Assertion : Ionic reactions are not instantaneous.
Reason : Oppositely charged ions exert strong forces.
Reason : Oppositely charged ions exert strong forces.
- AIf both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.
- BIf both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.
- CIf the Assertion is correct but Reason is incorrect.
- DIf the Assertion is incorrect but the Reason is correct.
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Similar Questions
Which of the following statements is correct?
Medium
View SolutionFind the average rate of formation of $NO_{2_{(g)}}$ in the following reaction:
$2 N_2O_{5_{(g)}} \rightarrow 4 NO_{2_{(g)}} + O_{2_{(g)}}$
Given that $\left[ -\frac{\Delta [N_2O_5]}{\Delta t} \right] = x \ mol \ dm^{-3} \ s^{-1}$
$2 N_2O_{5_{(g)}} \rightarrow 4 NO_{2_{(g)}} + O_{2_{(g)}}$
Given that $\left[ -\frac{\Delta [N_2O_5]}{\Delta t} \right] = x \ mol \ dm^{-3} \ s^{-1}$
For the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$ under certain conditions of temperature and partial pressure of the reactants,the rate of formation of $NH_3$ is $0.001 \ kg \ L^{-1} \ h^{-1}$. The rate of consumption of $H_2$ under the same condition is $..... \ kg \ L^{-1} \ h^{-1}$.
Difficult
View SolutionIdentify the correct expression for the rate of the following reaction: $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
Nitric oxide reacts with $H_2$ according to the reaction: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_2 O_{(g)}$. Identify the correct relation for the rate of disappearance of reactants and the rate of appearance of products.
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