A gas sample at 40.0*C occupies a volume of 2.32 L. If the temperature is raised to 75*C, what will the volume be, assuming the pressure remains constant?

The final volume of the gas sample at the given condition is 2.58 L.

The given parameters:

The final volume of the gas is calculated by applying Charles law as shown below;

Thus, the final volume of the gas sample at the given condition is 2.58 L.

Learn more about Charles law here: link

2.58L

Explanation:

We must convert the temperature from °C to Kelvin temperature

T1 = 40°C = 40 + 273 = 313K

V1 = 2.32 L

T2 = 75°C = 75 + 273 = 348K

V2 = ?

V1 /T1 = V2 /T2

2.32 / 313 = V2 / 348

Cross multiply to express in linear form

313 x V2 = 2.32 x 348

Divide both side by the coefficient of V2 ie 313. We have

V2 = (2.32 x 348) /313

V2 = 2.58L

Therefore, if the temperature is raised to 75°C, the volume of the gas will be 2.58L

answer: mercury

explanation:

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa