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A sample of gas at $1.2atm$ and $27^\circ C$ is heated at constant pressure to $57^\circ C$. Its final volume is found to be$4.75L$. What was the original volume?A) $4.32$ litersB) $5.02$ litersC) $4.22$ litersD) None of these.

Last updated date: 13th Jul 2024
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Hint: We need to know that the assertion of Charles' law is as per the following: the volume (V) of a given mass of a gas, at consistent pressing factor (P), is straightforwardly relative to its temperature (T). As a numerical condition, Charles' law is composed as all things considered.
$V \propto T$
Given data contains,
The Final volume is $4.75L$
The Initial temperature is $27^\circ C$$\left( {300K} \right)$
The Final temperature is $57^\circ C$$\left( {330K} \right)$
$\dfrac{{{V_1}}}{{{T_1}}} = \dfrac{{{V_2}}}{{{T_2}}}$
Where,
${V_1}$- Initial volume
${V_2}$ -Final volume
${T_1}$-Initial temperature
${T_2}$- Final temperature
Now we can substitute the known values in formula we get,
$\Rightarrow {V_1} = \dfrac{{4.75 \times 300}}{{330}}$
On simplification we get,
$\Rightarrow {V_1} = 4.318L$
The initial volume of the solution is $4.318L$.

Thus option A is correct.