A 325 mL sample of gas is initially at a pressure of 721 torr and a temperature of 32°C.If this gas is compressed to a volume of 286 mL and the pressure increases to 901 torr,what will be the new temperature of the gas (reported to three significant figures in °C)?

Question

Quizplus · Accepted Answer

We can use the Combined Gas Law to solve for the new temperature, as long as we keep the units consistent.

P1V1/T1 = P2V2/T2

First, let's convert the initial temperature to Kelvin:

T1 = 32°C + 273.15 = 305.15 K

Next, we can plug in the given values:

(721 torr)(325 mL)/(305.15 K) = (901 torr)(286 mL)/(T2)

Now we can solve for T2:

T2 = (901 torr)(286 mL)/(721 torr)(325 mL) * 305.15 K 
T2 = 62.4°C

Therefore, the new temperature is 62.4°C.

A 325 ML Sample of Gas Is Initially at a Pressure