(b) Is this process endothermic or exothermic?

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insert step 1> Identify the process being described in the problem. Is it a chemical reaction, a phase change, or another type of process?

insert step 2> Determine if the process absorbs or releases energy. Endothermic processes absorb energy, while exothermic processes release energy.

insert step 3> Consider the context or any given data, such as temperature changes, heat flow, or enthalpy changes, to help identify the nature of the process.

insert step 4> If applicable, use the sign of the enthalpy change (ΔH) to determine the process type: a positive ΔH indicates an endothermic process, while a negative ΔH indicates an exothermic process.

insert step 5> Conclude whether the process is endothermic or exothermic based on the analysis from the previous steps.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Endothermic Processes

Endothermic processes are chemical reactions or physical changes that absorb energy from their surroundings, usually in the form of heat. This results in a decrease in the temperature of the surrounding environment. A common example is the melting of ice, where heat is absorbed to convert solid ice into liquid water.

Exothermic Processes

Exothermic processes are reactions or changes that release energy, typically as heat, into the surroundings. This leads to an increase in the temperature of the environment. Combustion reactions, such as burning wood or gasoline, are classic examples of exothermic processes, as they produce heat and light.

Thermodynamics

Thermodynamics is the branch of physical science that deals with the relationships between heat, work, temperature, and energy. It provides the framework for understanding whether a process is endothermic or exothermic by analyzing the energy changes involved. The first law of thermodynamics, which states that energy cannot be created or destroyed, is particularly relevant in determining the energy flow in chemical reactions.

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A 2.200-g sample of quinone (C₆H₄O₂) is burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 23.44 to 30.57 °C. b. What is the heat of combustion per mole of quinone?

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