Calcium carbonate decomposes according to the equilibrium with at 850 K

CHEMISTRY · Single correct · A Level · Chemistry · Chemical equilibria (Le Chatelier’s principle and Kc) · Chemical equilibria (Le Chatelier’s principle and Kc)

Problem

Calcium carbonate decomposes according to the equilibrium CaCO3(s)  ⇌  CaO(s)+CO2(g)\text{CaCO}_3(s)\;\rightleftharpoons\;\text{CaO}(s)+\text{CO}_2(g) with Kp=0.083 atmK_p = 0.083\,\text{atm} at 850 K. A container at 850 K initially contains solid CaCO3_3, solid CaO, and CO2_2 at a partial pressure of 0.10 atm0.10\,\text{atm}. Which statement about the direction of spontaneous change is correct? (a) Qp=0.10 atmQ_p = 0.10\,\text{atm}, so the reaction will shift toward products, increasing pCO2p_{\text{CO}_2}. (b) Qp=0.10 atmQ_p = 0.10\,\text{atm}, so the reaction will shift toward reactants, decreasing pCO2p_{\text{CO}_2}. (c) Because both solids appear in the equation, QpQ_p cannot be defined for this system. (d) Qp=10.10 atm=10 atmQ_p = \dfrac{1}{0.10}\,\text{atm}=10\,\text{atm}, so the reaction will shift toward reactants to reduce QpQ_p.

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