Question

If a reaction involves only solids and liquids
which of the following is true ?
(a) ΔH < ΔE (b) ΔH = ΔE
(c)ΔH > ΔE (d)ΔH = ΔE + RTΔn

Answer 1

Answer:

b is write answered

Explanation:

ok friend

Answer 2

(b) ΔH = ΔE is true if a reaction involves only solids and liquids.

Explanation:

The change in entropy and enthalpy is given by the equation:

ΔH = ΔE + Δng.RT

Where,

Δng = Number of gaseous moles = P - R

R = Gas constant

T = Temperature

Since, the reaction involves only solids and liquids, then the number of gaseous moles is zero.

ΔH = ΔE + ((0) × R × T)

ΔH = ΔE + 0

∴ ΔH = ΔE