For the gas-phase equilibrium N2O4(g) <=> 2NO2(g), the equilibrium constant K_p = 0.15 at 298 K. What is the value of K_c for this reaction? (R = 0.0821 Latm/(molK))

Answer and explanation

Correct answer: A. 6.13 * 10^(-3)

  1. Step 1: Recall relation: K_p = K_c (R T)^(Delta n_g).
  2. Step 2: Determine change in gas moles: Delta n_g = moles of product gas - moles of reactant gas = 2 - 1 = 1.
  3. Step 3: Rearrange for K_c: K_c = K_p / (R * T).
  4. Step 4: Compute R T: 0.0821 298 = 24.47.
  5. Step 5: Calculate K_c: 0.15 / 24.47 approx 6.13 * 10^(-3).
Answer
6.13 * 10^(-3).
Why not the others: '3.67' multiplies K_p by RT instead of dividing; '0.15' assumes Delta n_g = 0; '1.23 10^(-2)' uses T = 273 K.

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