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A sample of krypton gas at a pressure of 754 mm Hg and a temperature of 44c, occupies a volume of 13.7 liters. If the gas is heated at constant pressure to a temperature of 85c, the volume of the gas sample will be ___ L.

Answer :

Therefore, the volume of the gas sample when heated to a temperature of 85°C at constant pressure will be approximately 12.03 liters.

To find the final volume of the gas sample when heated at constant pressure, we can use the combined gas law:

P1 * V1 / T1 = P2 * V2 / T2

Where:

P1 = initial pressure

V1 = initial volume

T1 = initial temperature (in Kelvin)

P2 = final pressure

V2 = final volume (unknown)

T2 = final temperature (in Kelvin)

First, let's convert the initial and final temperatures to Kelvin:

T1 = 44°C + 273.15 = 317.15 K

T2 = 85°C + 273.15 = 358.15 K

Now, we can plug in the given values into the equation:

(754 mm Hg) * (13.7 L) / (317.15 K) = P2 * V2 / (358.15 K)

Rearranging the equation to solve for V2:

V2 = (P2 * V1 * T2) / (P1 * T1)

Plugging in the known values:

V2 = (754 mm Hg * 13.7 L * 358.15 K) / (317.15 K * 1 atm)

Converting mm Hg to atm:

1 atm = 760 mm Hg

V2 = (754 mm Hg * 13.7 L * 358.15 K) / (317.15 K * 760 mm Hg)

Calculating V2:

V2 ≈ 12.03 L

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