in the reaction C+CO2=2CO, the equilibrium pressure is 12 atm. if 50% of CO2 reacts kp for the change is
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104
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C(s) + CO2(g) --> 2CO(g)
P(total) = 12 atm
If half the CO2 reacted then CO2 is x/2 and CO is x, and Pt = 12. Then
x/2 + x = 12
1.5x = 12
x = 8
P(CO2) = 4 atm
P(CO) = 8 atm
The initial pressure of CO2 is 8 atm. When half of it reacts then 4 atm is left and the pressure of CO is twice as great, which is 8 atm.
Kp = P(CO)² / P(CO2)
Kp = 8² / 4
Kp = 16
C(s) + CO2(g) --> 2CO(g)
P(total) = 12 atm
If half the CO2 reacted then CO2 is x/2 and CO is x, and Pt = 12. Then
x/2 + x = 12
1.5x = 12
x = 8
P(CO2) = 4 atm
P(CO) = 8 atm
The initial pressure of CO2 is 8 atm. When half of it reacts then 4 atm is left and the pressure of CO is twice as great, which is 8 atm.
Kp = P(CO)² / P(CO2)
Kp = 8² / 4
Kp = 16
Answered by
15
Answer:16 atm is the answer
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