A sample of helium gas has a temperature of 298 K and a pressure of 3.60 atm, under a constant volume. What is the new temperature, if the pressure is increased to 3.80 atm?
PV = nRT
At constant volume, P = T
P1/P2 = T1/T2
3.60 atm / 3.80 atm = 298 K / T2
0.9474 = 298 / T2
T2 = 298 / 0.9474 = 314.5 K
Therefore, new temperature = 314.5 K
A sample of helium gas has a temperature of 298 K and a pressure of 3.60...
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