Calculate K_c for the following reaction. The equilibrium concentrations tor NO_2 and N_2O_4 are 0.050 M and 0.057 M at 380K. 2 NO_2 (g) = N_2O_4 (g) Calculate K_p for the following reaction at 380K. 1/2 N_2 O_4 (g) = NO_2 (g) Calculate the equilibrium concentration of HF for the following reaction. At a particular temperature the value of the equilibrium constant is K = 1.6 times 10^3. The initial concentration of hydrogen and iodine are both 0.10 M. [2 sf] H_2 (g) + F_2 = 2 HF(g) Calculate the equilibrium partial pressure of product B. At a particular temperature the equilibrium constant for the conversion of A to B is K_p = 0.035 and the initial partial pressure of A is 0.50 atm.
