Problem 1.
Let's use ideal gas law
where "R \\approx 8.314[{{\\rm{J}} \\over {{\\rm{K}} \\cdot {\\rm{mol}}}}]" - universal gas constant and "\\nu" is the amount of moles. Using this law for the first and the second state we get
Divide the second by the first
and for the pressure at the second state
Let's do the calculations using that "T[K] = T[^\\circ C] + 273.15" and "1[{\\rm{atm}}] = 760[{\\rm{torr}}]"
Problem 2.
Let's use the ideal gas law again
Methane has the chemical formula "C{H_4}" and has the molar mass "{M_{C{H_4}}} \\approx 16.043[{{\\rm{g}} \\over {{\\rm{mol}}}}]". The number of moles can be found as "\\nu = {m \\over M}" , thus
Let's do the calculations using that "1[{\\rm{mmHg}}] \\approx 133.322[{\\rm{Pa}}]"
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