Question

What is the pressure exerted by 1.2 mol of a gas with a temperature of 20°C and a volume of 9.5 L?

Answer 1

Answer:

The pressure exerted by 1.2 mol of a gas at given condition is 3.03 atm.

Explanation:

Moles of gases = n = 1.2 mol

Pressure of the gas = p

Volume occupied by the gas = 9.5 L

Temperature of the gas = 20 °C = 293 K

Using ideal gaseqaution:

$PV=nRT$

$P=\frac{nRT}{V}=\frac{1.2 mol\times 0.0820 atm L/mol K\times 293 K}{9.5 L}=3.03 atm$

The pressure exerted by 1.2 mol of a gas at given condition is 3.03 atm.

Answer 2

The pressure exerted by 1.2 mol of a gas at given condition is 3.03 atm.

Explanation:

Moles of gases = n = 1.2 mol

Pressure of the gas = p

Volume occupied by the gas = 9.5 L

Temperature of the gas = 20 °C = 293 K

Using ideal gaseqaution:

PV=nRTPV=nRT

P=\frac{nRT}{V}=\frac{1.2 mol\times 0.0820 atm L/mol K\times 293 K}{9.5 L}=3.03 atmP=

V

nRT

=

9.5L

1.2mol×0.0820atmL/molK×293K

=3.03atm

The pressure exerted by 1.2 mol of a gas at given condition is 3.03 atm.