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  • For reaction, the correct option is:  </p

For reaction,2Cl(g)\rightarrow Cl_{2}(g) the correct option is:
 

 

Option: 1

\Delta_{r}H<0 and \Delta_{r}S<0


Option: 2

\Delta_{r}H>0 and  \Delta_{r}S>0


Option: 3

\Delta_{r}H>0 and \Delta_{r}S<0

 


Option: 4

\Delta_{r}H<0 and \Delta_{r}S>0


Answers (1)

best_answer

The reaction occurs as follows:

\mathrm{2Cl(g)\: \longrightarrow\: Cl_{2}(g)}

Since the bond formation is taking place between two Chlorine atoms, an exothermic process change in enthalpy will be negative. 

On the other hand change in entropy will also be negative as the number of particles decreases. 

\mathrm{Thus,\: \Delta _{r}H\: <\: 0 \: and \: \Delta_{r} S<0}

Therefore, Option(1) is correct.

Posted by

SANGALDEEP SINGH

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