For gaseous reactions, if ΔH is the change in enthalpy and ΔU that in internal energy, then
A
ΔH is always greater than ΔU
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B
ΔH is always less than ΔU
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C
ΔH>ΔU only if the number of mole of the products is less than that of the reactants.
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D
ΔU<ΔH only if the number of mole of the reactants is less than that of the products.
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Solution
The correct options are CΔU<ΔH only if the number of mole of the reactants is less than that of the products. DΔH>ΔU only if the number of mole of the products is less than that of the reactants. As we know, ΔH=ΔU+ΔnRT Δn=nP−nR so ΔU<ΔH only if the number of mole of the reactants is less than that of the products. ΔH>ΔU only if the number of mole of the products is less than that of the reactants.