Test your understanding of reaction rates, order, and mechanisms
Question 1 of 10
Question 1
The rate of a chemical reaction:
Increases as the reaction proceeds
Decreases as the reaction proceeds
May increase or decrease during the reaction
Remains constant as the reaction proceeds
Question 2
The rate at which a substance reacts depends on its:
Atomic weight
Equivalent weight
Molecular weight
Active mass
Question 3
If doubling the concentration of a reactant 'A' increases the rate 4 times and tripling the concentration of 'A' increases the rate 9 times, the rate is proportional to:
Concentration of 'A'
Square of concentration of 'A'
Under root of the concentration of 'A'
Cube of concentration of 'A'
Question 4
The rate law for the reaction RCl + NaOH(aq) → ROH + NaCl is given by Rate = K₁[RCl]. The rate of the reaction will be:
Doubled on doubling the concentration of sodium hydroxide
Halved on reducing the concentration of alkyl halide to one half
Decreased on increasing the temperature of the reaction
Unaffected by increasing the temperature of the reaction
Question 5
The rate of chemical reaction at constant temperature is proportional to:
The amount of products formed
The product of masses of the reactants
The product of the molar concentration of the reactants
The mean free path of the reaction
Question 6
The concentration of a reactant decreases from 0.2 M to 0.1 M in 10 minutes. The rate of the reaction is:
0.01 M
10⁻²
0.01 mol dm⁻³ min⁻¹
1 mol dm⁻³ min⁻¹
Question 7
When a reaction is progressing:
The rate of the reaction goes on increasing
The concentration of the products goes on decreasing
The concentration of the reactants goes on decreasing
The reaction rate always remains constant
Question 8
Molecularity of a reaction:
Can be zero or fractional
Is always equal to the order of reaction
Is the number of molecules involved in the rate-determining step
Is derived from the balanced chemical equation
Question 9
According to the Arrhenius equation, the rate constant k is given by:
k = A e^(Ea/RT)
k = A e^(-Ea/RT)
k = A e^(RT/Ea)
k = A e^(-RT/Ea)
Question 10
For a reaction to occur according to collision theory:
Reacting molecules must collide with proper orientation
Reacting molecules must have energy equal to or greater than threshold energy
Both proper orientation and sufficient energy are required
Only proper orientation is required, energy doesn't matter