Import Question JSON

$\text{Hint: K is only temperature dependent.}$ $\text{Explanation:}$ $\text{Let's analyze this question carefully:}$ $\text{1. The equilibrium constant K for a reaction is a function of temperature only. It does not change with pressure, concentration, or the addition of a catalyst.}$ $\text{2. While pressure changes can shift the position of equilibrium (i.e., the relative amounts of reactants and products), they do not change the value of the equilibrium constant K itself.}$ $\text{3. When pressure increases, according to Le Chatelier's principle, the reaction will shift to favor the side with fewer moles of gas:}$ $\text{N}_2\text{(g)} + \text{3H}_2\text{(g)} \rightleftharpoons \text{2NH}_3\text{(g)}$ $\text{Left side: 4 moles of gas (1 mole of N}_2 \text{ and 3 moles of H}_2\text{)}$ $\text{Right side: 2 moles of gas (2 moles of NH}_3\text{)}$ $\text{So increasing pressure will shift the equilibrium toward the right (product side) because there are fewer moles of gas on that side. This will increase the concentration of NH}_3 \text{ and decrease the concentrations of N}_2 \text{ and H}_2\text{.}$ $\text{4. However, this shift in equilibrium does not change the value of K. The equilibrium constant K depends only on temperature.}$ $\text{Therefore, even though increasing pressure will shift the position of this equilibrium toward the products (right side), the value of the equilibrium constant K will remain the same as long as the temperature is constant.}$ $\text{The correct answer is option 1: K will remain the same.}$