The rate of a chemical reaction is defined as the change in:
- AMass of reactant per unit time
- BConcentration of reactant or product per unit time
- CTemperature per unit time
- DVolume of gas per unit time
The unit of reaction rate is:
- Amol dm-3
- Bmol dm-3 s-1
- Cmol s-1
- Ddm3 s-1
The rate of a reaction is generally:
- AConstant throughout the reaction
- BHighest at the beginning and decreases with time
- CLowest at the beginning and increases with time
- DIndependent of concentration
The rate law for a reaction is determined:
- AFrom the balanced chemical equation
- BExperimentally
- CFrom the stoichiometric coefficients
- DFrom the molar masses
For the reaction A → Products, if doubling [A] doubles the rate, the order with respect to A is:
The half-life of a first-order reaction is:
- A0.693k
- B1k[A0]
- C[A0]2k
- D2k[A0]
The minimum energy required for a reaction to occur is called:
- AEnthalpy
- BActivation energy
- CEntropy
- DFree energy
A catalyst increases the rate of a reaction by:
- AIncreasing the activation energy
- BDecreasing the activation energy
- CIncreasing the enthalpy change
- DDecreasing the temperature
In a reaction mechanism, the slowest step is called the:
- AIntermediate step
- BRate-determining step
- CFast step
- DElementary step
According to the Arrhenius equation, as temperature increases, the rate constant:
- ADecreases
- BIncreases
- CRemains constant
- DBecomes zero
