The equilibrium constant Kc for the reaction of H2 with I2 is57.0 at 700 K : H2

Question

The equilibrium constant Kc for the reaction of H2 with I2 is57.0 at 700 K : H2 (g) + I2 (g) 2HI(g)         KC = 57.0 at700 K If 1.00 mol of H2 is allowed to react with 1.00 mol of I2 in a10.0 L reaction vessel at 700 K, what are the concentrationsof H2, I2, and HI at equilibrium? b)What is the composition of the equilibrium mixture inmoles? The equilibrium constant Kc for the reaction of H2 with I2 is57.0 at 700 K : H2 (g) + I2 (g) 2HI(g)         KC = 57.0 at700 K If 1.00 mol of H2 is allowed to react with 1.00 mol of I2 in a10.0 L reaction vessel at 700 K, what are the concentrationsof H2, I2, and HI at equilibrium? b)What is the composition of the equilibrium mixture inmoles?

Explanation / Answer

We Know that :       The given Reaction is :        H2 (g) + I2 (g) 2HI (g)   intial : 1.0    1.0          0 change : - x     -x         + 2 x equilibrium : 1.0 - x / 10 1.0 - x/ 10   2 x / 10              Kc   = ( 2 x / 10 )2  / ( 1.0 - x / 10 ) x ( 1.0 - x / 10 )               57   = ( 2 x / 10 )2  / ( 1.0 - x / 10 ) x ( 1.0 - x / 10 )           Solving the above equation for X we get :           X = 0.790 M           The Equilibrium concentration of H2   = 0.021 M             The Equilibrium concentration of I2   = 0.021M               The Equilibrium Concentration of HI = 0.158M       The Equilibrium moles of   H2   = 0.21 moles         The Equilibriummoles of I2   = 0.21 moles          THeEquilibrium moles of HI = 1.58 moles

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