Question

The volume of a gas is 5.80L, measured at 1.00atm. What is the pressure of the gas in mmHg if the volume is changed to 9.65L ( temperature is kept constant)

Answer 1

Answer:

The new pressure is 456.76 mmHg

Explanation:

Step 1: Data given

The initial volume of the gas = 5.80 L

The initial pressure of the gas = 1.00 atm

The volume of the gas increases to 9.65 L

The temperature is kept constant

Step 2: Calculate the new pressure

P1*V1 = P2¨V2

⇒with P1 = the initial pressure of the gas = 1.00 atm

⇒with V1 = the initial volume of the gas = 5.80 L

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with V2 = the increased volume of the gas = 9.65 L

1.00 atm * 5.80 L = P2 * 9.65 L

P2 = (5.80 / 9.65)

P2 = 0.6010 atm

Step 3: Convert pressure from atm to mm Hg

0.6010 atm * 760 mmHg = 456.76 mmHg

The new pressure is 456.76 mmHg