At a given temperature, the equilibrium constant K_c for the reaction 2 NO(g) + 2 H_2(g)...
The equilibrium constant K_c for the reaction H_2 (g) + Br_2(g) 2 HBr(g) is 2.180 times 10^6 at 730 degree C. Starting with 2.20 moles of HBr in a 21.6-L reaction vessel, calculate the concentrations of H_2, Br_2 and HBr at equilibrium. [H_2] = [Br_2] = [HBr] =
The equilibrium constant, K_c, for the following reaction is 55.6 at 698 K: H_2(g) + I_2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.351 moles of H_2 and 0.351 moles of I_2 are introduced into a 1.00 L vessel at 698 K. [H_2] = M [I_2] = M [HI] = M
For the reaction: N_2(g) + O_2(g) = 2 NO(g) K_c = 4.0 at a particular temperature. Suppose we begin an experiment by mixing 0.1 mol of N_2 and 0.1 mol of O_2 in a 1.0-liter container. What will be the concentration of NO (in mol/L) once equilibrium is reached at the given temperature? [enter number with one decimal place]
Be sure to answer all parts. The equilibrium constant K_c for the reaction H_2(g) + Br_2(g) = 2HBr(g) is 2.180 Times 10^6 at 730DegreeC. Starting with 5.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H_2, Br_2, and HBr at equilibrium. [H_2] = M [Br_2] = M [HBr] = M
The k_eq for the reaction: 2 NO(g) + 2 H_2(g) rightarrow N_2(g) + 2 H_2O(g) is 650. The concentrations at a given time were measured as NO = 0.1 M, H_2 = 0.05 M, H_2O = 0.1 M, and N_2 = 0.001 M. Is the reaction at equilibrium?
An decrease in temperature increases the reaction rate because temperature affects the equilibrium constant of the reaction a smaller fraction of the collisions have the correct orientation of molecules. the activation energy of the reaction will decrease. less collisions will have enough energy to exceed the activation energy. the activation energy of the reaction will increase. The equilibrium constant, K_p, for the reaction H_2(g) + I_2(g) doubleheadarrow 2HI(g) is 10.0 at 450 degree C. A rigid cylinder at that temperature...
Given the reactions determine the value of K_c for the reaction Consider the equilibrium In which direction will the equilibrium shit when (a) N_2O_4 is added, (b) NO: removed, (c) the pressure is increased by addition of N_2(g). (d) the volume is increased, (e) the temperature is decreased?
For the following equilibrium: N_2(g) + H_2(g) rightarrow NH_3(g) delta H= -386 kJ/mole Predict the direction the equilibrium will shift if: N_2 is added? H_2 is removed? NH_3 is added? NH_3 is removed? the volume of the container is decreased? the pressure is increased by adding Argon gas? the reaction is cooled? equal number of moles of H_2 and NH_3 are added? a catalyst is added The equilibrium constant for the following reaction is 5.0 at 400 degree C. CO_(g)...
Select the equilibrium expression, K_c, for the following reaction: CH_4(g) + 2 H_2S(g) CS)2(g) + 4 H_2(g) K_c= [H_2][CS_2I/[CH_4][H_2S] K_c = [Ch_4][H_2S]/[H_2][CS_2] K_c= [CH_4][CS_2]/[H_2]^4[H_2S]^2 K_c = [H_2]^4[CS_2]/CH_4][C_2S]^2
A 100-mL reaction vessel initially contains 2.60 X 10^-2 mol of NO and 1.30 times 10^-2 mol of H_2. At equilibrium, the concentration of NO in the vessel is 0.161 M. At equilibrium the vessel also contains N_2, H_2O, and H_2. What is the value of the equilibrium constant K_c for the following reaction? At 500degreeC, the equilibrium constant K_p for the synthesis of ammonia.