A sample of helium gas initially at 37.0°C,785 torr and was heated to 58.0°C while the volume expanded to .What is the final pressure in atm?

Question

A sample of helium gas initially at 37.0°C,785 torr and  was heated to 58.0°C while the volume expanded to  .What is the final pressure in atm?

Quizplus · Accepted Answer

We can use the combined gas law to solve for the final pressure:
(P1)(V1)/(T1) = (P2)(V2)/(T2)
Converting the initial and final temperatures to Kelvin:
T1 = 37.0°C + 273.15 = 310.15 K
T2 = 58.0°C + 273.15 = 331.15 K
Plugging in the values:
(785 torr)(11.671 L)/(310.15 K) = (P2)(14.794 L)/(331.15 K)
Solving for P2:
P2 = (785 torr)(11.671 L)(331.15 K)/(14.794 L)(310.15 K) = 0.681 atm
Therefore, the final pressure is B)0.681 atm.

A Sample of Helium Gas Initially at 37