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Consider two gases, A and B, are in a container at room temperature. What effect will the following changes have on the rate of the reaction between these gases? The number of molecules of gas A is doubled.


A.decrease

B.increase

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lublana

Answer:

B: increase.

Explanation:

When we are considering two gases A and B in a container at room temperature .

We have to find the change on  rate of reaction when the number of molecules of gases A is doubled

Let [A]=a and [B]=b

A+B\(\rightarrow\) product

Rate of reaction

\(R_1=k[A][B]=kab\)

We know that concentration is increases with increase in number of moles

When the number of molecules of gases A is doubled then concentration of gases A increases.

Therefore ,[A]=2a

Rate of reaction

\(R_2=k(2a)(b)=2kab\)

\(R_2=2R_1\)

Hence, the rate of reaction is  2 times the initial rate of reaction.Therefore, the rate of reaction will increase when the number of molecules of gases A is doubled.

Answer: B: increase.

Answer:

The answer is increase.

Explanation:

I just took the assignment.

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