3A → 2B,rate of reaction +d[B]/dt is equals to
3A → 2B,rate of reaction +d[B]/dt is equals to
– \(\frac{3}{2}\frac{d[A]}{dt}\)
– \(\frac{2}{3}\frac{d[A]}{dt}\)
\(-\frac{1}{3}\frac{d[A]}{dt}\)
\(2d\frac{d[A]}{dt}\)
The Correct Option is B
Solution and Explanation
The correct option is (B) : \(\frac{2}{3}\frac{d[A]}{dt}\)
3A→2B For the given reaction we can write rate of reaction: −\(\frac{1}{3}\)=\(\frac{d[A]}{dt}\) =−\(\frac{1}{20}\)\(\frac{d[B]}{dt}\) ⇒+\(\frac{d[B]}{dt}\)= −\(\frac{2}{3}\frac{d[A]}{dt}\)
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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