Question

A gas occupies .745 L at 55.9 Kelvin. At what Celsius temperature will its volume be 53.89? Assume pressure remains constant

Answer 1

`"4043.5 K"`

`"4043.5 K"-"273.15"="3770.4"^@"C"`

Explanation:

We can apply Charles law in here which states that under constant pressure V(volume) is proportional to Temperature

Therefore `V/T=(V')/(T')`

And it's sure that the question is not changing adiabatically. As we also don't know the values of specific heat.
Therefore substituting the values in the equation gives us:

`0.745/55.9=53.89/(T')`(assuming the final volume is in litre)

=> `T'= "4043.56 K"`

Answer 2

The final temperature is `"4040 K"` or `"3770"^@"C"`.

Explanation:

This is an example of Charles' law, which states that the volume of a given amount of gas held at constant pressure is directly proportional to the Kelvin temperature. This means that if the volume increases so does the temperature, and vice versa. The equation for this law is:

`V_1/T_1=V_2/T_2`

Known

`V_1="0.745 L"`

`T_1="55.9 K"`

`V_2="53.89 L"`

Unknown

`T_2`

Solution

Rearrange the equation to isolate `T_2`. Plug in the known values and solve.

`T_2=(V_2T_1)/V_1`

`T_2=(53.89"L"xx55.9"K")/(0.745"L")="4040 K"` (rounded to three significant figures)

Temperature in degrees Celsius:

Subtract `273.15` from the Kelvin temperature.

`"4040 K"-"273.15"="3770"^@"C"`