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The difference in energy between reactants and the transition state is called

The half-life of the reaction becomes half when initial concentrations of reactants are doubled. The order of the reaction will be

Which one of the following factors does not affect the equilibrium position?

In N₂ +3H₂ ⇌ 2NH₃ the yield of the product will be minimum if

2X+Y ⇌ Z At equilibrium 0.20 mole of X, 0.45 mole of Y and 0.15 mole of Z are present, Calculate Kc

2HI_(g) ⇌ H_2(g) + I_2(g)
For the above reaction if Kc is 0.25, then Kp for
this reaction will be

A buffer is prepared by mixing the solutions of equimolar acetic acid and sodium acetate. The pH should be equal to

If the equilibrium constant KC value for a certain reaction is very small, then:

The rate of chemical reaction roughly doubles for every 10°C rise in temperature. If the temperature is raised by 20°C, the rate may increase

In a reaction 2X + Y → M + N
If the concentration is of Y kept constant and that of X is tripled. The rate of reaction will

Rate of an exothermic reaction is increased by increasing all except

For the gas phase reaction
2X+Y ⇋ 2Z  ∆H= -ive kJ/mol. The yield of Z at equilibrium could be increased by

Following is an exothermic reaction
A+ B ⇌ C+ D. Which is the correct statement

The solubility product of a salt AB is 0.25 mol²/dm⁶. What will be its solubility (mol/dm³)

Catalyst can change

One of the following is not a physical method for determination of the rate of reaction

For the first-order reaction, the half-life is related to the expression k t_1/2 = 0.693. Half-life is the 1
A. Time is taken for the conc. of the product to increase to half of its original value.

The pKa value of CH₃COOH is 4.74. The pH of an equimolar solution of acetic acid and sodium acetate is:

The rate expression of a reaction is, Rate = k[A][B]²
What happens to the rate of reaction if concentrations of A and B are doubled?

If the value of the Kc is large then it shows that the products are:

The rate of a reaction involving ions can be studied by the method

The rate of first-order reaction depends on

The pH of buffer in which concentrations of salt and base are 0.1M and 0.01M respectively
(pKb = 4.0)

Which of the followings is a pseudo-first-order reaction?

1.0g mole of ethyl alcohol and 1.0g mole of acetic acid are mixed. At equilibrium 0.666g mole of the ester is present. The value of the equilibrium constant is