[aficc]

The equilibrium constant K for the reaction C (s) + CO_2(g) <--> 2CO (g) is 1.9 at 1000 K and 0.133 at 298 K.

1. If excess C is allowed to react with 25.0 g of CO_2 in a 3.00-L flask, how many grams of CO are produced at 298 K? At 1000k?

2. What are the partial pressures of each gas at 298 K? At 1000k?

3. Would you expect K to increase or decrease if the pressure were increased at constant temperature and volume?

for 1. number of moles of co2 is 25g/44g/mol = 0.568...and then i'm just stuck here. I think once the number of moles of C is calculated... ICE chart can be used to solve the rest...

Help please

[Yggdrasil]

You don't need to calculate the number of moles of C.  Since C is a solid, you don't include it's concentration in the formula for the equilibrium constant.  Therefore,

K = [CO]²/[CO₂]

and you can use an ICE table to do the rest.