For the following reaction the initial concentrations are [CO2] = 0.291 M, [HCl] = 0.746 M, [CCl4] = 0.358 M, and [H2O] = 0.802 M. The equilibrium concentration of HCl is 0.573 M. Calculate the equilibrium constant for the reaction.   CO2(g) + 4HCl(g) ----- CCl4(g) + 2 H2O (g)

Calculate the equilibrium concentrations for all reactants and products if initial concentrations of CH4 is 0.400 M, H2S is 0.800 M, CS2 is 0.400 M, H2 is 0.800 M are mixed and allowed to establish equilibrium.  The Kc for the reaction is 0.0360 and the equilibrium concentration of CH4is 0.556 M.   CH4(g) + 2H2S(g) ↔  CS2(g) + 4H2(g) Group of answer choices [CH4] = 0.556 M, [H2S] = 0.488 M, [CS2] = 0.556 M, [H2] = 1.42 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.244 M, [H2] = 0.176 M. [CH4] = 0.556 M, [H2S] = 0.244 M, [CS2] = 0.956 M, [H2] = 1.36 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.556 M, [H2] = 1.42 M.

Write the pressure equilibrium constant expression for this reaction.  2CH3OH(l)+3Os(g) --> 2CO2(g)+4H2O(g)

The equilibrium constant, K, for the following reaction is 1.29x10-2 at 600 K. COC,(g) CO(g) + Cl2(g) + C2(g) Calculate the equilibrium concentrations of reactant and products when 0.262 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COCI,] = [CO] [Ch] MMM

The equilibrium constant, K, for the following reaction is 6.59×10-2 at 546 K. PCl5 (g)  PCl3 (g) +  Cl2 (g) An equilibrium mixture of the three gases in a 6.59 L container at 546 K contains 0.254 M PCl5,   0.129 M PCl3 and 0.129 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.7 L?

At 2000°C the equilibrium constant for the reaction is Kc = 2.4 x 10³. 2 NO(g) = N₂(g) + O₂(g) If the initial concentration of NO is 0.100 M, what are the equilibrium concentrations of NO, N₂, and O₂? [0₂] 0.049 [N₂] 0.049 [NO] 0.002 M M X M

The equilibrium constant, K, for the following reaction is 3.92×10-2 at 531 K.PCl5(g) PCl3(g) + Cl2(g)An equilibrium mixture of the three gases in a 7.63 L container at 531 K contains 0.331 M PCl5,   0.114 M PCl3 and 0.114 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 18.0 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M     Submit Answer

For the reaction   2H2O(g)↽−−⇀2H2(g)+O2(g)   the equilibrium concentrations were found to be [H2O]=0.250 M, [H2]=0.590 M, and [O2]=0.750 M. What is the equilibrium constant for this reaction? Kc=

CO2(g) + H2(g) « H2O(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000 K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured.                                      [H2]  = 0.20 mol/L                                   [CO2]  = 0.30 mol/L                      [H2O] = [CO]  = 0.55 mol/L (a)   What is the mole fraction of CO(g) in the equilibrium mixture? (b)   Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constant for the reaction. (c)   Determine Kp in terms of Kc for this system. (d)   When the system is cooled from 2,000 K to a lower temperature, 30.0 percent of the CO(g) is converted back to CO2(g). Calculate the value of Kc at this lower temperature. (e)   In a different experiment, 0.50 mole of H2(g) is mixed with 0.50 mole of CO2(g) in a 3.0-liter reaction vessel at 2,000 K. Calculate the equilibrium concentration, in moles per liter, of CO(g) at this…