Question

A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 ∘C. What is the final volume of the gas, in milliliters, when the pressure and temperature of the gas sample are changed to the following, if the amount of gas does not change651 mmHg and 290 K

Answer 1

Answer:

From the general gas lawa

PV/T=k---constant

Phase 1

735×1.2/385K=2.3

Phase 2

K(constant)×T/P

2.3×290/651

Volume=1.0246dm³

Answer 2

The final volume of the gas in mL that initially has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 ∘C is 772.2mL.

How to calculate volume?

The volume of the gas can be calculated as follows:

P1V1/T1 = P2V2/T2

Where;

• P1 = initial pressure = 1.2atm
• P2 = final pressure = 0.86 atm
• V1 = initial volume = 735mL
• V2 = final volume = ?
• T1 = initial temperature = 385K
• T2 = final temperature = 290K

1.2 × 735/385 = 0.86 × V2/290

2.29 = 0.00297V2

V2 = 772.2mL

Therefore, the final volume of the gas in mL that initially has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 ∘C is 772.2mL.

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