Determine the subtraction level of HSO4 at 45 ° C temperature and 10 atm pressure. (Given, Kp = 0.6)
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The equilibrium constant K
p
for the reaction, N
2
(g)+O
2
(g)⇋2NO(g) at 1500
o
C is 120. If N
2
and O
2
at an initial pressure of 0.25 atm each are maintained at 1500
o
C till equilibrium is established, calculate the partial pressure of N
2
,O
2
and NO in the equilibrium mixture.
Solution
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The inital partial pressures are
P
N
2
=P
O
2
=0.25 atm
P
NO
=0 atm
Let us say that x atm of nitrogen reacts with x atm of oxygen to form 2x atm of NO at equilibrium.
The equilibrium partial pressures are
P
N
2
=P
O
2
=0.25−x atm
P
NO
=2x atm
K
P
=
P
N
2
×P
O
2
P
NO
2
120=
(0.25−x)×(0.25−x)
(2x)
2
10.95=
0.25−x
2x
0.25−x=
10.95
2x
0.25−x=0.18x
0.25=1.18x
x=0.21
The equilibrium partial pressures are
P
N
2
=P
O
2
=0.25−x=0.25−0.21=0.04 atm