Consider the following reaction in a 3.5 L flask at constant temperature: CO 2 (
ID: 705743 • Letter: C
Question
Consider the following reaction in a 3.5 L flask at constant temperature:
CO2 (g) + H2 (g) ? CO (g) + H2O (g) Kp = 11
What will happen to the partial pressure of hydrogen under the following initial scenarios?
a. 1 atm of carbon dioxide and 2 atm of hydrogen
b. 3.2 atm of carbon dioxide, 0.9 atm of water and 1 atm of carbon monoxide
c. 1.4 atm of carbon dioxide, 2.5 atm of hydrogen, 0.75 atm of carbon monoxide and 5.3 atm of water
Explanation / Answer
a. only CO2,H2 is present.so that, forward reaction takes place,that results decrease in partial pressure of hydrogen
b. here CO2 and CO,H2O(g) is present, as there is no H2 available.backward reaction takes place.so that, partial pressure of hydrogen increases.
c. reaction quotient(qp) = pCO*pH2O/pCO2*pH2
= (0.75*5.3)/(1.4*2.5)
= 1.136
qp < Kp, so that, forward reaction takes place.that results decrease in partial pressure of hydrogen