If ∆ H is the change in enthalpy and ∆ E , the change in internal energy accompanying a gaseous reaction, then

If

∆ H

is the change in enthalpy and

∆ E,

the change in internal energy accompanying a gaseous reaction, then

$∆ H$ is always greater than $∆ E$
$∆ H < ∆ E$ only if the number of moles of the products is greater than the number of moles of the reactants
$∆ H$ is always less than $∆ E$
$∆ H < ∆ E$ only if the number of moles of products is less than the number of moles of the reactants

Solution

As

∆ H = ∆ E + ∆ n_{g} R T

If

n_{p} < n_{r}; ∆ n_{g} = n_{p} - n_{r} = - v e

Hence

∆ H < ∆ E

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Asked in: JEE-TOPICTESTS-CHEMISTRY

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