Question

A sample of 2.0 moles of helium gas is contained in a tank with a volume of 5.0L at a temperature of 25°C. What is the pressure of the gas in the tank

in atm?
Given: R = 0.0821 L.atm/mol.K
O 9.8 atm
O 0.00069 atm
O 0.82 atm
O 0.0082 atm

Answer 1

Answer: Pressure of the gas in the tank is 9.8 atm.

Step-by-step explanation:

Given: Moles = 2.0 moles, Volume = 5.0 L

Temperature =
`25^(o)C = (25 + 273) K = 298 K`

Formula used to calculate pressure is as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

`PV = nRT\\P * 5.0 L = 2.0 mol * 0.0821 L atm/mol K * 298 K\\P = (2.0 mol * 0.0821 L atm/mol K * 298 K)/(5.0 L)\\= 9.8 atm`

Thus, we can conclude that pressure of the gas in the tank is 9.8 atm.