(D) For an ideal gas mixture, the final temperature $T$ is given by the conservation of internal energy. Since both gases are monoatomic, the molar he

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(D) For an ideal gas mixture, the final temperature $T$ is given by the conservation of internal energy. Since both gases are monoatomic, the molar heat capacity at constant volume $C_V$ is the same for both.The formula for the final temperature is:$T = \frac{n_1 T_1 + n_2 T_2}{n_1 + n_2}$Given:$n_1 = 4 \,mol$, $T_1 = 400 \,K$$n_2 = 2 \,mol$, $T_2 = 700 \,K$Substituting the values:$T = \frac{4(400) + 2(700)}{4 + 2}$$T = \frac{1600 + 1400}{6}$$T = \frac{3000}{6}$$T = 500 \,K$

Class 11 Physics Kinetic Theory of Gases Mixture of Gases

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If $4$ moles of an ideal monoatomic gas at temperature $400 \,K$ is mixed with $2$ moles of another ideal monoatomic gas at temperature $700 \,K$, the temperature of the mixture is:

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A
$550^{\circ} C$
B
$5000^{\circ} C$
C
$550 \,K$
D
$500 \,K$

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Kinetic Theory of Gases

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Mixture of Gases

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If $4$ moles of an ideal monoatomic gas at temperature $400 \,K$ is mixed with $2$ moles of another ideal monoatomic gas at temperature $700 \,K$, the temperature of the mixture is:

Similar Questions

If $\alpha$ moles of a monoatomic gas are mixed with $\beta$ moles of a polyatomic gas and the mixture behaves like a diatomic gas,then [neglect the vibrational mode of freedom]:

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