Question

A given sample of a gas has a volume of 5.10 L at 27°C and 640 mm Hg. Its volume and temperature are changed to 2.10 L and 100°C, respectively. What is the pressure in mm Hg at these conditions?

Answer 1

`1932.50\text{ mmHg}`

Step-by-step explanation:

Here, we want to calculate the final pressure

Mathematically from the general gas equation:

`(P_1V_1)/(T_1)\text{ = }(P_2V_2)/(T_2)`

where:

P1 is the initial pressure which is 640 mmHg

V1 is the initial volume which is 5.1 L

T1 is the initial temperature (we convert this to Kelvin by adding 273: 27 + 273 = 300 K)

P2 is the final pressure which is what we want to calculate

V2 is the final volume which is 2.1 L

T2 is the final temperature (we convert to Kelvin by adding 273 K : 273 + 100 = 373 K)

Substituting the values, we have it that:

`P_2\text{ = }(P_1V_1T_2)/(T_1V_2)`

Substituting the values, we have it that:

`P_2\text{ = }\frac{640\text{ }*5.1*373}{300*2.1}\text{ = 1932.50 mmHg}`