Gaseous NH3 is placed in a closed container at 33 °C, where it partially decomposes to N₂ and H₂: 2 NH3(g) = 1 N₂(g) + 3 H₂(g) At equilibrium it is found that p(NH3) = 0.008450 atm, p(N₂) = 0.007140 atm, and p(H₂) = 0.003440 atm. What is the value of Kp at this temperature? Kp =

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**Equilibrium Reaction and Calculation of \( K_p \):**

Gaseous \(\text{NH}_3\) is placed in a closed container at **33 °C**, where it partially decomposes to \(\text{N}_2\) and \(\text{H}_2\), according to the following equilibrium reaction:

\[ 2 \text{NH}_3(g) \rightleftharpoons 1 \text{N}_2(g) + 3 \text{H}_2(g) \]

At equilibrium, the partial pressures are measured as follows:

- \( p(\text{NH}_3) = 0.008450\) atm,
- \( p(\text{N}_2) = 0.007140\) atm,
- \( p(\text{H}_2) = 0.003440\) atm.

**Objective:**

Determine the value of \( K_p \) for this reaction at 33 °C.

**Calculation:**

The equilibrium constant \( K_p \) for the reaction is expressed as:

\[
K_p = \frac{(p(\text{N}_2) \times (p(\text{H}_2))^3)}{(p(\text{NH}_3))^2}
\]

Insert the given partial pressures into the expression to find \( K_p \).

\[ K_p = \frac{(0.007140) \times (0.003440)^3}{(0.008450)^2} \]

**Note to Educators:**

Ensure students are aware that the units for partial pressures must be consistent when calculating \( K_p \). This exercise is useful for reinforcing concepts of chemical equilibrium and the use of equilibrium constants in gaseous reactions.
Transcribed Image Text:**Equilibrium Reaction and Calculation of \( K_p \):** Gaseous \(\text{NH}_3\) is placed in a closed container at **33 °C**, where it partially decomposes to \(\text{N}_2\) and \(\text{H}_2\), according to the following equilibrium reaction: \[ 2 \text{NH}_3(g) \rightleftharpoons 1 \text{N}_2(g) + 3 \text{H}_2(g) \] At equilibrium, the partial pressures are measured as follows: - \( p(\text{NH}_3) = 0.008450\) atm, - \( p(\text{N}_2) = 0.007140\) atm, - \( p(\text{H}_2) = 0.003440\) atm. **Objective:** Determine the value of \( K_p \) for this reaction at 33 °C. **Calculation:** The equilibrium constant \( K_p \) for the reaction is expressed as: \[ K_p = \frac{(p(\text{N}_2) \times (p(\text{H}_2))^3)}{(p(\text{NH}_3))^2} \] Insert the given partial pressures into the expression to find \( K_p \). \[ K_p = \frac{(0.007140) \times (0.003440)^3}{(0.008450)^2} \] **Note to Educators:** Ensure students are aware that the units for partial pressures must be consistent when calculating \( K_p \). This exercise is useful for reinforcing concepts of chemical equilibrium and the use of equilibrium constants in gaseous reactions.
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