Exercise 14.55 Consider the reaction: NiO(s)+CO(g)⇌Ni(s)+CO2(g) Kc=4000.0 at 1500 K When calculating the answer, do not round to the appropriate number of significant figures until the last calculation step.

If a mixture of solid nickel(II) oxide and 0.10000 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of CO2?

See your other post above.

To find the equilibrium concentration of CO2, you need to use the given equilibrium constant (Kc) and set up an ICE (initial, change, equilibrium) table. Here's how you can solve the problem step by step:

1. Write the balanced chemical equation for the reaction:
NiO(s) + CO(g) ⇌ Ni(s) + CO2(g)

2. Determine the initial concentrations of the reactants. In this case, you are given that the initial concentration of carbon monoxide (CO) is 0.10000 M. Because nickel(II) oxide (NiO) is a solid, it does not contribute to the equilibrium expression.

3. Set up the ICE table and let 'x' represent the change in concentration for CO2:

| NiO(s) | CO(g) | Ni(s) | CO2(g) |
---------------------------------------------------
Initial | 0 | 0.1000 | 0 | 0 |
Change | -x | -x | +x | +x |
Equilibrium | 0 - x | 0.1000 - x | x | x |

4. Write the expression for the equilibrium constant (Kc):
Kc = [Ni(s)] * [CO2(g)] / [NiO(s)] * [CO(g)]

According to the balanced equation, the stoichiometric coefficients of all the reactants and products are 1. Therefore, the equilibrium expression simplifies to:
Kc = [Ni(s)] * [CO2(g)] / [CO(g)]

Substituting the values from the ICE table, we have:
4000.0 = (x) / (0.1000 - x)

5. Solve the equation to find the value of 'x':
Rearrange the equation: 4000.0 = x / (0.1000 - x)
Cross-multiply: 4000.0 * (0.1000 - x) = x
Expand and rearrange: 400.0 - 4000.0x = x
Add 4000.0x to both sides: 4000.0x + x = 400.0
Combine like terms: 4001.0x = 400.0
Solve for 'x': x = 400.0 / 4001.0

Calculate x: x ≈ 0.09997500624

6. Calculate the equilibrium concentration of CO2:
From the ICE table: [CO2(g)] = x

Substitute the value of 'x':
[CO2(g)] ≈ 0.09997500624 M

So, the equilibrium concentration of carbon dioxide (CO2) is approximately 0.09997500624 M.