Question

For the reaction 2 NO₂(g) ⇌ 2 NO(g) + O₂(g) Kp = 1.11 × 10⁻⁵ at 200 °C. A 2.50 L vessel at 200 °C is filled with NO₂(g) at an initial pressure of 3.25 atm and allowed to come to equilibrium. What will be the pressure (in atm) of NO(g) at equilibrium?

Name: for the reaction 2 no2g 2 nog o2g kp 111 105 at 200 c a 250 l vessel at 200 c is filled with no2g at an initial pressure of 325 atm and allowed to come to equilibrium what will be the pressu 01294
Uploaded: 2024-03-11T15:30:58-08:00
Duration: 3 min 7 s
Channel: Susan Hallstrom
Description: for the reaction 2 no2g 2 nog o2g kp 111 105 at 200 c a 250 l vessel at 200 c is filled with no2g at an initial pressure of 325 atm and allowed to come to equilibrium what will be the pressu 01294

          For the reaction 2 NO₂(g) ⇌ 2 NO(g) + O₂(g) Kp = 1.11 × 10⁻⁵ at 200 °C. A 2.50 L vessel at 200 °C is filled with NO₂(g) at an initial pressure of 3.25 atm and allowed to come to equilibrium. What will be the pressure (in atm) of NO(g) at equilibrium?

Added by Stephen W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Susan Hallstrom

03/11/2024

Step 1

The reaction is: \[ 2 \text{NO}_2(g) \rightleftharpoons 2 \text{NO}(g) + \text{O}_2(g) \] The expression for \( K_p \) is: \[ K_p = \frac{P_{\text{NO}}^2 \cdot P_{\text{O}_2}}{P_{\text{NO}_2}^2} \] Show more…

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For the reaction 2 NO₂(g) ⇌ 2 NO(g) + O₂(g) Kp = 1.11 × 10⁻⁵ at 200 °C. A 2.50 L vessel at 200 °C is filled with NO₂(g) at an initial pressure of 3.25 atm and allowed to come to equilibrium. What will be the pressure (in atm) of NO(g) at equilibrium?