In which of the following reactions is chlorine (Cl) oxidized? Br2 + 2Cl− → Cl2 + 2Br− Cl2 + 2e− → 2Cl− 2ClO3− + 12H+ → Cl2 + 6H
2 answers:
Answer:
Explanation:
Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.
Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.
On reactant side:
Oxidation state of chlorine = -1
On product side:
Oxidation state of chlorine = 0
The oxidation state of chlorine increases from -1 to 0. Thus, it is getting oxidized and it undergoes oxidation reaction.
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Answer : The enthalpy change for the reaction is, 97.7 kJ
Explanation :
According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.
According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.
The given main chemical reaction is,
The intermediate balanced chemical reaction will be,
(1)
(2)
(3)
Now we are multiplying reaction 1 by 2 and reversing reaction 3 and then adding all the equations, we get :
(1)
(2)
(3)
The expression for enthalpy of main reaction will be,
Therefore, the enthalpy change for the reaction is, 97.7 kJ