For adiabatic processes "pV^{\\gamma}=\\text{const}" . Here "\\gamma=1.4" , therefore for initial and final conditions
"p_1V_1^{\\gamma} = p_2V_2^{\\gamma}" . We know that "V_2 = 3V_1," therefore
"p_2 = p_1 \\left(\\dfrac{V_1}{V_2} \\right)^{\\gamma} = p_1 \\left(\\dfrac13 \\right)^{\\gamma} ." Standard temperature and pressure imply the temperature "T=273.15\\,\\mathrm{K}, p = 10^5\\,\\mathrm{Pa}." So "p_1 = 10^5\\,\\mathrm{Pa}" and
"p_2 = 10^5\\,\\mathrm{Pa}\\cdot \\left(\\dfrac13 \\right)^{1.4} \\approx 2.15 \\cdot10^4\\,\\mathrm{Pa}."
According to the ideal gas law,
"p_1V_1 = \\nu RT_1, \\; p_2V_2 = \\nu RT_2," so
"\\dfrac{p_2V_2}{p_1V_1} = \\dfrac{T_2}{T_1}, \\;\\; T_2 = T_1 \\cdot \\dfrac{p_2V_2}{p_1V_1} = 273.15\\cdot \\dfrac{2.15\\cdot10^4\\,\\mathrm{Pa}\\cdot3}{10^5\\,\\mathrm{Pa}} = 176\\,\\mathrm{K}."
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