For the reaction cal, which one of the following conditions would favour the yield of C on the basis of Le-Chatelier principle?
High pressure, high temperature
Only low temperature
High pressure, low temperature
Only low pressure
For the reaction,
the equilibrium constant, KP at 300K is 16.0. The value of KP for
8
0.25
0.125
32
In which of the following case, does the reaction go farthest to completion?
K= 102
K = 10
K = 10-2
K = 1
pH of a buffer solution decreases by 0.02 units when 0.12 g of acetic acid is added to 250 mL of a buffer solution of acetic acid and potassium acetate at 27C. The buffer capacity of the solution is
0.1
10
1
0.4
The equilibrium constant for the given reaction is 100.
What is the equilibrium constant for the reaction given below?
10
1
0.1
0.01
20 mL of 0.1 M acetic acid is mixed with 50 mL of potassium acetate. Ka of acetic acid = 1.8 x 10-5 at 27C. Calculate concentration of potassium acetate if pH of the mixture is 4.8.
0.1 M
0.04 M
0.4 M
0.02 M
The standard free energy change of a reaction is Calculate the equilibrium constant Kp in log Kp (R =8.314 JK -1mol-1 ).
20.16
2.303
2.016
13.83
Given the equilibrium system:
What change will shift the equilibrium to the right?
Decreasing the temperature
Increasing the temperature
Dissolving NaCl crystals in the equilibrium mixture
Dissolving NH4NO3 crystals in the equilibrium mixture
B.
Increasing the temperature
This is the endothermic reaction hence, increasing the temperature will shift the equilibrium to the right.
Equivalent amounts of H2 and I2, are heated in a closed vessel till equilibrium is obtained. If 80% of the hydrogen can be converted to HI, the Kc at this temperature is :
64
16
0.25
4
For the reaction the equilibrium constant KP changes with:
total pressure
catalyst
the amount H2 and I2
temperature