Import Question JSON

$\text{Let's analyze both statements separately:}$ $\text{Assertion (A): Combustion is an exothermic process.}$ $\text{This statement is true. Combustion reactions involve the rapid oxidation of a substance, typically with oxygen, resulting in the release of energy in the form of heat and light. By definition, an exothermic process is one that releases energy to the surroundings, and combustion reactions always release energy.}$ $\text{Reason (R): Combustion is a spontaneous process.}$ $\text{This statement is also true. Spontaneous processes are those that occur without continuous external energy input once initiated. Combustion reactions, once started (e.g., with a spark or flame), continue on their own without requiring additional energy input. The negative Gibbs free energy change (}\Delta\text{G < 0) for combustion reactions confirms their spontaneity.}$ $\text{Now we need to determine if (R) is the correct explanation of (A):}$ $\text{While both statements are true, the reason why combustion is exothermic is not because it is spontaneous. Combustion is exothermic because the formation of new bonds in the products (typically CO}_2 \text{ and H}_2\text{O) releases more energy than is required to break the bonds in the reactants. The exothermic nature is related to the net energy change in bond breaking and forming.}$ $\text{On the other hand, the spontaneity of combustion is related to the overall decrease in Gibbs free energy, which depends on both enthalpy and entropy changes. While the exothermic nature (negative enthalpy change) contributes to spontaneity, it is not the other way around - spontaneity does not explain why a process is exothermic.}$ $\text{Therefore, the correct option is 2: Both (A) and (R) are true but (R) is not the correct explanation of (A).}$