The following equilibrium pressures at a certain temperature were observed for the reaction:
2NO2(g) <--> 2NO(g) + O2(g)
PNO2 = 0.55 atm
PNO = 6.5 x 10-5 atm
PO2 = 4.5 x 10-5 atm
Calculate the value for the equilibrium constant kp at this temperature.
At 327°C, the equilibrium concentration are:
[CH3OH] = 0.15 M
[CO] = 0.24 M
[H2] = 1.1 M
for the reaction: CH3OH(g) <--> CO(g) + 2H2(g)
Calculate kp at this temperature.
In which direction will the position of the equilibrium be shifted for each of the following changes, given the reaction bellow?
2HI(g) <--> H2(g) + I2(g)
H2(g) is added.
Answer with one of the following:
Shift right, shift left, or no shift.
I2(g) is removed.
Answer with one of the following:
Shift right, shift left, or no shift.
HI(g) is removed.
Answer with one of the following:
Shift right, shift left, or no shift.
In a rigid container, some Ar(g) is added.
Answer with one of the following:
Shift right, shift left, or no shift.
The volume of the container is doubled.
Answer with one of the following:
Shift right, shift left, or no shift.
The temperature is decreased (the reaction is exothermic)
Answer with one of the following:
Shift right, shift left, or no shift.