$ {NO_2}$ required for a reaction is produced by the decomposition of $ {N2O5}$ in $ {CCl4}$ as per the equation
$ { 2N2O5(g) -> 4NO2(g) + O2(g).}$
The initial concentration of $ {N2O5}$ is $3.00\, mol$ $ {L^{-1}}$ and it is $2.75\, mol$ $ {L^{-1}}$ after $30$ minutes. The rate of formation of $ {NO2}$ is :
- $\ce{2.083 \times 10^{-3} \; mol \; L^{-1} \; min^{-1}}$
- $\ce{4.167 \times 10^{-3} \; mol \; L^{-1} \; min^{-1}}$
- $\ce{8.333 \times 10^{-3} \; mol \; L^{-1} \; min^{-1}}$
- $\ce{1.667 \times 10^{-2} \; mol \; L^{-1} \; min^{-1}}$
The Correct Option is D
Solution and Explanation
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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