Assertion :For a reaction $A + B \to C$ , the rates of reaction for $A, B$ and $C$ are equal Reason: For any reaction, the rate of reaction for all reactants and products are equal

Both assertion and reason are correct and reason is the correct explaination of the assertion

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Both assertion and reason are correct, but reason is not the correct explanation of the assertion

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Assertion is correct, but reason is incorrect

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Assertion is incorrect, but reason is correct

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Solution

The correct option is C Assertion is correct, but reason is incorrect
For a given reaction, $a A + b B \to c C$
Rate of reactions are equal for $A, B$ and $C$ when the stoichiometry coefficients are equal ; $a = b = c$

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Similar questions

Assertion (A) The enthalpy of reaction remains constant in the presence of a catalyst.

Reason (R) A catalyst participating in the reaction forms different activated complex and lowers down the activation energy but the difference in enrgy of reactant and product remains the same.

(a) Both assertion and reason are correct and the reason is correct explanation of assertion
(b) Both assertion and reason are correct, but reason does not explain assertion.
(c) Assertion is correct, but reason is incorrect
(d) Both assertion and reason are incorrect
(e) Assertion is incorrect but reason is correct.

Assertion (A) Rate constant determined from Arrhenius equation are fairly accurate for simple as well as complex molecules.

Reason (R) Reactant molecules undergo chemical change irrespective of their orientation during collision.

Assertion (A) Order of the reaction can be zero or fractional.

Reason (R) We cannot determine order from balanced chemical equation.

Assertion (A) Order and molecularity are same.

Reason (R) Order is determined experimentally and molecularity is the sum of the stoichimetric coeffcient of rate determining elementary step.

Assertion (A) All collision of reactant molecules lead to product formation.

Reason (R) Only those collisions in which molecules have correct orientation and sufficient kinetic energy lead to compound formation.

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Assertion :For a reaction A+B→C , the rates of reaction for A,B and C are equal Reason: For any reaction, the rate of reaction for all reactants and products are equal

The correct option is C Assertion is correct, but reason is incorrectFor a given reaction, aA+bB→cCRate of reactions are equal for A, B and C when the stoichiometry coefficients are equal ; a=b=c

Assertion :For a reaction $A + B \to C$ , the rates of reaction for $A, B$ and $C$ are equal Reason: For any reaction, the rate of reaction for all reactants and products are equal

The correct option is C Assertion is correct, but reason is incorrect
For a given reaction, $a A + b B \to c C$
Rate of reactions are equal for $A, B$ and $C$ when the stoichiometry coefficients are equal ; $a = b = c$