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**Q1. **For a reaction, the rate constant is 2.34s^(-1). The half-life period for reaction is
Solution

K=2.34s^(-1)
Unit of k suggest that the reaction is of 1st order, hence for 1st order reaction,
t_(1/2)=0.693/k
=0.693/2.34=0.30s

**Q2.**Effect of temperature on reaction rate is given by
Solution

Effect of temperature on reaction rate is given by Arrhenius equation
k=Ae^(-E_a/RT)

**Q3. **The rate constant for a chemical reaction has units L mol^(-1) s^(-1),order of the reaction will be
Solution

**Q4. **For the non-equilibrium process, A+B⟶ Products, the rate is first order with respect to A and second order respect to B. If 1.0 mole each of A and B are introduced into a 1 litre vessel and the initial rate was 1.0×〖10〗^(-2) mol/litre-sec. The rate (in mol litre^(-1) sec^(-1) ) when half of the reactants have been used:
Solution

**Q6. **A zero order reaction is one:
Solution

Zero order reactions occur with constant rate.

**Q8.**The rate constant of a reaction is found to be 3×〖10〗^(-3) mol L^(-1) min┴(-1) . The order of reaction is
Solution

**Q9.**For the elementary step,
(CH_3 )_3∙CBr(aq)⟶(CH_3 )_3 C^+ (aq)+Br^- (aq) the molecularity is:
Solution

Molecularity represents the number of molecules of reactants taking part in an elementary step of reaction

**Q10. **Which of the following statement is incorrect about the molecularity of a reaction?

Solution

Order may or may not be equal to molecularity.

**Q1.**For a reaction, the rate constant is 2.34s^(-1). The half-life period for reaction is

Solution

K=2.34s^(-1) Unit of k suggest that the reaction is of 1st order, hence for 1st order reaction, t_(1/2)=0.693/k =0.693/2.34=0.30s

K=2.34s^(-1) Unit of k suggest that the reaction is of 1st order, hence for 1st order reaction, t_(1/2)=0.693/k =0.693/2.34=0.30s

**Q2.**Effect of temperature on reaction rate is given by

Solution

Effect of temperature on reaction rate is given by Arrhenius equation k=Ae^(-E_a/RT)

Effect of temperature on reaction rate is given by Arrhenius equation k=Ae^(-E_a/RT)

**Q3.**The rate constant for a chemical reaction has units L mol^(-1) s^(-1),order of the reaction will be

Solution

**Q4.**For the non-equilibrium process, A+B⟶ Products, the rate is first order with respect to A and second order respect to B. If 1.0 mole each of A and B are introduced into a 1 litre vessel and the initial rate was 1.0×〖10〗^(-2) mol/litre-sec. The rate (in mol litre^(-1) sec^(-1) ) when half of the reactants have been used:

Solution

**Q6.**A zero order reaction is one:

Solution

Zero order reactions occur with constant rate.

Zero order reactions occur with constant rate.

**Q8.**The rate constant of a reaction is found to be 3×〖10〗^(-3) mol L^(-1) min┴(-1) . The order of reaction is

Solution

**Q9.**For the elementary step, (CH_3 )_3∙CBr(aq)⟶(CH_3 )_3 C^+ (aq)+Br^- (aq) the molecularity is:

Solution

Molecularity represents the number of molecules of reactants taking part in an elementary step of reaction

Molecularity represents the number of molecules of reactants taking part in an elementary step of reaction

**Q10.**Which of the following statement is incorrect about the molecularity of a reaction?

Solution

Order may or may not be equal to molecularity.

Order may or may not be equal to molecularity.