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For a second-order reaction, what is the unit of the rate of the reaction?
- a)s-1
- b)mol L-1s-1
- c)Lmol-1s-1
- d)mol-2 L2 s-1
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
For a second-order reaction, what is the unit of the rate of the react...
The unit for the rate constant of a second order reaction is Lmol−1s−1.
For a second order reaction, rate=k[A]2
molL−1s−1=k(molL−1)2
k=Lmol−1s−1
For a second order reaction, rate=k[A]2
molL−1s−1=k(molL−1)2
k=Lmol−1s−1
Most Upvoted Answer
For a second-order reaction, what is the unit of the rate of the react...
Option C is wrong here, since we are asked to find out the unit for the rate of the reaction but NOT the rate constant. If it was mentioned as rate constant, then it would have been Lmol-1s-1 but since rate of reaction always has the same unit ,i.e., change in concentration per unit time, so answer should be B.
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For a second-order reaction, what is the unit of the rate of the react...
Explanation:
In a second-order reaction, the rate of the reaction is determined by the concentration of two reactants. The rate equation for a second-order reaction can be expressed as:
rate = k[A][B]
Where:
- rate is the rate of the reaction
- k is the rate constant
- [A] and [B] are the concentrations of the reactants A and B, respectively
To determine the unit of the rate of the reaction, we need to consider the units of the rate constant (k) and the concentrations of the reactants.
The rate constant (k) has units that depend on the overall order of the reaction. In a second-order reaction, the units of the rate constant are typically given as L mol^-1 s^-1.
The concentrations of the reactants are given in terms of moles per liter (mol L^-1).
Unit analysis:
Multiplying the units of the rate constant (L mol^-1 s^-1) by the concentrations of the reactants ([A] and [B], both in mol L^-1), we get:
rate = k[A][B] = (L mol^-1 s^-1)(mol L^-1)(mol L^-1)
Simplifying the units, we have:
rate = L mol^-1 s^-1 mol^2 L^-2
Since mol^2 L^-2 can be written as L mol^-1, the final unit of the rate of the reaction is:
rate = L mol^-1 s^-1
Therefore, the correct answer is option 'C' (L mol^-1 s^-1).
In a second-order reaction, the rate of the reaction is determined by the concentration of two reactants. The rate equation for a second-order reaction can be expressed as:
rate = k[A][B]
Where:
- rate is the rate of the reaction
- k is the rate constant
- [A] and [B] are the concentrations of the reactants A and B, respectively
To determine the unit of the rate of the reaction, we need to consider the units of the rate constant (k) and the concentrations of the reactants.
The rate constant (k) has units that depend on the overall order of the reaction. In a second-order reaction, the units of the rate constant are typically given as L mol^-1 s^-1.
The concentrations of the reactants are given in terms of moles per liter (mol L^-1).
Unit analysis:
Multiplying the units of the rate constant (L mol^-1 s^-1) by the concentrations of the reactants ([A] and [B], both in mol L^-1), we get:
rate = k[A][B] = (L mol^-1 s^-1)(mol L^-1)(mol L^-1)
Simplifying the units, we have:
rate = L mol^-1 s^-1 mol^2 L^-2
Since mol^2 L^-2 can be written as L mol^-1, the final unit of the rate of the reaction is:
rate = L mol^-1 s^-1
Therefore, the correct answer is option 'C' (L mol^-1 s^-1).
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