Chemical kinetics deals with: A) Equilibrium B) Rate of reaction C) Structure of atom D) Thermodynamics Answer: B
Rate of reaction is defined as: A) Change in temperature B) Change in concentration per unit time C) Change in pressure D) Change in volume Answer: B
Unit of rate of reaction is: A) mol B) mol/L C) mol L⁻¹ s⁻¹ D) s⁻¹ Answer: C
Order of reaction is: A) Always whole number B) Sum of powers of concentration C) Always 1 D) Independent of rate Answer: B
Molecularity refers to: A) Number of molecules in rate law B) Number of reacting species in a step C) Order of reaction D) Rate constant Answer: B
For zero-order reaction, rate is: A) Independent of concentration B) Directly proportional C) Inversely proportional D) Square of concentration Answer: A
Unit of zero-order rate constant is: A) s⁻¹ B) mol L⁻¹ s⁻¹ C) L mol⁻¹ s⁻¹ D) mol² Answer: B
Half-life of zero-order reaction depends on: A) Initial concentration B) Rate constant only C) Temperature only D) Pressure Answer: A
For first-order reaction, half-life is: A) Constant B) Depends on concentration C) Increases with time D) Zero Answer: A
Unit of first-order rate constant is: A) mol L⁻¹ s⁻¹ B) s⁻¹ C) L mol⁻¹ s⁻¹ D) mol² Answer: B
Second-order reaction unit of k is: A) s⁻¹ B) mol L⁻¹ s⁻¹ C) L mol⁻¹ s⁻¹ D) L² mol⁻² s⁻¹ Answer: C
Rate law expression is: A) Derived experimentally B) Always theoretical C) Independent of experiment D) Fixed formula Answer: A
Catalyst increases reaction rate by: A) Increasing temperature B) Lowering activation energy C) Changing equilibrium D) Increasing pressure Answer: B
Activation energy is: A) Minimum energy required for reaction B) Maximum energy C) Heat of reaction D) Internal energy Answer: A
Arrhenius equation relates: A) Rate and pressure B) Rate constant and temperature C) Volume and temperature D) Energy and pressure Answer: B
Increasing temperature increases rate because: A) More collisions B) Higher activation energy C) Lower pressure D) Less energy Answer: A
Reaction rate decreases when: A) Temperature increases B) Concentration increases C) Catalyst added D) Temperature decreases Answer: D
Collision theory explains: A) Equilibrium B) Reaction rate C) Atomic structure D) Thermodynamics Answer: B
Effective collision requires: A) Proper orientation B) Low energy C) No contact D) Zero energy Answer: A
Rate constant depends on: A) Concentration B) Temperature C) Pressure D) Volume Answer: B
Pseudo first-order reaction involves: A) Two reactants B) One reactant C) Excess of one reactant D) Zero order Answer: C
Graph of zero-order reaction is: A) Straight line (concentration vs time) B) Curve C) Hyperbola D) Exponential Answer: A
First-order reaction graph is linear for: A) [A] vs t B) ln[A] vs t C) 1/[A] vs t D) t vs [A] Answer: B
Second-order reaction graph is linear for: A) [A] vs t B) ln[A] vs t C) 1/[A] vs t D) t² vs [A] Answer: C
Slowest step determines: A) Molecularity B) Rate of reaction C) Equilibrium D) Energy Answer: B
Reaction mechanism is: A) Single step B) Sequence of steps C) Final product D) Rate law Answer: B
Intermediate is: A) Reactant B) Product C) Formed and consumed D) Catalyst Answer: C
Catalyst is regenerated at: A) Beginning B) Middle C) End D) Never Answer: C
Temperature rise increases rate constant: A) Linearly B) Exponentially C) Logarithmically D) Randomly Answer: B
Rate law for first-order reaction is: A) Rate = k[A] B) Rate = k[A]² C) Rate = k D) Rate = k/[A] Answer: A
Rate law for second-order reaction is: A) k[A] B) k[A]² C) k D) k/[A] Answer: B
Zero-order rate law is: A) k[A] B) k[A]² C) k D) k/[A] Answer: C
Half-life formula for first-order is: A) t₁/₂ = 0.693/k B) t₁/₂ = k/0.693 C) t₁/₂ = [A]/k D) t₁/₂ = k[A] Answer: A
Doubling concentration doubles rate in: A) Zero-order B) First-order C) Second-order D) All Answer: B
Doubling concentration quadruples rate in: A) Zero-order B) First-order C) Second-order D) Third-order Answer: C
Integrated rate law is used to: A) Determine order B) Find temperature C) Find pressure D) Find volume Answer: A
Rate constant increases with: A) Pressure B) Temperature C) Volume D) Mass Answer: B
High activation energy means: A) Fast reaction B) Slow reaction C) No reaction D) Instant reaction Answer: B
Reaction with low Ea is: A) Slow B) Fast C) Impossible D) Reversible Answer: B
Enzymes act as: A) Inhibitors B) Catalysts C) Reactants D) Products Answer: B
Increasing surface area increases rate due to: A) More collisions B) Less energy C) Less contact D) Low temperature Answer: A
Reaction rate is highest at: A) Start B) Middle C) End D) Constant Answer: A
Rate law depends on: A) Stoichiometry B) Mechanism C) Temperature D) Volume Answer: B
Reaction order can be: A) Fractional B) Integer only C) Zero only D) Negative only Answer: A
Molecularity is always: A) Fractional B) Integer C) Zero D) Negative Answer: B
Arrhenius equation: A) k = Ae^(-Ea/RT) B) PV = nRT C) E = mc² D) F = ma Answer: A
Increasing catalyst concentration: A) Decreases rate B) Increases rate C) No effect D) Stops reaction Answer: B
Rate of reaction depends on: A) Nature of reactants B) Temperature C) Catalyst D) All Answer: D
