9. A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temper

Question

9. A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temperature. The equilibrium concentrations are [N2] = 0.66 M, [H2] = 1.21 M, and [NH3] = 0.10 M. Calculate the equilibrium constant, Kc, if the reaction is represented as ( 1/2 )N2(g) + ( 3/2 )H2(g) NH3(g) Kc=

10. The equilibrium constant Kc for the reaction I2(g) 2I(g) is 3.85 × 10^5 at 725°C. Calculate Kc and KP for the equilibrium

11. Br2(g) 2Br(g) When 1.65 moles of Br2 are put in a 0.950L flask, 3.50 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Kc for the reaction. 2I(g) I2(g) at the same temperature. Kc = × 10 (Enter your answer in scientific notation.) KP =

Explanation / Answer

Given reaction is

( 1/2 )N2(g) + ( 3/2 )H2(g) NH3(g)

Kc = [NH3] /[N2]1/2[H2]3/2

Kc = 0.10/(0.66)1/2 * (1.21) 3/2

Kc = 0.10/0.33 *0.886

Kc = 0.3420

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