At 0°c and 760mm hg pressure, a gas occupies a volume of 100cm cube. The Kelvin temperature of the gas is increased by one - fifth while the pressure is increased one and a half times. Calculate the final volume of the gas.

80

To solve this problem, we need to use the combined gas law, which relates the initial and final states of a gas sample. The combined gas law equation is as follows:

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

Here, P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures in Kelvin.

Let's plug in the given values into the equation:

Initial pressure (P1) = 760 mmHg
Initial volume (V1) = 100 cm^3
Initial temperature (T1) = 0°C = 273 K (converting to Kelvin)

Final pressure (P2) = 1.5 * 760 mmHg = 1140 mmHg
Final temperature (T2) = (1 + 1/5) * 273 K = 327.6 K

Now we can solve for the final volume (V2):

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

(760 mmHg * 100 cm^3) / (273 K) = (1140 mmHg * V2) / (327.6 K)

Simplifying the equation:

(760 * 100) / 273 = (1140 * V2) / 327.6

(76000) / (273) = (1140 * V2) / (327.6)

V2 = (76000 * 327.6) / (1140 * 273)

V2 ≈ 91.05 cm^3

Therefore, the final volume of the gas is approximately 91.05 cm^3.

Use (P1V1/T1) = (P2V2/T2)

You have T1 = 273, make T2 1/5 larger. You have 760 for P1, make P2 1-1/2 times that.