Assuming you have the equilibrium constant value for a given chemical equation, determine the concentration of products and reactants at equilibrium for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g); Kc = 6.0 x 10^2 at 500°C. If the initial concentration of N2 is 0.1 M and the initial concentration of H2 is 0.2 M, what is the concentration of NH3 at equilibrium?

Question

Assuming you have the equilibrium constant value for a given chemical equation, determine the concentration of products and reactants at equilibrium for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g); Kc = 6.0 x 10^2 at 500°C. If the initial concentration of N2 is 0.1 M and the initial concentration of H2 is 0.2 M, what is the concentration of N

Answer 1

To solve this problem, we will use the ICE  Initial, Change, Equilibrium  table method. First, let's set up the ICE table:``          N2 g    +   3H2 g       2NH3 g Initial:   0.1M        0.2M         0MChange:   -x          -3x          +2xEquilibrium: 0.1-x     0.2-3x       2x``Now, we can write the expression for the equilibrium constant, Kc:Kc = [NH3]^2 /  [N2] * [H2]^3 Given Kc = 6.0 x 10^2, we can substitute the equilibrium concentrations into the expression:6.0 x 10^2 =  2x ^2 /   0.1 - x  *  0.2 - 3x ^3 Now, we need to solve for x. Since this is a complex equation, we can make an assumption that x is small compared to the initial concentrations of N2 and H2. This means that 0.1 - x  0.1 and 0.2 - 3x  0.2. This simplifies the equation to:6.0 x 10^2 =  2x ^2 /  0.1 * 0.2^3 Now, we can solve for x: 2x ^2 = 6.0 x 10^2 * 0.1 * 0.2^3 2x ^2 = 6.0 x 10^2 * 0.1 * 0.008 2x ^2 = 4.82x = sqrt 4.8 2x = 2.19x = 1.095Now that we have the value of x, we can find the concentration of NH3 at equilibrium:[NH3] = 2x = 2 * 1.095 = 2.19 MSo, the concentration of NH3 at equilibrium is 2.19 M.