(b) Is this process endothermic or exothermic?

Verified step by step guidance

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.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

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.

Recommended video:

Guided course

01:18

First Law of Thermodynamics

Related Practice

Textbook Question

Consider the data about gold metal in Exercise 5.26(b). (c) What is the molar heat capacity of Au(s)?

Textbook Question

When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 21.6 to 37.8 °C (a) Calculate the quantity of heat (in kJ) released in the reaction.

Textbook Question

When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 21.6 to 37.8 °C (b) Using your result from part (a), calculate H (in kJ/mol KOH) for the solution process. Assume that the specific heat of the solution is the same as that of pure water.

Textbook Question

A 1.50-g sample of quinone (C₆H₄O₂) is burned in a bomb calorimeter whose total heat capacity is 8.500 kJ/°C. The temperature of the calorimeter increases from 25.00 to 29.49°C. (b) What is the heat of combustion per gram of quinone and per mole of quinone?

Textbook Question

A 1.50-g sample of quinone (C₆H₄O₂) is burned in a bomb calorimeter whose total heat capacity is 8.500 kJ/°C. The temperature of the calorimeter increases from 25.00 to 29.49 °C. (a) Write a balanced chemical equation for the bomb calorimeter reaction.

Textbook Question

A 2.20-g sample of phenol (C₆H₅OH) was burned in a bomb calorimeter whose total heat capacity is 11.90 kJ/°C. The temperature of the calorimeter plus contents increased from 21.50 to 27.50 °C. (a) Write a balanced chemical equation for the bomb calorimeter reaction.