For N2(g) + 3H2(g) <=> 2NH3(g) at constant temperature, what is the effect of increasing the pressure by decreasing the volume?
Answer and explanation
Correct answer: D. The equilibrium shifts to the right, and the value of the equilibrium constant is unchanged
- Step 1: Left side has 4 moles of gas, right side 2 moles.
- Step 2: Increasing pressure favours the side with fewer gas particles, the right.
- Step 3: Only a change in temperature changes the equilibrium constant.
Answer
shifts right, K unchanged.
Why not the others: Left is the side with more moles; K changes only with temperature; the two sides differ in moles of gas.
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