The rate of reaction between two reactants A and B decreases by a factor of 4,if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is:
- -1
- -2
- 1
- 2
The Correct Option is B
Solution and Explanation
The method below can be used to determine the response rate: rate = \(K[A]^x \times[B]^y\)
A is the concentration of reactant A, B I is the concentration of reactant B, x is the order of reaction with respect to A, and y is the order of reaction with respect to reactant B in the above formula.
The rate constant is given as k.
The relationship between the rate and concentration of the reactant is known as the order of reaction.
\(\frac{r_1}{4}\) = \(K[A]^x \times[B]^y\)
\(\frac{r_1}{4\times r_1}=(2)^y\)
\(\frac{1}{4}=(2)^y\)
\(\bigg(\frac{1}{2}\bigg)^2=(2)^y\)
\((2)^{-2}-(2)^y\)
\(\therefore y = -2\)
So, the correct option is (B): -2
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Concepts Used:
Rate of a Chemical Reaction
The rate of a chemical reaction is defined as the change in concentration of any one of the reactants or products per unit time.
Consider the reaction A → B,
Rate of the reaction is given by,
Rate = −d[A]/ dt=+d[B]/ dt
Where, [A] → concentration of reactant A
[B] → concentration of product B
(-) A negative sign indicates a decrease in the concentration of A with time.
(+) A positive sign indicates an increase in the concentration of B with time.
Factors Determining the Rate of a Reaction:
There are certain factors that determine the rate of a reaction:
- Temperature
- Catalyst
- Reactant Concentration
- Chemical nature of Reactant
- Reactant Subdivision rate