Q1: In ammonia synthesis (N₂ + 3H₂ = 2NH₃), there is a decrease in total volume, hence to get high equilibrium conversion, the reaction should be carried out at

ANS:B - high pressure.

In the ammonia synthesis reaction 𝑁2+3𝐻2→2𝑁𝐻3N2​+3H2​→2NH3​, the total volume of the products is less than the total volume of the reactants. This indicates that the reaction results in a decrease in total volume. According to Le Chatelier's principle, if a reaction results in a decrease in total volume, increasing the pressure will favor the side of the reaction with fewer moles of gas. In this case, the reactants side has fewer moles of gas (1 mole of nitrogen and 3 moles of hydrogen), while the products side has more moles of gas (2 moles of ammonia). Therefore, increasing the pressure will favor the formation of ammonia. So, to achieve a high equilibrium conversion of ammonia, the reaction should be carried out at high pressure. This helps shift the equilibrium towards the products side, increasing the yield of ammonia. Conversely, carrying out the reaction at low pressure would result in lower conversion of reactants to products, as it would favor the side with fewer moles of gas, which is the reactants side. Temperature also plays a role in the reaction, but in this case, the pressure effect dominates. However, the reaction typically requires a moderate temperature range, neither too low nor too high, to balance achieving a reasonable rate of reaction with maximizing the yield of ammonia. Therefore, "very high temperature" would not be the optimal condition for achieving high equilibrium conversion.