A quantity of gas occupies a certain volume when the temperature is -73oC and the pressure is 1.5 atmospheres. If the pressure is increased to 4.5 atmospheres and the volume is halved at the same time, what will be the new temperature of the gas?
General Gas Law:
\(\frac{P_1 V_1}{T_1}\) = \(\frac{P_2 V_2}{T_2}\)
where T\(_1\) = -73 + 273 = 200k, T\(_2\) = ?,
V\(_1\) = 1, V\(_2\) = \(\frac{1}{2V}\),
P\(_1\) = 1.5, P\(_2\) = 4.5
T\(_2\) = \(\frac{P_2 V_2 T_1}{P_1 V_1}\)
T\(_2\) = \(\frac{4.5 * 1/2 * 200}{1.5 X 1}\)
T\(_2\) → 300k or 27ºC
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