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Acid-Base Equilibrium
Atomic Structure And Related Patterns In The Periodic Table
Bonding And Structure, And Intermolecular Forces
Chemical Equilibrium
D-Block Elements (Transition Elements)
DESCRIPTIVE INORGANIC CHEMISTRY: Group IV (14)
DESCRIPTIVE INORGANIC CHEMISTRY: Halogens (GROUP VII or 17)
DESCRIPTIVE INORGANIC CHEMISTRY: Modern Periodic Table, Periodicity And S-Block Elements
Functional Group Chemistry And Reaction Mechanism
ORGANIC CHEMISTRY: Fundamentals
Raoult’s Law And Phase Equilibria
Reaction Kinetics
Redox Equilibrium
The Mole Concept

5/35 MCQs for:

Reaction Kinetics

In a study of rate of reaction

3X + 2Y + Z → 2XY + XZ

Solutions containing different initial concentrations of X, Y and Z were allowed to react. The time taken for the concentration of XY and XZ to reach a certain level was measured. The results are shown in the picture.

The rate law for the reaction above is:

R = K[X][Y].

R = K[X]⁰[Y]².

R = K[X]²[Y].

R = K[X][Y]².

The decomposition of hydrogen iodide, has rate constants of 9.51 x 10⁻⁹ L mol⁻¹ s⁻¹ at 500 K and 1.10 x 10⁻⁵ L mol⁻¹ s⁻¹ at 600 K. The activation energy for this reaction is:

1.76 x 10² J mol⁻¹.

1.76 x 10² kJ mol⁻¹.

1.76 x 10⁵ kJ mol⁻¹.

1.76 x 10² kJ.

Consider a termolecular reaction of the type

A + 2B → products.

The units of the rate constant for the reaction is:

dm⁶ mol⁻² s⁻¹.

mol dm⁻³ s⁻¹.

dm⁶ mol⁻² s⁻².

dm⁹ mol⁻³ s⁻¹.

The two most important theories of kinetics are:

Collision theory and transition state theory.

Catalysis theory and transition state theory.

Collision theory and catalysis theory.

Intermediate state theory and transition state theory.

By what factor does the rate change in each of the following cases (assuming constant temperature)?
A reaction is second order in reactant C, and [C] is tripled.

6

12

9

3