Answer: Option (d) is the correct answer.
Explanation:
The reaction given is as follows.
[tex]Cl_{2}(g) + 2KBr (aq) \rightarrow 2KCl(aq) + Br_{2}(l)[/tex]
From this equation, it can be seen that chlorine gas reacts with aqueous potassium bromide solution to give aqueous potassium chloride and liquid bromine.
Also, chlorine is more reactive than bromine because it is smaller in size than bromine and has less shielding effect so it will readily accept an electron. Thus, chlorine displaces bromine from potassium bromide solution.
Thus, we can conclude that chlorine gas reacts with potassium bromide to form potassium chloride in solution and liquid bromine.
Answer:
Chlorine gas reacts with potassium bromide to form potassium chloride in solution and liquid bromine
Explanation:
Cl2(g) + 2KBr(aq) → 2KCl(aq)+ Br2(l)
From the options, we only have one where there is Chlorine, in the form of a gas and that is the fifth option, remember that the little parenthesis below the elements show us the state in which those given element are found at the moment of the reaction, so Chlorine gas reacts with potassium bromide in acqous or liquid state to form potassium chloride in acqous or liquid state and liquid bromine.
