STATEMENT-1: The total translational kinetic | vedclass

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(B) For an ideal gas,the total translational kinetic energy $(K)$ is given by the formula $K = \frac{3}{2} nRT$.From the ideal gas equation,we know th

Vedclass · Accepted Answer

$STATEMENT-1$ is True,$STATEMENT-2$ is True; $STATEMENT-2$ is $NOT$ a correct explanation for $STATEMENT-1$.

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(B) For an ideal gas,the total translational kinetic energy $(K)$ is given by the formula $K = \frac{3}{2} nRT$.From the ideal gas equation,we know that $PV = nRT$.Substituting $nRT$ with $PV$,we get $K = \frac{3}{2} PV = 1.5 PV$.Thus,$STATEMENT-1$ is True.$STATEMENT-2$ describes the nature of molecular collisions in a gas,which is a fundamental postulate of the Kinetic Theory of Gases,but it does not explain why the kinetic energy is related to $PV$ in the specific ratio of $1.5$. Therefore,$STATEMENT-2$ is True but is not the correct explanation for $STATEMENT-1$.

$STATEMENT-1$: The total translational kinetic energy of all the molecules of a given mass of an ideal gas is $1.5$ times the product of its pressure and its volume. Because
$STATEMENT-2$: The molecules of a gas collide with each other and the velocities of the molecules change due to the collision.

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$STATEMENT-1$: The total translational kinetic energy of all the molecules of a given mass of an ideal gas is $1.5$ times the product of its pressure and its volume. Because$STATEMENT-2$: The molecules of a gas collide with each other and the velocities of the molecules change due to the collision.