B
2000 grams
C
1568 grams
D
3200 grams
Verified step by step guidance1
Identify the balanced chemical equation: 4 NH3 + 5 O2 → 4 NO + 6 H2O. This tells us that 4 moles of NH3 react with 5 moles of O2.
Calculate the molar mass of NH3. The molar mass of nitrogen (N) is approximately 14.01 g/mol and hydrogen (H) is approximately 1.01 g/mol. Therefore, the molar mass of NH3 is 14.01 + (3 * 1.01) g/mol.
Determine the number of moles of NH3 in 1326.76 grams. Use the formula: \( \text{moles of NH3} = \frac{\text{mass of NH3}}{\text{molar mass of NH3}} \).
Use the stoichiometry of the balanced equation to find the moles of O2 needed. According to the equation, 4 moles of NH3 react with 5 moles of O2. Therefore, \( \text{moles of O2} = \frac{5}{4} \times \text{moles of NH3} \).
Calculate the mass of O2 required using its molar mass. The molar mass of O2 is approximately 32.00 g/mol. Use the formula: \( \text{mass of O2} = \text{moles of O2} \times \text{molar mass of O2} \).
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