ICE Chart Video Lessons

Concept:

Problem: Given that K p = 1.5 x 10 -4 for the reaction 2 CO(g) &lt;=&gt; 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 atmb. 0.0031 atmc. 0.00016 atmd. 0.0992 atme. 0.0525 atm

FREE Expert Solution

We are asked to get the equilibrium partial pressures of CO2 when 4 atm CO is initially placed in the reaction:

2 CO(g) ⇌ C(graphite) + CO2(g)

When dealing with equilibrium and Kp:

Kp → equilibrium units are in pressure
Kp is an equilibrium expression:

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

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 CO2 using an ICE chart where we have 4 atm CO initially. From this, we can construct an ICE table:

80% (255 ratings)
Problem Details

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