Question

If 3.00 moles of gas in a container has a volume of 60. L and at a temperature of 400. K, what is the pressure inside the container?

If 1.9 moles of a gas are held in a container at 5.00 atm and 4.8x10³ mL, what is the temperature of the gas?

What is the mass of 72.6 L of hydrogen gas held at a temperature of -48.0°C and a pressure of 680.4 mm Hg?

Answer 1

Question 1

PV= nRT

where:

P s the pressure of the gas, V is the volume of the gas,

n is the amount of substance of gas (in moles),

R is gas constant, T is the absolute temperature of the gas.

P = ? V = 60 L , n = 3 , R = 0.0821 L atm K-1 Mol-1, T = 400 K

Substitute in the equation and find P

P x 60 = 3 x 0.0821 x 400

P = 1.642 atm

Question 2

P = 5 atm V = 4.8x103 mL or 4.8 L , n = 1.9 , R = 0.0821 L atm K-1 Mol-1 , T = ?

Substitute in the equation and find T

5 x 4.8 = 1.9 x 0.0821 x T

T = 153.85 K

Question 3

P = 680.4 mmHg or 0.8952 atm V = 72.6 4.8 L , n = ? , R = 0.0821 L atm K-1 Mol-1 , T = 225 K

Substitute in the equation and find n

0.8952 x 72.6 = n x 0.0821 x 225

n = 3.518 Moles

The mass of 72.6 L of hydrogen gas = 3.518 x 2.016 = 7.09 gm