The Reaction Quotient Video Lessons

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Problem: A 1.00 L reaction vessel contains 1.2 mol CO(g), 1.5 mol H 2(g), and 2.0 mol CH3OH(g). How will Ptotal change as the system approaches equilibrium at constant T?CO(g) + 2H2(g) ⇌ CH3OH(g)          K c = 14.5

FREE Expert Solution

We´re asked to determine the change of Ptotal as the given system approaches equilibrium at constant T.


The equilibrium reaction is:

CO(g) + 2H2(g)  CH3OH(g)          Kc = 14.5


We know that the initial amount of CO is 1.2 mol, of H2 is1.5 mol, and of CH3OH is 2.0 mol.

In a 1.00 L container, the concentration of each is:

Molarity (M)=moles of soluteLites of solutionCO=1.2 mol of CO1.00 L=1.2 M COH2=1.5 mol of H21.00 L=1.5 M H2CH3OH=2.0 mol of CH3OH1.00 L=2.0 M CH3OH



Since we have the initial concentrations of products and reactants, we calculate the reaction quotient (Q) to determine if the reaction is at equilibrium or not.


The formula for Q is:

Q=productsreactants



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Problem Details

A 1.00 L reaction vessel contains 1.2 mol CO(g), 1.5 mol H 2(g), and 2.0 mol CH3OH(g). How will Ptotal change as the system approaches equilibrium at constant T?

CO(g) + 2H2(g) ⇌ CH3OH(g)          K c = 14.5

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