Subject Test < Jote You are attempting question 3 o For the reaction N2(g) + 3H2(g) + 2NH, (8), equilibrium pressures are P. = 2.6 am, Pa = 5.6 atm, and Px; – 1.2 atm . Calculate the Gibb’s free energy of the reaction at a temperature of 298K. (A) 1.43 kJ (B) 1.43x10- J (C) 1.41x103 J (D) 4.25x10' J niswer.
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For the reaction; N
2(g)
+3H
2(g)
⇌2NH
3(g)
.
At 400 K,K
p
=41 atm
−2
. Find the value of K
p
for each of the following reactions at the same temperature:
(i) 2NH
3(g)
⇌N
2(g)
+3H
2(g)
;
(ii)
2
1
N
2(g)
+
2
3
H
2(g)
⇌NH
3(g)
;
(iii) 2N
2(g)
+6H
2(g)
⇌4NH
3(g)
.
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(i) K
p
=
[NH
3
]
2
[H
2
]
3
[N
2
]
=[
[N
2
][H
2
]
3
[NH
3
]
2
]
−1
=(41)
−1
=
41
1
=0.024 atm
2
(∵
[N
2
][H
2
]
3
[NH
3
]
2
=41)
(ii) K
p
=
[H
2
]
3/2
[N
2
]
1/2
[NH
3
]
=[
[H
2
]
3
[N
2
]
[NH
3
]
2
]
1/2
=(41)
1/2
=6.4 atm
−1
(iii) K
p
=
[N
2
]
2
[H
2
]
6
[NH
3
]
4
=[
[N
2
][H
2
]
3
[NH
3
]
2
]
2
=(41)
2
=1.681×10
3
atm
−4
.
Explanation:
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