Questions: EXERCISE Le Châtelier's Principle: Summary I Kp for the following reaction is 0.16 at 25°C. 2 NOBr(g) ⇌ 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is +16.1 kJ. Predict the effect of increasing the container volume on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change). - shift left - shift right - no change

EXERCISE Le Châtelier's Principle: Summary I
Kp for the following reaction is 0.16 at 25°C.
2 NOBr(g) ⇌ 2 NO(g) + Br2(g)

The enthalpy change for the reaction at standard conditions is +16.1 kJ. Predict the effect of increasing the container volume on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change).
- shift left
- shift right
- no change

Transcript text: EXERCISE Le Châtelier's Principle: Summary I $\mathrm{K}_{\mathrm{p}}$ for the following reaction is 0.16 at $25^{\circ} \mathrm{C}$. \[ 2 \mathrm{NOBr}(\mathrm{~g}) \rightleftarrows 2 \mathrm{NO}(\mathrm{~g})+\mathrm{Br}_{2}(\mathrm{~g}) \] The enthalpy change for the reaction at standard conditions is +16.1 kJ . Predict the effect of increasing the container volume on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change). shift left shift right no change Check Next (4 of 4 ) Show Approach

Solution

Solution Steps

Step 1: Identify the Reaction and Given Data

We are given the reaction: \[ 2 \mathrm{NOBr}(\mathrm{~g}) \rightleftarrows 2 \mathrm{NO}(\mathrm{~g}) + \mathrm{Br}_{2}(\mathrm{~g}) \] with an equilibrium constant $\mathrm{K}_{\mathrm{p}} = 0.16$ at $25^{\circ} \mathrm{C}$ and an enthalpy change $\Delta H = +16.1 \, \text{kJ}$.

Step 2: Understand the Effect of Volume Change on Equilibrium

According to Le Châtelier's Principle, if the volume of the container is increased, the system will respond by shifting the equilibrium to counteract this change. Increasing the volume decreases the pressure.

Step 3: Determine the Direction of Equilibrium Shift

For a gaseous reaction, increasing the volume (decreasing the pressure) will favor the side with more moles of gas. In this reaction:

The left side (reactants) has 2 moles of $\mathrm{NOBr}$.
The right side (products) has 2 moles of $\mathrm{NO}$ and 1 mole of $\mathrm{Br}_{2}$, totaling 3 moles.

Since the right side has more moles of gas, the equilibrium will shift to the right to increase the pressure.