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

2 Answers
May 10, 2018

"4043.5 K"4043.5 K

"4043.5 K"-"273.15"="3770.4"^@"C"4043.5 K273.15=3770.4C

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"

May 10, 2018

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"