In option D difference between no of gaseous atoms on LHS and RHS is not the same. So ∆n is -2
therefore by putting ∆n to the formula ∆h=∆u +∆nRT
we get ∆h is not equal to ∆u or ∆e

ΔH and ΔE represent different types of energy changes in a chemical reaction. ΔH refers to the change in enthalpy, which is the heat energy absorbed or released during a chemical reaction at constant pressure. ΔE, on the other hand, represents the change in internal energy, which is the total energy of the system.

To determine which reaction has a ΔH ≠ ΔE, we need to compare the enthalpy change (ΔH) with the internal energy change (ΔE) for each reaction.

a) H2(g) + I2(g) → 2HI(g)
In this reaction, hydrogen gas and iodine gas react to form hydrogen iodide gas. Since this is a chemical reaction involving gases, the only significant energy change is the breaking and formation of bonds. The enthalpy change (ΔH) for this reaction is negative because energy is released when the new bonds form. The internal energy change (ΔE) is also negative because the system loses energy. Therefore, ΔH = ΔE, and this reaction does not satisfy the condition ΔH ≠ ΔE.

b) HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
This is a neutralization reaction between hydrochloric acid and sodium hydroxide, resulting in the formation of sodium chloride and water. The enthalpy change (ΔH) for this reaction is negative because energy is released when the new bonds form. The internal energy change (ΔE) is also negative because the system loses energy. Therefore, ΔH = ΔE, and this reaction does not satisfy the condition ΔH ≠ ΔE.

c) C(s) + O2(g) → CO2(g)
This reaction represents the combustion of carbon to form carbon dioxide. The enthalpy change (ΔH) for this reaction is negative because energy is released when the new bonds form. The internal energy change (ΔE) is also negative because the system loses energy. Therefore, ΔH = ΔE, and this reaction does not satisfy the condition ΔH ≠ ΔE.

d) N2(g) + 3H2(g) → 2NH3(g)
This reaction represents the synthesis of ammonia from nitrogen and hydrogen gases. The enthalpy change (ΔH) for this reaction is negative because energy is released when the new bonds form. However, the internal energy change (ΔE) is positive because the system gains energy. Therefore, ΔH ≠ ΔE, and this reaction satisfies the condition ΔH ≠ ΔE.

In conclusion, the reaction N2(g) + 3H2(g) → 2NH3(g) is the only one among the given options that satisfies the condition ΔH ≠ ΔE.