Final answer:
The chemical reaction between N2 and H2 to form NH3 is governed by stoichiometry that uses volume ratios based on Avogadro's law. The calculated volume of NH3 gas formed would be approximately 6.67 liters, assuming complete reaction, but the problem as stated suggests 7.33 litres, which is not possible; the maximum yield is 6.67 liters. Reaction yield cannot be calculated accurately from the given information.
Step-by-step explanation:
To calculate the volume of NH3 gas formed and the reaction yield after putting 5 liters of N2 and 10 liters of H2 into a reaction vessel, we use the stoichiometry of the balanced chemical equation: N2 + 3 H2 → 2 NH3. This equation tells us that a given volume of nitrogen gas reacts with three times that volume of hydrogen gas to produce two times that volume of ammonia gas, given that pressure and temperature remain constant.
According to the problem, the total volume after the reaction is 9 liters. Because the reaction consumes the gases in a 1:3 ratio, and we started with 5 liters of N2, we would expect to use 15 liters of H2 for a complete reaction. However, only 10 liters of H2 are available, indicating that H2 is the limiting reactant. The reaction would consume all 10 liters of H2 and a corresponding 1/3 of that volume of N2 (which is 10/3 liters or approximately 3.33 liters). The remaining volume of N2 is 5 - 10/3 liters, approximately 1.67 liters.
With all the H2 reacted, we'll have formed 2 times the volume of NH3 as the N2 that has reacted, which is 2 * (10/3) or approximately 6.67 liters of NH3. Since we ended up with 9 litres of volume, and the unreacted N2 gas occupies approximately 1.67 liters, the volume of NH3 present is 9 - 1.67 liters, which is approximately 7.33 liters. This suggests that there are some unreacted gases present, possibly due to incomplete reaction or formation of side-products.
The theoretical yield of NH3 is 6.67 litres, but the actual yield is 7.33 liters, perhaps due to measurement errors or assumptions in the problem. However, the reaction yield cannot exceed the theoretical yield, which means the maximum possible yield is 6.67 liters, or 100%.