Consider the reactions given below. On the basis of these reactions find out which of the
the algebraic relationships is correct?
1. | x=y | 2. | x=2y |
3. | x>y | 4. | x<y |
Hint: Enthalpy of formation of the compound can be positive or negative
depending on the type of reaction.
Explanation:
In a chemical reaction, the reactant first converts into its atomic state,
then combined, and formed a product.
In the first reaction, C and H are present in their atomic state hence
they will combine and released X amount of energy.
In the second reaction, molecule first converts into atomic hydrogen,
then combined with a carbon atom and formed a product.
The overall for both reactions are as follows:
\({i. \Delta H_r=x=- energy \ of \ the \ bonds \ being \ formed \ (four \ \mathrm{C}-\mathrm{H} \ bond \ formed)}\)
\(ii. \Delta \mathrm{H}_{\mathrm{r}}=\mathrm{y}= \ energy \ of \ the \ bond \ being \ broken \ ( \mathrm{H}-\mathrm{H} \ bond \ break) - \)
\( \ energy \ of \ the \ bonds \ being \ formed \ (four \ \mathrm{C}-\mathrm{H} \ bond \ formed)\)
In both the reaction's energy of the bonds being formed is equal
but in the second reaction, extra energy is used to break the hydrogen molecule bond. Thus, x>y.
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