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:

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:

$\overline{){\mathbf{Q}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

88% (328 ratings)
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