Question #8f2ab

1 Answer
Apr 30, 2017

The mixture is at equilibrium, so a change in volume/pressure will cause the total moles of reactants and products to change.


We can find the new pressure of the system after the volume is reduced by using the equation:

#P_1V_1 = P_2V_2#

#(1.2atm)(2.0L) = (P_2)(1.0L)#

#P_2 = ((1.2atm)(2.0L))/(1.0L)#

#P_2 = 2.4 atm#

But since CO(g) and H2(g) react to form an equilibrium, given by the formula:

#CO(g) + 2H_2(g) rarr CH_3OH(g)#

The increased pressure will cause more of the reactants to form the product, therefore reducing the pressure (because 3 mols reactant will form 1 mol product).

So the final pressure will be more than 1.2 atm but less than the predicted 2.4 atm.