Chemical Kinetics and Equilibrium

Consider the following statements.

I. In some reactions, reactants react rapidly in the presence of sunlight.

II. Neutralisation reaction is an example of irreversible reaction.

Which of the above statements is/are true?

Statement I: Generally, catalyst increases, the rate of reaction in forward direction.

Statement II: Catalyst decreases the activation energy of the reactant.

Which of the following represents the rate constant for the reaction in which activation energy is zero?

Statement I: The reactions with the greater activation energy will be faster.

Statement II: The reaction with the smaller activation energy will be faster.

Consider the following statements, in homogeneous reactions, the:

I. Reactants found in the same physical state.

II. Reaction proceeds in forward direction when concentration of reactants is more than products.

III. Reaction between ethanol and acetic acid in the presence of sulphuric acid is an example of slow reaction.

Which of the above statements are correct?

In a reaction, the concentration of reactants is equal to the concentration of products. This state of a reaction is called as:

Corrosion is the oxidative deterioration of a metal, such as tranishing of silver, rusting of iron and development of a green coating on copper and bronze. Corrosion is an example of:

A group of students in a school laboratory, mixed the solution of $\mathrm{NaCl}$ with ${\mathrm{AgNO}}_3$ during an experiment. But they could not able to determine the rate of reaction because:

Solubility of calcium oxides in water increases on lowering the temperature. Thus, dissolution process is:

In the presence of a catalyst, what happens to the chemical equilibrium?

What is the role of a positive catalyst in a chemical reaction?