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:
▪ 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:
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 ofGiven that K p = 1.5 x 10 -4 for the reaction 2 CO(g) <=&...as high difficulty.