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The chlorination of methane occurs in a number of steps that result in the formation of chloromethane and hydrogen chloride. The overall reaction is 2CH4(g) 3Cl2(g) ⟶ 2CH3Cl(g) 2HCl(g) 2Cl^-(g). Suppose that a chemist combines 277 mL of methane and 957 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K. If the reaction reaches 65.7% completion, what is the total pressure in the flask? What is the partial pressure of CH4? What is the partial pressure of C
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