Chemistry

Chemistry

Problem

At a certain temperature the equilibrium constant for the reaction 2 SO2(g)+O2(g)⇌2 SO3(g)\mathrm{2\,SO_2(g) + O_2(g) \rightleftharpoons 2\,SO_3(g)} is Kp=3.0.K_p = 3.0. An equilibrium mixture in a rigid container has PSO2=0.50 atm,  PO2=0.20 atm,  PSO3=0.40 atm.P_{\mathrm{SO_2}} = 0.50\,\text{atm},\; P_{\mathrm{O_2}} = 0.20\,\text{atm},\; P_{\mathrm{SO_3}} = 0.40\,\text{atm}. The container is then compressed to half its original volume at constant temperature. After compression and before any reaction occurs, each partial pressure doubles. What is the partial pressure of SO3\mathrm{SO_3} (in atm) after the system has re-established equilibrium at the new volume? a) 0.87 b) 1.10 c) 0.91 d) 0.95

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