Question

What temperature does a 0.25 L cylinder containing 0.10 mol of helium gas need to be cooled in order for the pressure to be 253.25 kPa? (Given: R = 8.314 L∙kPa/K∙mol

Answer 1

is c 76.15 k

Step-by-step explanation:

Answer 2

Answer: The gas needs to be cooled down to 76.15 K

Step-by-step explanation:

To calculate the temperature of the gas, we use the equation given by ideal gas, which is:

`PV=nRT`

where,

P = Pressure of the gas = 253.25 kPa

V = Volume of the gas = 0.25 L

n = Number of moles of gas = 0.10 mol

R = Gas constant =
`8.314\text{ L kPa }K^(-1)mol^(-1)`

T = Temperature of the gas = ? K

Putting values in above equation, we get:

`253.25kPa* 0.25L=0.10mol* 8.314\text{ L kPa }K^(-1)mol^(-1)* T\\\\T=76.15K`

Hence, the gas needs to be cooled down to 76.15 K