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The heat content of the products is more than that of the reactants in an endothermic reaction. If true enter 1 else 0.

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Hint: Endothermic reactions are those chemical reactions which require energy from external surroundings, for the reaction to proceed.

Step-by-step solution: In order to answer this question, we need to have an understanding of endothermic and exothermic reactions and the enthalpy change associated with them.
Endothermic reactions proceed by absorbing energy from the surroundings in the form of heat while in exothermic reactions, energy is released in the form of heat or light to the surroundings. This is because the total energy of the products is less than that of the reactants.
Enthalpy is defined as the amount of heat absorbed or released during the course of a chemical reaction. Enthalpy is also termed as the “heat content”. It is denoted by $H.$ Enthalpy change $\Delta H$ for an exothermic reaction is negative while for an endothermic reaction, it is positive.
Let us consider a general endothermic reaction of the type,
\[A + B + q \to C + D\]
In this equation, $q$ is the amount of heat energy absorbed during the reaction, in order to yield the products $C$ and $D$ .
Now, if we will calculate the enthalpy change for the above reaction, we will proceed as follows,
$\Delta H_{Reaction} = H_{Products} - H_{Reactants}$ $ = + q$ …. (1)
Positive sign of $q$ signifies that the heat has been absorbed in the reaction.
From equation (1), we can write $H_{Reactants} + q = H_{Products}$
We can clearly see that the heat content of products is more than that of heat content of reactants.

Note: Exothermic reactions may occur spontaneously which results in high randomness of the system. This is followed by a negative heat flow or decrease in enthalpy.
Endothermic reactions are nonspontaneous and thus some work needs to be done in order to proceed these reactions. These reactions are characterized by a positive heat flow or an increase in the enthalpy.