It is desired to increase the volume of $800 c m^{3}$ of a gas by $20$ % keeping the pressure constant. To what temperature should the gas be heated, if the initial temperature is $22^{\circ} C$ ?

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Solution

Applying Charles' law we get,
$\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}}$ (Temperature in Kelvin)
$\frac{800}{295} = \frac{960}{T_{2}}$
$T_{2} = 354$
$T_{2} = 354 - 273 = 81^{o} C$

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It is desired to increase the volume of 800 cm3 of a gas by 20% keeping the pressure constant. To what temperature should the gas be heated, if the initial temperature is 22∘C?

Applying Charles' law we get,V1T1=V2T2 (Temperature in Kelvin)800295=960T2T2=354T2=354−273=81 oC

It is desired to increase the volume of $800 c m^{3}$ of a gas by $20$ % keeping the pressure constant. To what temperature should the gas be heated, if the initial temperature is $22^{\circ} C$ ?

Applying Charles' law we get,
$\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}}$ (Temperature in Kelvin)
$\frac{800}{295} = \frac{960}{T_{2}}$
$T_{2} = 354$
$T_{2} = 354 - 273 = 81^{o} C$