High School

Consider the following reaction at 40.°C:

\[ \text{2 NOCl(g)} \rightleftharpoons \text{2 NO(g)} + \text{Cl}_2\text{(g)} \]

ΔG° = 38.1 kJ

If 1.82 atm of NOCl are reacted in a rigid container at 40.°C, calculate the equilibrium partial pressure (in atm) of NO.

Answer :

Final answer:

To calculate the equilibrium partial pressure of NO in the given reaction, use the equilibrium constant expression and the given equilibrium constant value. Solve the equations to find the value of x, representing the change in concentration of NOCl at equilibrium, and use it to calculate the equilibrium partial pressure of NO.

Explanation:

To calculate the equilibrium partial pressure of NO in the given reaction, we need to use the equilibrium constant expression and the given equilibrium constant value. The equilibrium constant expression for this reaction is K = [NO]^2/[NOCl]^2 * [Cl2]. Using the value of the equilibrium constant (K) and the initial pressure of NOCl, we can calculate the equilibrium partial pressure of NO.

  1. First, let's calculate the initial concentration of NOCl:
  2. Initial concentration of NOCl = initial pressure of NOCl / (gas constant * temperature)
  3. Next, use the equilibrium constant expression to write the equation in terms of x:
  4. K = [2x]^2 / [(1.82 - x)^2 * (1.82 - x)]
  5. Now, solve the equation to find the value of x, which represents the change in concentration of NOCl at equilibrium:
  6. Solve the quadratic equation to find the value of x.
  7. Finally, use the value of x to calculate the equilibrium partial pressure of NO:
  8. Equilibrium partial pressure of NO = 2 * x

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