The temperature of a gas at -173^{circ} C is | vedclass

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(C) According to Gay-Lussac's Law,for a fixed mass of gas at constant volume,the pressure is directly proportional to its absolute temperature: $P \pr

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$-73$

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(C) According to Gay-Lussac's Law,for a fixed mass of gas at constant volume,the pressure is directly proportional to its absolute temperature: $P \propto T$.Therefore,$\frac{P_{1}}{T_{1}} = \frac{P_{2}}{T_{2}}$.Given:$P_{1} = 1 	ext{ atm}$$T_{1} = -173^{\circ} C = (-173 + 273) K = 100 K$$P_{2} = 2 	ext{ atm}$Substituting the values:$T_{2} = \frac{P_{2} 	imes T_{1}}{P_{1}} = \frac{2 	imes 100}{1} = 200 K$.Converting back to Celsius:$t_{2} = T_{2} - 273 = 200 - 273 = -73^{\circ} C$.

The temperature of a gas at $-173^{\circ} C$ is $1 \text{ atm}$ at constant volume. Up to what temperature should the gas be heated so that the pressure becomes $2 \text{ atm}$ (in $^{\circ} C$)?

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