What can be concluded about the reaction represented below in terms of spontaneity?
Answers
Answer:
Explanation:
Answer:
The reaction is not spontaneous below 1000 °C, at equilibrium at 1000 °C, and spontaneous above 1000 °C.
Explanation:
2A + B
→
2C
Δ
H
=
89 kJ⋅mol
-1
;
Δ
S
=
0.070 kJ⋅mol
-1
K
-1
A reaction is
spontaneous if
Δ
G
<
0
at equilibrium if
Δ
G
=
0
not spontaneous if
Δ
G
>
0
Δ
G
=
Δ
H
−
T
Δ
S
Δ
H
is +, and
Δ
S
is +.
At low temperatures, the
Δ
H
term will predominate.
Δ
G
will be +, and the reaction will not be spontaneous.
At high temperatures, the
T
Δ
S
term will predominate.
Δ
G
will be negative, and the reaction will be spontaneous.
At equilibrium,
Δ
G
=
Δ
H
−
T
Δ
S
=
0
89
kJ⋅mol
-1
−
T
×
0.070
kJ⋅mol
-1
K
-1
=
0
T
=
89
0.070 K
-1
=
1271 K
=
1000 °C
The reaction is at equilibrium at 1000 °C.