We are asked to **get the equilibrium partial pressures of CO _{2} when 4 atm CO is initially placed in the reaction:**

**2 CO(g) ⇌ C(graphite) + CO _{2}(g)**

When dealing with equilibrium and K_{p}:

• **K _{p} **→ equilibrium units are in pressure

•

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

▪ **only aqueous and gaseous species** are included in the equilibrium expression

▪ the **coefficient** of each compound in the reaction equation will be the **exponent **of the concentrations in the equilibrium expression

We can calculate for the partial pressure of CO_{2} using an ICE chart where we have 4 atm CO initially. From this, we can construct an ICE table:

Given that K _{p} = 1.5 x 10 ^{-4} for the reaction 2 CO(g) <=> C(graphite) + CO _{2}(g), what is the partial pressure of CO _{2}(g) at equilibrium if initially 4.00 atm of CO(g) is in contact with graphite?

a. 0.0024 atm

b. 0.0031 atm

c. 0.00016 atm

d. 0.0992 atm

e. 0.0525 atm

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty of*Given that K p = 1.5 x 10 -4 for the reaction 2 CO(g) <=&...*as high difficulty.