Consider the reaction. A(aq) = 2 B(aq) K = 9.80 × 10-6 at 500 K If a 2.60 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = M

A mixture initially contains AA, BB, and CC in the following concentrations: [A][A]A_1 = 0.700 MM , [B][B]B_1 = 1.15 MM , and [C][C]C_1 = 0.300 MM . The following reaction occurs and equilibrium is established: A+2B⇌CA+2B⇌C At equilibrium, [A][A]A_2 = 0.570 MM and [C][C]C_2 = 0.430 MM . Calculate the value of the equilibrium constant, KcKcK_c.

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For the reaction in a sealed container at a constant temperature,2NO(g)+Br2​(g)<--->2NOBr(g)the initial concentrations are 4.50 M NO, 4.60 M Br2, and no NOBr. At equilibrium, [NOBr] = 2.20 M.  Calculate the value of K under the reaction conditions.

6. For the reaction A S B, if K > 1, what are the relative concentrations of A and B at equilibrium?

A mixture initially contains AA, BB, and CC in the following concentrations: [A][A] = 0.300 M� , [B][B] = 0.900 M� , and [C][C] = 0.550 M� . The following reaction occurs and equilibrium is established: A+2B⇌CA+2B⇌C At equilibrium, [A][A] = 0.150 M� and [C][C] = 0.700 M� . Calculate the value of the equilibrium constant, Kc�c. Express your answer numerically. View Available Hint(s)for Part A

Consider the reaction. A(aq) 2B(aq) K=6.05 x 10-6 at 500 K If a 1.60 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? [B] = M