At 298 K, for the reaction 2H + ( aq ) + 2 Br − ( aq ) + 2 NO 2 ( g ) → Br 2 ( l ) + 2 HNO 2 ( aq ) , Δ t H ° = − 61.6 kJ mol − 1 and the standard molar entropies are H + ( a q ) , 0 J mol − 1 K − 1 ; Br − ( a q ) , 82.4 J mol -1 K − 1 ; NO 2 ( g ) , 240.1 J mol − 1 K − 1 , Br 2 ( l ) , 152.2J mol- 1 K-1. Determine (a) Δ t G ° at 298 K and (b) whether the reaction proceeds spontaneously in the forward or the reverse direction when reactants and products are in their standard states.
At 298 K, for the reaction 2H + ( aq ) + 2 Br − ( aq ) + 2 NO 2 ( g ) → Br 2 ( l ) + 2 HNO 2 ( aq ) , Δ t H ° = − 61.6 kJ mol − 1 and the standard molar entropies are H + ( a q ) , 0 J mol − 1 K − 1 ; Br − ( a q ) , 82.4 J mol -1 K − 1 ; NO 2 ( g ) , 240.1 J mol − 1 K − 1 , Br 2 ( l ) , 152.2J mol- 1 K-1. Determine (a) Δ t G ° at 298 K and (b) whether the reaction proceeds spontaneously in the forward or the reverse direction when reactants and products are in their standard states.
At 298 K, for the reaction
2H
+
(
aq
)
+
2
Br
−
(
aq
)
+
2
NO
2
(
g
)
→
Br
2
(
l
)
+
2
HNO
2
(
aq
)
,
Δ
t
H
°
=
−
61.6
kJ
mol
−
1
and the standard molar entropies are
H
+
(
a
q
)
,
0
J
mol
−
1
K
−
1
;
Br
−
(
a
q
)
,
82.4
J
mol
-1
K
−
1
;
NO
2
(
g
)
,
240.1
J
mol
−
1
K
−
1
,
Br
2
(
l
)
, 152.2J mol-1K-1. Determine (a)
Δ
t
G
°
at 298 K and (b) whether the reaction proceeds spontaneously in the forward or the reverse direction when reactants and products are in their standard states.
Calculate the standard reaction entropy at 298 K when 1 mol NH3(g) is formed from its elements in their reference states.
Given ΔHrxn∘= −135 kJ, ΔS∘rxn= −263 J/K, & T= 299 K, will the reaction be spontaneous?
In the expression, S = k ln W, W is called the number of microstates. Explain clearly the meaning of the word "microstate", and why a system under a given set of conditions normally has many microstates.
Chapter 13 Solutions
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