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A sample of gas in a 32.1 L container is initially at 15°C and 667 mmHg. If the pressure is reduced to 427 mmHg and the temperature is increased to 81°C, what is the final volume? Add 273 to convert to Kelvin. Report your answer in liters to three significant figures.
Expert Answer
This is ideal gas law ratios, we can relate 2 states via:
P1V1/T1 = P2V2/T2
since the ratios are kept
we need absolute pressure, temperature and volume
so
V1 = 32.1 L, T1 = 15 C = 15+ 273 K = 288 K, P1 = 667 mm Hg
V2 = X L, T2 = 81 C = 81 + 273 K = 354 K, P2 = 427 mm Hg
substitute
32.1*667/288 = 427*V2/354
V2 = 32.1*667/288 * 354 / 427
V2 = 61.63306 L
3 sig fig = 61.6 liters
