POST ASSESSMENT PART 1B NUMBER 27

[Phuong Tran 1G]

27. A mixture of 2.5 moles H2O and 100 g of C are placed in a 50 L container and allowed to come to equilibrium subject to the following reaction:
C(s) + H2O (g) ⇌ CO (g) + H2 (g)
The equilibrium concentration of hydrogen is found to be [H2] = 0.040 M. What is the equilibrium concentration of water, [H2O]?

A. 0.010 M

B. 2.5

C. 20

D. None of the above

How do I approach this problem?

[Isha_Maniyar_Dis2E]

You can ignore the amount of C(s), because this does not affect the equilibrium (it is a solid). First convert the moles of gaseous H2O to concentration (moles / L). This is your initial. You can then complete the ICE table accordingly.

Hope this helped!