Question

What is the initial temperature of a gas if the volume changed from 1.00 l to 1.10 l and the final temperature was determined to be 255.0°c? 232°c -41°c 207°c 480°c none of the above?

Answer 1

using charles law
v1/t1=v2/t2
v1=1l
v2=1.1l
t2=255+273=528
t1=?
1/t1=1.1/528
cross multiply
1.1t1=528 divide both sides by 1.1
t1=528/1.1
t1=480k or 207celcius

Answer 2

Answer : The initial temperature of gas is
`207^oC`

Explanation :

Charles's Law : It is defined as the volume of the gas is directly proportional to the temperature of the gas at constant pressure and number of moles.

`V\propto T`

or,

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

where,

`V_1` = initial volume of gas = 1.00 L

`V_2` = final volume of gas = 1.10 L

`T_1` = initial temperature of gas = ?

`T_2` = final temperature of gas =
`255.0^oC=273+255.0=528.0K`

Now put all the given values in the above equation, we get:

`(1.00L)/(T_1)=(1.10L)/(528.0K)`

`T_1=480K=480-273=207^oC`

Therefore, the initial temperature of gas is
`207^oC`