The temperature of a gas is -73^{circ}C. To w | vedclass

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(B) The initial temperature $T_1 = -73^{\circ}C = (-73 + 273) K = 200 K$.The average kinetic energy of gas molecules is given by $E = \frac{3}{2} kT$,

Vedclass · Accepted Answer

$127$

Vedclass · Answer

(B) The initial temperature $T_1 = -73^{\circ}C = (-73 + 273) K = 200 K$.The average kinetic energy of gas molecules is given by $E = \frac{3}{2} kT$,which implies $E \propto T$.Therefore,$\frac{E_2}{E_1} = \frac{T_2}{T_1}$.Given that the kinetic energy is doubled,$E_2 = 2E_1$,so $\frac{2E_1}{E_1} = \frac{T_2}{200 K}$.$T_2 = 2 	imes 200 K = 400 K$.Converting back to Celsius: $T_2(^{\circ}C) = 400 - 273 = 127^{\circ}C$.

The temperature of a gas is $-73^{\circ}C$. To what temperature in $^{\circ}C$ should the gas be heated so that the average kinetic energy of its molecules becomes doubled?

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