Let the concentration of both. The given reaction is:
It is given that the value of equilibrium constant, .
Now we can write the expression for equilibrium as:
Therefore, at equilibrium,
Q: 20. One of the reactions that takes place in producing steel from iron ore is the reduction of iron (II) oxide by carbon monoxide to give iron metal and
What are the equilibrium partial pressures of and at 1050 K if the initial partial
For the given reaction,
It is given that
Since , the reaction will proceed in the backward direction.
Therefore, we can say that the pressure of CO will increase while the pressure of will decrease
Now, let the increases in pressure of in pressure of be p. Then we can write,
Therefore, equilibrium partial of
And, equilibrium partial pressure of
Q: 21. Equilibrium constant, for the reaction
at 500 K is 0.061.
At a particular time, the analysis shows that composition of the reaction mixture is . Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?
The given reaction is:
Now, we know that,
It is given that.
Since the reaction is not at equilibrium.
Since, the reaction will proceed in the forward direction to reach equilibrium.