Certain amount of a gas occupies a volume of 0.4 litre at $17^{o} C$ . To what temperature should it be heated so that its volume gets (a) doubled (b) reduced to half, pressure remaining constant.

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Solution

(a) $\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}}$ by Charles law
$\frac{0.4}{273 + 17}$ Kelvin= $\frac{0.8}{T_{2}}$
$T_{2} = 300 \times 2$
$T_{2} = 600$ Kelvin
$T_{2} = 600 - 273$
$T_{2} = 327^{0} C$

(b) $\frac{0.4}{300} = \frac{0.2}{T_{2}}$
$T_{2} = \frac{300}{2}$
$T_{2} = 150$ Kelvin
$T_{2} = 150 - 273$
$T_{2} = - 123^{0} C$

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Certain amount of a gas occupies a volume of 0.4 litre at 17oC. To what temperature should it be heated so that its volume gets (a) doubled (b) reduced to half, pressure remaining constant.

(a)V1T1=V2T2 by Charles law0.4273+17 Kelvin=0.8T2T2=300×2T2=600 KelvinT2=600−273T2=3270C(b)0.4300=0.2T2T2=3002T2=150 KelvinT2=150−273T2=−1230C

Certain amount of a gas occupies a volume of 0.4 litre at $17^{o} C$ . To what temperature should it be heated so that its volume gets (a) doubled (b) reduced to half, pressure remaining constant.