Consider the following decomposition reaction at 700 K. 2CaSO_4(s) ---> 2CaO(s)

Question

Consider the following decomposition reaction at 700 K.

2CaSO_4(s) ---> 2CaO(s) + 2SO_2(g) + O_2(g)

If K_p = 0.032 at this temperature, what will be the equilibrium overall pressure starting from pure CaSO_4(s)?

a. 0.20 bar
b. 0.40 bar
c. 0.011 bar
d. 0.22 bar
e. 0.60 bar

Show work on how you got answer. simply guessing will not receive credit.

Explanation / Answer

2CaSO_4(s) ---> 2CaO(s) + 2SO_2(g) + O_2(g) ------------------------------2X---------X Kp = (2X)^2 * X = 4 X^3 = 0.032 => X = 0.2 equilibrium overall pressure = 3X = 0.6 e) 0.6 bar

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