If reaction C = D is at equilibrium with PC=0.5 atm and PD=1.0 atm, then PC is increased to 1.0 atm while PD remains the same. What is the new equilibrium partial pressure of D?
A. 0.67 atm
B. 1.00 atm
C. 1.33 atm
D. 1.67 atm
consider the reaction
C ---> D
Kp = ( pD / pC)
given
pD = 1 , pC = 0.5
so
Kp = 1 / 0.5
Kp = 2
now
C ---> D
now partial pressure of C is icreased to 1 atm
now
using ICE table
initial pressure of C , D are 1 , 1
change in pressure of C , D are -x , +x
equilibrium pressure of C , D are 1-x , 1 + x
now
Kp = (pD) / (pC)
2 = (1+x) / ( 1-x)
2 (1-x) = 1 + x
2 - 2x = 1 + x
1 = 3x
x = 1/3 = 0.333
now
pD = 1 + x = 1 + 0.33 = 1.33 atm
so
the new equilibrium partial pressure of D is 1.33 atm
so
the answer is C) 1.33 atm
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