Consider the following reaction: CO(g) + 2 H2(g) ⇌...

Question

Consider the following reaction: CO(g) + 2 H₂(g) ⇌ CH₃OH(g)

An equilibrium mixture of this reaction at a certain temperature was found to have [CO] = 0.110 M , [H₂]= 0.114 M , and [CH₃OH] = 0.190 M. What is the value of the equilibrium constant (K_c) at this temperature?

Jules Bruno · Accepted Answer

We’re being asked to determine the equilibrium constant for this reaction:CO(g) + 2 H2(g) ⇌ CH3OH(g)Recall that the equilibrium constant is the ratio of the products and reactants. We use Kp when dealing with pressure and Kc when dealing with concentration:Kp=PproductsPreactants     Kc=[products][reactants]Note that solid and liquid compounds are ignored in the equilibrium expression.[readmore]Since we’re given the concentration of each compound, we use Kc. The Kc expression for the reaction is:Kc=[products][reactants]=[CH3OH][CO][H2]2Note that each concentration is raised by the stoichiometric coefficient: [CH3OH] is raised to 1, [H2] is raised to 2, and [CO] is raised to 1.We’re given the following equilibrium concentrations:[H2] = 0.114 M             [CH3OH] = 0.190 M[CO] = 0.110 MSolving for Kc:Kc=[CH3OH][CO][H2]2Kc=[0.190][0.110][0.114]2Kc = 132.91The equilibrium constant of the reaction is 132.91.

Problem: Consider the following reaction: CO(g) + 2 H2(g) ⇌ CH3OH(g)An equilibrium mixture of this reaction at a certain temperature was found to have [CO] = 0.110 M , [H2]= 0.114 M , and [CH3OH] = 0.190 M. What is the value of the equilibrium constant (Kc) at this temperature?

FREE Expert Solution

Problem Details

Problem: Consider the following reaction: CO(g) + 2 H2(g) ⇌ CH3OH(g)An equilibrium mixture of this reaction at a certain temperature was found to have [CO] = 0.110 M , [H2]= 0.114 M , and [CH3OH] = 0.190 M. What is the value of the equilibrium constant (Kc) at this temperature?

FREE Expert Solution

Problem Details

Sign up for free to watch this video!