Chemistry

Problem

Calcium carbonate decomposes according to the equilibrium

\text{CaCO}_3(s)\;\rightleftharpoons\;\text{CaO}(s)+\text{CO}_2(g)

with

K_p = 0.083\,\text{atm}

at 850 K. A container at 850 K initially contains solid CaCO

_3

, solid CaO, and CO

_2

at a partial pressure of

0.10\,\text{atm}

. Which statement about the direction of spontaneous change is correct? a)

Q_p = 0.10\,\text{atm}

, so the reaction will shift toward products, increasing

p_{\text{CO}_2}

. b)

Q_p = 0.10\,\text{atm}

, so the reaction will shift toward reactants, decreasing

p_{\text{CO}_2}

. c) Because both solids appear in the equation,

Q_p

cannot be defined for this system. d)

Q_p = \dfrac{1}{0.10}\,\text{atm}=10\,\text{atm}

, so the reaction will shift toward reactants to reduce

Q_p