Gibbs Free Energy (Sections)
(i) spontanous at all temperatures; (ii) not spontaneous at any temperature; (iii) spontaneous at low T but not spontaneous at high T; (iv) spontaneous at high T but not spontaneous at low T.
Classify each of the following reactions as one of the four possible types summarized in Table:
Table How Signs ofΔH andΔS Affect Reaction Spontaneity
ΔH | ΔS | -TΔS | ΔG= ΔH- TΔS | Reaction Characteristics | Example |
- | + | - | - | Spontaneous at all temperatures | 2 O3(g)→3 O2(g) |
+ | - | + | + | Nonspontaneous at all temperatures | 3 O2(g)→2 O3(g) |
- | - | + | + or - | Spontaneous at low T; nonspontaneous at high T | H2O(l)→H2O(s) |
+ | + | - | + or - | Spontaneous at high T; nonspontaneous at low T | H2O(s)→H2O(l) |
(a) N2(g) + 3 F2(g)→2 NF3(g) ΔH° = -249 kJ; ΔS° = -278 J/K
(b) N2(g) + 3 Cl2(g)→2 NCl3(g) ΔH° = 460 kJ; ΔS° = -275 J/K
(c) N2F4(g)→2 NF2(g) ΔH° = 85 kJ; ΔS° = 198 J/K
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