Question

How many moles of CO₂ would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equiLiBrium has been reestablished?

Answer 1

To increase carbon monoxide to 0.300 mol at equilibrium, 0.100 mol of CO₂ is needed to be added to the system, as CO and CO₂ are in a 1:1 molar ratio in the equilibrium reaction.

Step-by-step explanation:

The original question prompts for the amount of CO₂ needed to increase carbon monoxide to 0.300 mol once equilibrium has been reestablished. It is essential to understand the equilibrium reaction:

CO(g) + H₂O(g) = CO₂(g) + H₂(g).

In the original equilibrium, we have 0.20 mol of CO. To increase CO to 0.300 mol, let's consider 'x' as the change in moles of CO due to the reaction shifting towards the products:

Initial: CO(g) 0.20 mol + x
Final: CO(g) 0.300 mol

Through stoichiometry, the equilibrium reaction shows that CO and CO₂ are in a 1:1 ratio; thus for each mole of CO increased, one mole of CO₂ is consumed. Therefore, 'x' is 0.100 mol, and the system requires 0.100 mol of CO₂ to be added to shift the equilibrium and produce the additional 0.100 mol of CO needed.

In the context of equilibrium mixtures, the water vapor concentration can stay the same even though some water is removed because the system will shift to re-establish equilibrium, which involves either producing or consuming H₂O.