Mustard gas, a chemical weapon used in World War II and more recently in the Middle East has been shown to have to have a therapeutic index that enables it to be used as an effective agent in the chemotherapy of Hodgkin’s disease. It can be generated according to the reaction: SCl2(g) + 2C2H4(g) ====== S(CH2CH2Cl)2(g) An evacuated 2.5-liter flask at 20.0°C is filled with 0.129 mol of SCl2 and 0.296 mol C2H4. After equilibrium is established, 0.01745 mol mustard gas is present.       What is the partial pressure of each gas at equilibrium? What is the equilibrium constant K at 20.0oC?

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Q: please highlight the correct answer

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