Reaction mechanism helps to: A) Predict rate law B) Predict volume C) Predict pressure D) Predict temperature Answer: A
Rate-determining step is: A) Fastest step B) Slowest step C) Middle step D) First step Answer: B
The rate of a reaction is fastest when concentration is: A) Lowest B) Zero C) Highest D) Constant Answer: C
Which factor does NOT affect reaction rate? A) Temperature B) Catalyst C) Color D) Concentration Answer: C
In a first-order reaction, rate depends on: A) Square of concentration B) Concentration C) No concentration D) Pressure Answer: B
Half-life of second-order reaction depends on: A) Initial concentration B) Only rate constant C) Temperature only D) Pressure Answer: A
Which reaction has constant rate? A) First-order B) Second-order C) Zero-order D) Third-order Answer: C
The slope of ln[A] vs time graph equals: A) k B) -k C) 1/k D) -1/k Answer: B
The slope of 1/[A] vs time graph equals: A) k B) -k C) 1/k D) -1/k Answer: A
Rate constant is independent of: A) Temperature B) Catalyst C) Concentration D) Activation energy Answer: C
Arrhenius factor A represents: A) Activation energy B) Frequency factor C) Rate D) Temperature Answer: B
Activation energy decreases with: A) Catalyst B) Temperature C) Pressure D) Volume Answer: A
Reaction rate doubles when temperature increases by about: A) 1°C B) 5°C C) 10°C D) 50°C Answer: C
Reaction mechanism involves: A) Only one step B) Multiple steps C) No steps D) Random process Answer: B
Elementary reaction is: A) Multi-step B) Single-step C) Complex D) Slow Answer: B
Order of elementary reaction equals: A) Molecularity B) Rate C) Time D) Temperature Answer: A
Intermediate species are: A) Stable B) Final products C) Short-lived D) Catalysts Answer: C
Which is true for catalyst? A) Consumed permanently B) Changes equilibrium C) Lowers activation energy D) Increases Ea Answer: C
Which graph gives rate constant for first-order reaction? A) [A] vs t B) ln[A] vs t C) 1/[A] vs t D) t² vs [A] Answer: B
Reaction rate is zero when: A) Concentration is zero B) Temperature is high C) Catalyst added D) Pressure high Answer: A
Rate law is determined by: A) Stoichiometry B) Experiment C) Theory only D) Pressure Answer: B
High temperature increases reaction rate due to: A) More collisions B) Less energy C) Low pressure D) Less molecules Answer: A
A catalyst provides: A) New reaction pathway B) Higher activation energy C) No pathway D) Higher pressure Answer: A
Reaction order is sum of: A) Coefficients B) Powers of concentration C) Reactants D) Products Answer: B
Molecularity is defined for: A) Overall reaction B) Elementary step C) Rate law D) Equilibrium Answer: B
Molecularity can be: A) Zero B) Fractional C) Integer only D) Negative Answer: C
Order of reaction can be: A) Fractional B) Negative C) Zero D) All Answer: D
Reaction rate depends on: A) Nature of reactants B) Temperature C) Catalyst D) All Answer: D
Fast reactions have: A) High Ea B) Low Ea C) No Ea D) Infinite Ea Answer: B
Slow reactions have: A) Low Ea B) High Ea C) No Ea D) Zero Ea Answer: B
Rate constant k increases with: A) Temperature B) Volume C) Mass D) Pressure Answer: A
Arrhenius equation shows exponential relation between: A) k and T B) k and P C) V and T D) E and P Answer: A
Rate-determining step controls: A) Overall rate B) Temperature C) Volume D) Pressure Answer: A
Catalyst affects: A) Rate B) Equilibrium C) Product D) Temperature Answer: A
Which is not a unit of rate constant? A) s⁻¹ B) L mol⁻¹ s⁻¹ C) mol L⁻¹ s⁻¹ D) kg Answer: D
Reaction order is experimentally found using: A) Graph B) Theory C) Guess D) Pressure Answer: A
If rate = k[A]²[B], order is: A) 2 B) 3 C) 1 D) 4 Answer: B
Half-life of first-order reaction is independent of: A) Initial concentration B) Rate constant C) Temperature D) Catalyst Answer: A
Rate of reaction increases with: A) Decrease in temperature B) Increase in concentration C) Decrease in pressure D) Decrease in surface area Answer: B
Surface area affects reactions involving: A) Gases B) Liquids C) Solids D) All Answer: C
Increasing pressure increases rate for: A) Solids B) Liquids C) Gases D) All Answer: C
Reaction rate is maximum at: A) Beginning B) End C) Middle D) Constant Answer: A
A straight line graph indicates: A) Constant rate B) Changing rate C) Zero rate D) Infinite rate Answer: A
Integrated rate law helps to find: A) Order B) Pressure C) Volume D) Mass Answer: A
Catalyst is: A) Reactant B) Product C) Substance that speeds reaction D) Inhibitor Answer: C
Reaction with multiple steps is: A) Simple B) Complex C) Fast D) Slow Answer: B
Collision theory requires: A) Energy B) Orientation C) Contact D) All Answer: D
Effective collision needs: A) Correct orientation B) Sufficient energy C) Both D) None Answer: C
Rate constant decreases when: A) Temperature increases B) Temperature decreases C) Catalyst added D) Pressure increases Answer: B
Rate constant is symbolized by: A) k B) r C) t D) v Answer: A
Unit of rate constant depends on: A) Temperature B) Order of reaction C) Pressure D) Volume Answer: B
Chemical kinetics studies: A) Speed of reactions B) Equilibrium C) Thermodynamics D) Structure Answer: A