Question

A gas expands from a volume of 2.00L at 36.0oC to a volume of 2.50 L, what is the final temperature, if the pressure is constant?

Answer 1

We shall consider V, the volume and T, the temperature.
According to Boyle's Laws:

`(V1)/(T1) = (V2)/(T2)`
In our case:

`(2.00)/(36.0) = (2.50)/(T2) =\ \textgreater \ T2= (2.50*36.00)/(2.00) = 45`

Answer 2

The final temperature is 45.45 Celcius

Step-by-step explanation:

The Combined Gas Law:

The combined gas law allows to derive relationships between the variable that undergoes like pressure, temperature and volume.

`(P_1V_1)/(T_1) =(P_2V_2)/(T_2)`

It is given thatpressure is constant so,

`P_1=P_2`

Hence combined gas law becomes,

`( V_1)/(T_1)=(V_2)/(T_2)`

Substituting the values given in the question,

`(2.00)/(36)=(2.50)/(T_2)`

`0.055=(2.50)/(T_2)`

`T_2=(2.50)/(0.055)`

`T_2`=45.45 C