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,

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

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:

$\frac{1.00L}{T_1}=\frac{1.10L}{528.0K}$

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

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