Assertion (A) At 300 K, kinetic energy of 16 | vedclass

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(A) The kinetic energy $(KE)$ of $n$ moles of an ideal gas is given by $KE = \frac{3}{2} nRT$.For $16 \ g$ of methane ($CH_4$, molar mass = $16 \ g/mo

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Both $(A)$ and $(R)$ are true and $(R)$ is the correct explanation of $(A)$

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(A) The kinetic energy $(KE)$ of $n$ moles of an ideal gas is given by $KE = \frac{3}{2} nRT$.For $16 \ g$ of methane ($CH_4$, molar mass = $16 \ g/mol$), $n = \frac{16}{16} = 1 \ mol$.For $32 \ g$ of oxygen ($O_2$, molar mass = $32 \ g/mol$), $n = \frac{32}{32} = 1 \ mol$.Since both samples contain $1 \ mol$ of gas at the same temperature $(300 \ K)$, their kinetic energies are equal. Thus, $(A)$ is true.The kinetic energy of $1 \ mol$ of any ideal gas is $\frac{3}{2} RT$, which depends only on temperature. Thus, $(R)$ is true and correctly explains $(A)$.

Assertion $(A)$ At $300 \ K$, kinetic energy of $16 \ g$ of methane is equal to the kinetic energy of $32 \ g$ of oxygen.
Reason $(R)$ At constant temperature, kinetic energy of one mole of all gases is equal.

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Assertion $(A)$ At $300 \ K$, kinetic energy of $16 \ g$ of methane is equal to the kinetic energy of $32 \ g$ of oxygen.Reason $(R)$ At constant temperature, kinetic energy of one mole of all gases is equal.