For the reaction
$ 2{{N}_{2}}{{O}_{5}}(g)\xrightarrow[{}]{{}}4N{{O}_{2}}(g)+{{O}_{2}}(g) $
if the concentration of $ N{{O}_{2}} $ increases by $ 5.2\times {{10}^{-3}} $ M in 100 s then the rate of the reaction is:
- $ 1.3\times {{10}^{-5}}M{{s}^{-1}} $
- $ 0.5\times {{10}^{-4}}M{{s}^{-1}} $
- $ 7.6\times {{10}^{-4}}M{{s}^{-1}} $
- $ 2\times {{10}^{-3}}M{{s}^{-1}} $
The Correct Option is A
Solution and Explanation
= $ \frac{5.2\times {{10}^{-3}}}{4\times 100} $
$ =1.3\times {{10}^{-5}}M{{s}^{-1}} $
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\[ 2A + B \rightarrow 2C + D \]
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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