Question

equal volume of H2 and Cl2 are mixed.how will the volume of the mixture changes after the reaction at same temperature and pressure?? 1-unchanged. 2-reduced to half. 3-increases two fold. 4-none of these please answer quickly​

Answer 1

At the same temperature and pressure, the volume of the mixture of equal volumes of and will be unchanged. (option 1)

• According to Avogadro's law, under the conditions of the same temperature and pressure, volume is directly proportional to the number of moles.
• $H_2(g) +Cl_2(g)---- > 2HCl(g)$

t=0       1            1                           0

t=t        0           0                          2          (completion)

• As we can see the number of moles of the product after the reaction is the same as the number of moles of the reactant, there is no change in the number of moles and hence there is no change in the volume.

Answer 2

Answer:

The correct option is 1) Volume remains unchanged.

Explanation:

According to Avogadro's hypothesis,

$P V= nRT$

However, under the same temperature and pressure conditions,

Volume ∝ no. of moles

Let "n" be the number of moles.

Therefore, in the reaction given below, the no. of moles are:-

                                  $H_{2(g)} + Cl_{2 (g)}$ ⇒$2HCL_{(g)}$

                                     n         n           2n

At t = start                   n           n             0

At t = completion       0           0              2n

Initial no. of moles = 2n

Final no. of moles = 2n

There is no change in the number of moles since the number of moles of the product is equal to the number of moles of the reactant. As a result, the volume remains unchanged.

#SPJ2