a. Using ideal gas law, find the pressure of CH4 and CO2:
"P_1=\\frac{n_1RT}{V}=\\frac{1.57\u00b78.314\u00b7(25+273)}{25\u00b710^{-3}}=155670\\text{ Pa}, \\\\\\space\\\\\nP_2=\\frac{n_2RT}{V}=\\frac{0.87\u00b78.314\u00b7(25+273)}{25\u00b710^{-3}}=86263\\text{ Pa}," the total pressure can be found by Dalton's law:
"P=P_1+P_2=241933\\text{ Pa}."
b. Repeat the procedures from (a):
"P_1=\\frac{n_1RT}{V}=\\frac{2.63\u00b78.314\u00b7(25+273)}{25\u00b710^{-3}}=260772\\text{ Pa}, \\\\\\space\\\\\nP_2=\\frac{n_2RT}{V}=\\frac{1.24\u00b78.314\u00b7(25+273)}{25\u00b710^{-3}}=122949\\text{ Pa}, \\\\\\space\\\\\nP=P_1+P_2=383721\\text{ Pa}."
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