Respuesta :
This is an incomplete question, here is the complete question.
The solid XY decomposes into gaseous X and Y:
[tex]XY(s)\rightleftharpoons X(g)+Y(g)[/tex] Kp = 4.1 (at 0°C)
If the reaction is carried out in a 1 L container, which initial amounts of X and Y will result in the formation of solid XY?
a) 5 mol X; 0.5 mol Y
b) 2.0 mol X; 2.0 mol Y
c) 1 mol X; 1 mol Y
d) All of the above
Answer : The correct option is, (D)
Explanation :
Reaction quotient (Q) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.
The given balanced chemical reaction is,
[tex]XY(s)\rightleftharpoons X(g)+Y(g)[/tex]
The expression for reaction quotient will be :
[tex]Q=[X][Y][/tex]
In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.
The given equilibrium constant value is, [tex]K_p=4.1[/tex]
Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.
If the initial amount of X and Y to form XY then the product of their product must be greater than Kp.
Now we have to calculate the product of partial pressure.
PV = nRT
[tex]P=\frac{nRT}{V}[/tex]
Moles of X Moles of Y Pressure of X Pressure of Y Q
5.0 0.5 112.1 11.2 1255.52
2 2 44.8 44.8 89.6
1 1 22.4 22.4 44.8
There are 3 conditions:
When [tex]Q>K_c[/tex] that means product > reactant. So, the reaction is reactant favored.
When [tex]Q<K_c[/tex] that means reactant > product. So, the reaction is product favored.
When [tex]Q=K_c[/tex] that means product = reactant. So, the reaction is in equilibrium.
From the above we conclude that, in all the three options [tex]Q>K_c[/tex] that means product > reactant. So, the reaction is reactant favored that means reaction must shift to the reactant (left) to be in equilibrium.
Hence, the correct option is, (D)
