An average incandescent light bulb with a volume of 0.130 L contains 0.216 grams of argon gas. After the bulb had been burning for a few minutes, the temperature of the gas reached 100 °C.

What was the pressure of the gas at that temperature?

1.2 atm

4.01 atm

1.37 atm

0.23 atm

3.08 atm

P = 1.2 atm

Explanation:

Given dа ta:

Volume = 0.130 L

Mass of argon = 0.216 g

Temperature = 100°C (273+100 = 373K)

Pressure = ?

Solution:

Number of moles of argon:

Number of moles = mass / molar mass

Number of moles = 0.216 g / 40 g/mol

Number of moles = 0.005 mol

Pressure of argon:

PV = nRT

P = nRT/V

P = 0.005 mol * 0.0821 atm. L/mol. k * 373 k / 0.130 L

P = 0.15l * atm / 0.130 L

P = 1.2 atm