객관식
What volume of 0.128 M HCl is needed to completely neutralize 2.87 g of Mg(OH)₂?
1042
views
3. Chemical Reactions
Stoichiometry
객관식
What volume of ammonia, NH3, in liters at STP can be produced from 2.0 kg of hydrogen gas, H2, and an excess of nitrogen gas, N2? (N2 (g) + 3 H2 (g) → 2 NH3 (g))
A
74.6 L
B
22.4 L
C
149.2 L
D
44.8 L
검증된 단계별 안내1
First, convert the mass of hydrogen gas (H2) from kilograms to grams. Since 1 kg = 1000 g, multiply 2.0 kg by 1000 to get 2000 g of H2.
Next, calculate the number of moles of hydrogen gas using its molar mass. The molar mass of H2 is approximately 2.02 g/mol. Use the formula: \( \text{moles of H2} = \frac{\text{mass of H2}}{\text{molar mass of H2}} \).
Using the balanced chemical equation \( \text{N}_2 (g) + 3 \text{H}_2 (g) \rightarrow 2 \text{NH}_3 (g) \), determine the mole ratio between H2 and NH3. From the equation, 3 moles of H2 produce 2 moles of NH3.
Calculate the moles of NH3 produced using the mole ratio. Use the formula: \( \text{moles of NH3} = \frac{2}{3} \times \text{moles of H2} \).
Finally, convert the moles of NH3 to volume at STP (Standard Temperature and Pressure). At STP, 1 mole of any gas occupies 22.4 liters. Use the formula: \( \text{volume of NH3} = \text{moles of NH3} \times 22.4 \text{ L/mol} \).
관련 영상
관련 실천
