Question

A 4.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C?

Answer 1

Answer: 1.05 atm

Explanation: 1.05 atm i know because i got it right

Answer 2

Based on the ideal gas equation, the final pressure of the gas is 1.05 atm.

What is the total pressure of the gas?

Moles of initial gas is calculated from the formula of the ideal gas equation:

• n = PV/RT

Where:

• R = 0.082 L.atm/K.mol
• T = 25°C = 298 K
• P = 1.00 atm
• V = 4.00 L

Then:

n = 1 × 4/0.082 × 298

n = 0.164 moles

Moles of added gas = mass/molar mass

molar mass of N2 = 28 g

Moles of added gas = 2/28

Moles of added gas = 0.0714

Total moles of gas = 0.235 moles

New temperature of gas = -55°C = 218 K

using the ideal gas equation, the final pressure, P, is calculated as follows:

P = nRT/V

P = 0.235 × 0.082 × 218/4

P = 1.05 atm.

Therefore, the final pressure of the gas is 1.05 atm.

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