# Educational Activity: Understanding Exothermic and Endothermic Reactions## Image Transcription and ExplanationThis exercise is part of a Chemistry assignment focusing on classifying chemical reactions as either exothermic or endothermic. It involves the combustion reaction of methane in a Bunsen burner.### Part A**Objective:** Classify the given reaction as exothermic or endothermic.**Reaction:** \[ \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(g) + 802 \text{kJ} \]**Options:**- Exothermic reaction- Endothermic reactionThe reaction of methane with oxygen releases 802 kJ of energy, indicating it is an exothermic reaction.### Part B**Objective:** Given \(\Delta H\), express your answer as an integer.- Input box with a label: "kJ"- Button to submit the answerThe reaction enthalpy, \(\Delta H\), is provided as 802 kJ, showing the energy released when methane combusts.### Graphs and DiagramsThere are no graphs or diagrams associated with this image. The focus is on understanding the chemical equation and energy change associated with the reaction.---This educational activity helps students learn how to classify reactions based on their energy changes and understand the concept of exothermic and endothermic processes in chemical reactions.

The energy difference between the products and reactants is known as the energy change of a reaction.If the energy of the products is lower than the energy of the reactants, the enthalpy change of the reaction is negative and the reaction is known as an exothermic reaction. If the energy of the products is higher than the energy of the reactants, the enthalpy change of the reaction is positive and the reaction is known as an endothermic reaction. The exothermic and endothermic reactions are represented as follows:In the given reaction the heat energy is generated, hence the reaction is an exothermic reaction and the enthalpy change of the reaction will be negative. Part Aexothermic reactionPart B∆H of the reaction is as follows:-802 kJ