|Praopan YodrabumCHE-1202L-01St. Francis collegeLabster lab report: Basic Chemistry Thermodynamics: Solve the challenge of storing renewableenergyLearning ObjectivesExplain the first and second laws of thermodynamicsUnderstand and apply the concept of reaction spontaneityExplain the differences between the enthalpy of combustion, and enthalpy offormationUnderstand the relationship between internal energy and enthalpyPresent Hess’s law in connection with performing enthalpy change calculationsPresent the concepts of exothermic and endothermic reactionsAbstract:In this experiment, the heat of formation of magnesium oxide was calculated bymeasuring the enthalpies of other reactions that could then be added together to obtain the heat offormation of magnesium oxide using Hess’s Law. The two other reactions that were conducted inthe experiment, were the reaction between solid magnesium and hydrochloric acid, as well asthe reaction between magnesium oxide and hydrochloric acid. Knowing these two reactions, andthe heat of formation of water, the heat of formation of magnesium oxide can be found. Thespecific heat of an unknown metal was also found in the lab, through the use of q=mcΔT.Introduction:For this lab, one of the most important concepts that were applied was Hess’s Law. This lawstates that enthalpy for a reaction is equivalent to the addition of enthalpies from reactions thatcan be added together to get the desired reaction. These reactions can be seen as steps of theoverall reaction. Another important aspect of the lab was the transfer of heat from the reaction tothe surroundings. The equation q=mcΔT can be used in order to determine the amount of heat Final Report 3Basic Chemistry Thermodynamics: Solve the challenge of storing renewable energyNAMES:JUNE VERNON B. PASASADABAINSTRUCTOR:ENGR. CHARLIE J VILLARBADATE: 12/08/20ABSTRACT:In total three experiments were conducted to familiarize the laws ofthermodynamics, the concepts of enthalpy and entropy, Gibbs free energy andits relation to spontaneity, and energy storage. Each experiment tackled differentconcepts and this was implemented via the labster learning resource. The firstexperiment posed the problem of transporting solar energy over long distancesand investigated the most efficient way of storing energy in doing so. The secondexperiment used the combustion of octane in a system to determine its energycontent. It showed the relation between enthalpy and the internal energy of thesystem. The third experiment used the transformation of reactants carbondioxide and molecules of water into products of propane and oxygen to discussthe enthalpy and entropy of a reaction in terms of Gibbs free energy. Theseexperiments reveal important concepts in energy conservation and the mostefficient storage material to be utilized in doing so. The concepts of enthalpy andentropy and spontaneity in Gibbs free energy are important supplementaryconcepts to learn in solving the challenge being posed.INTRODUCTION:Objectives: learn about the laws of thermodynamics(1), the very important concepts of enthalpy andentropy(2) and how to use the Gibbs free energy to determine whether a reaction will occurspontaneously or not.(3). Investigate which would be the most efficient way to store energy(4)The first experiment is meant to investigate the problem of conserving solarpower in the most efficient way possible and transporting it at long distances.The experiment familiarized the law of conservation of energy and the mostefficient means of energy storage based on specific energy and energy density. Itcontinued by tackling the most relevant forms of energy storage for long termgiven the problem being posed.The combustion of 1.00 gram of octane was an experiment used to show therelation between the enthalpy and the internal energy of the system. The heatenergy given out by the system is indication of the enthalpy of combustion andthis was measured by the bomb calorimeter.Results of the experiment were |
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Energy is one of the great subject matters of our time, but what is energy actually? In this simulation you will learn the fundamental thermodynamic concepts of enthalpy, entropy and Gibbs free energy. You will also determine the internal energy of a chemical compound by using bomb calorimetry, and you’ll even travel inside the calorimeter to see it in action!
The challenge of storing energy
What is the best way to store energy? There is no simple answer, but in this simulation, you will be encouraged to give it some thought while learning about the very nature of energy and how it connects to chemical reactions. You will assess whether the gasoline component octane is a suitable chemical for energy storage by using a bomb calorimeter.
The fundamental concepts of thermodynamics
The first and second laws of thermodynamics and the core concepts of enthalpy, entropy and Gibbs free energy are introduced in this simulation. You can play around with the energy levels of reactants and products on a virtual energy surface to learn about endothermic and exothermic reactions. The concept of reaction spontaneity is linked to the concept of Gibbs free energy and its temperature dependence is explored in an interactive game. You will have access to a state-of-the-art bomb calorimeter and can travel inside to see it in action, in order to really be able to understand how it works. From here the concept of chemical bond energy is linked to the thermodynamic calculations of enthalpy on the calorimeter output.
Combine theory and practice
Throughout the simulation you will combine the fundamental teachings of thermodynamics with the experimental results from the calorimeter.
Will you be able to suggest a solution for the energy storage challenge?