At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE° ?
At constant pressure for which of the reactions shown below should ΔH° be greater than ΔE° ?
I. 2 SO2(g) + O2(g) → 2 SO3(g)
II. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l)
III. H2(g) + Cl2(g) → 2 HCl(g)
IV. N2O4(g) → 2 NO2(g)
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Think about the definition of change in enthalpy at constant pressure:
ΔH° = ΔE° + PΔV
Because P is positive, ΔH°>ΔE° when the change in volume is positive i.e. reaction IV, where 1 mole of gas becomes 2 moles of gas (for ideal gases at constant pressure and temperature, number of moles is proportional to volume)