11. Calculate the energy required to produce 12.00 mol of CI207 on the basis of the

Chemistry

1 answer:

Ber [7]3 years ago

4 0

Answer: 780 kcal are required to produce 12.00 mol of $Cl_2O_7$

Explanation:

Endothermic reactions are defined as the reactions in which energy of the product is greater than the energy of the reactants. The total energy is absorbed in the form of heat and written along with reactants.

The balanced chemical reaction is:

$2Cl_2(g)+7O_2(g)+130kcal\rightarrow 2Cl_2O_7(g)$

According to stoichiometry :

2 moles of $Cl_2O_7$ are produced by absorption of energy = 130 kcal

Thus 12.00 moles of $Cl_2O_7$ are produced by absorption of energy = $\frac{130}{2}\times 12.00=780kcal$

Thus 780 kcal are required to produce 12.00 mol of $Cl_2O_7$

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In the reaction 2H2O (1)+ 2Cl^- (aq)= H2(g)+Cl2 (g)+ 2OH^-(aq), which substance is reduced?

Oksanka [162]

Answer:- C. H

Explanations:- Reduction is gain of electron. In other words we could say that decrease in oxidation number is reduction.

As per the rules, oxidation number of hydrogen in its compounds is +1(except metal hydrides) and the oxidation number of oxygen in its compounds is -2.

The oxidation number in elemental form is zero.

In $H_2O$ , the oxidation number of H is +1 and oxidation number of O is -2. Oxidation number of Cl in $Cl^-$ is -1. On product side, the oxidation number of hydrogen in $H_2$ is zero and in $OH^-$ the oxidation number of H is +1 and that of O is -2. Oxidation number of Cl in $Cl_2$ is 0.