Question

A container of oxygen has a volume of 349 mL at a temperature of 22.0°C . What volume will the gas occupy at 50.0°C?

Answer 1

We assume a constant pressure. Thus Charles' Law applies.

Explanation:

Charles' Law states that at constant pressure, and constant amount of gas, volume is proportional to absolute temperature, i.e. `VpropT`.

So `V=kT`, where `V` = volume, `k` is some constant, and `T` is absolute temperature.

So, in each case, `V_1=kT_1, and V_2=kT_2`. If we solve for `k`, then `V_1/T_1 = V_2/T_2`.

Thus, `V_2=(V_1xxT_2)/T_1` `=` `(0.349*dm^3xx337cancelK)/(295cancelK)` `=` `??` `dm^3`

Note that `V_2` will be bigger (reasonably), because `T_2` has increased from `T_1`.

Answer 2

The final volume will be 382 mL.

Explanation:

Charles' law states that the volume of a given amount of a gas kept at constant pressure, is directly proportional to the temperature in Kelvins. http://chemistry.bd.psu.edu/jircitano/gases.html

The equation needed to solve this problem is `V_1/T_1=V_2/T_2`.

Given/Known
`V_1="349 mL"`
`T_1="22.0"^"o""C"+273.15="295.2 K"`
`T_2="50.0"^"o""C"+273.15="323.2 K"`

Unknown
`V_2`

Equation

`V_1/T_1=V_2/T_2`

Solution
Rearrange the equation to isolate `V_2` and solve.

`V_2=(V_1T_2)/T_1`

`V_2=(349"mL"xx323.2cancel"K")/(295.2cancel"K")="382 mL"`