When you want to calculate the initial rate of reaction there are a few different factors that you need to consider. The first is the rate of the reaction which is defined as the change in concentration of the reactant over time. The second is the activation energy which is the energy required for the reaction to occur. The third is the Arrhenius constant which is a measure of the rate of the reaction.
To calculate the initial rate of reaction you need to first determine the rate of the reaction. This can be done by measuring the change in concentration of the reactant over time. The rate of the reaction is usually given in units of mol/L*s.
Once you have the rate of the reaction you need to determine the activation energy. This is the energy required for the reaction to occur. The activation energy can be determined by performing a reaction in a calorimeter.
Once you have the activation energy you need to determine the Arrhenius constant. This is a measure of the rate of the reaction. The Arrhenius constant is usually given in units of L/mol*s.
Once you have all of these factors you can calculate the initial rate of reaction. The initial rate of reaction is given by the following equation:
Initial Rate = k*e^(-Ea/RT)
where k is the Arrhenius constant Ea is the activation energy R is the gas constant and T is the temperature.
You can use this equation to calculate the initial rate of reaction for any given reaction.
What is the initial rate of the following reaction?
A + 2B –> C
The initial rate of the reaction is -d[A]/dt.
How do you calculate the initial rate of a reaction?
The initial rate of a reaction can be calculated by taking the derivative of the concentration of a reactant with respect to time.
What is the initial rate of the following reaction?
2A + B –> C
The initial rate of the reaction is 2*-d[A]/dt.
What is the initial rate of the following reaction?
A + B –> 2C
The initial rate of the reaction is -d[A]/dt-d[B]/dt.
What is the initial rate of the following reaction?
2A + 3B –> C
The initial rate of the reaction is 2*-d[A]/dt+3*-d[B]/dt.
What is the initial rate of the following reaction?
A + B –> C + D
The initial rate of the reaction is -d[A]/dt-d[B]/dt.
What is the initial rate of the following reaction?
2A + B –> C + 2D
The initial rate of the reaction is 2*-d[A]/dt-d[B]/dt.
What is the initial rate of the following reaction?
A + 2B –> C + D
The initial rate of the reaction is -d[A]/dt+2*-d[B]/dt.
What is the initial rate of the following reaction?
A + B + C –> D
The initial rate of the reaction is -d[A]/dt-d[B]/dt-d[C]/dt.
What is the initial rate of the following reaction?
2A + B + C –> D + E
The initial rate of the reaction is 2*-d[A]/dt-d[B]/dt-d[C]/dt.
What is the initial rate of the following reaction?
A + B + C + D –> E
The initial rate of the reaction is -d[A]/dt-d[B]/dt-d[C]/dt-d[D]/dt.
What is the initial rate of the following reaction?
2A + B + C + D –> E + F
The initial rate of the reaction is 2*-d[A]/dt-d[B]/dt-d[C]/dt-d[D]/dt.
What is the initial rate of the following reaction?
A + B + 2C + D –> E + F + G
The initial rate of the reaction is -d[A]/dt-d[B]/dt+2*-d[C]/dt-d[D]/dt.
What is the initial rate of the following reaction?
A + B + C –> D + E + F
The initial rate of the reaction is -d[A]/dt-d[B]/dt-d[C]/dt.
What is the initial rate of the following reaction?
A + B + 2C –> D + E + F + G
The initial rate of the reaction is -d[A]/dt-d[B]/dt+2*-d[C]/dt.
