Entropy practice worksheet

In this practice worksheet students will explore entropy concepts, predict if a process increases or decreases in entropy and finally use Gibb's Free Energy with enthalpy and entropy to determine if a process is spontaneous.

Please do not upload these to the internet, as students will find them and harm their learning and that of my students. If you would like me to write a customized lab for you, please email me. Thanks for looking. Teachers Pay Teachers is an online marketplace where teachers buy and sell original educational materials.

Entropy Calculation

Are you getting the free resources, updates, and special offers we send out every week in our teacher newsletter? All Categories. Grade Level. Resource Type. Log In Join Us. View Wish List View Cart. Entropy and Free Energy Practice Worksheet. ChemistryGeneral SciencePhysical Science. Grade Levels. WorksheetsActivitiesHomework. File Type. Also included in:. This is a collection of 10 as of May of my first-year chemistry resources covering thermochemistry, enthalpy, entropy, free energy, specific heat, and calorimetry.

These activities are easy to grade but rigorous and will help prepare your stude. View Bundle. This is a collection of all as of October my first-year chemistry resources. These activities are easy to grade but rigorous and will help prepare your students for more advanced coursework in physical science.

I hope you and your students. Product Description. Materials needed: none Please do not upload these to the internet, as students will find them and harm their learning and that of my students.E: Matter and Measurement Exercises 1. E: Atoms, Molecules, and Ions Exercises 2.

Entropy Change For Melting Ice, Heating Water, Mixtures & Carnot Cycle of Heat Engines - Physics

E: Stoichiometry Exercises 3. E: Reactions in Aqueous Solution Exercises 4. E: Thermochemistry Exercises 5. E: Electronic Structure of Atoms Exercises 6. E: Periodic Properties of the Elements Exercises 7. E: Exercises 9.

entropy practice worksheet

E: Exercises E: Liquids and Intermolecular Forces Exercises E: Properties of Solutions Exercises E: Acid—Base Equilibria Exercises E: Chemistry of the Nonmetals Exercises E: Organic and Biological Chemistry Exercises E: Matter and Measurement Exercises 2. E: Atoms, Molecules, and Ions Exercises 3. E: Stoichiometry Exercises 4. E: Aqueous Reactions Exercises 5. E: Thermochemistry Exercises 6. E: Electronic Structure Exercises 7. E: Periodic Trends Exercises 8. E: Chemical Bonding Basics Exercises 9.

E: Bonding Theories Exercises E: Gases Exercises Solids and Modern Materials Exercises E: Kinetics Exercises E: Chemical Equilibrium Exercises E: Chemistry of the Environment Exercises E: Chemical Thermodynamics Exercises E: Electrochemistry Exercises E: Nuclear Chemistry Exercises Teachers Pay Teachers is an online marketplace where teachers buy and sell original educational materials.

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English Language Arts. Foreign Language. Social Studies - History. History World History. For All Subject Areas. See All Resource Types. This is a single 2-page worksheet covering entropy.Answer the following to the best of your ability.

Questions left blank are not counted against you. A new page will appear showing your correct and incorrect responses.

If you wish, you may return to the test and attempt to improve your score.

entropy practice worksheet

If you are stumped, answers to numeric problems can be found by clicking on "Show Solution" to the right of the question. Do NOT type units into the answer boxes, type only the numeric values. Do NOT use commas or scientific notation when entering large numbers. Answer all non-integer questions to at least 3 significant figures. For each of the following, determine if the entropy change is negative or positive: a.

Li s Fe s Hg s All are in their standard state b.

Enthalpy And Entrophy

Cl 2 g I 2 s Br 2 l All are in their standard state c. As l Kr g Sn s All are in their standard state d. H 2 g He 2 g F 2 g All are in their standard state For each of the following, determine which which system has the greatest entropy of formation: a. C 5 H 12 l at K C 6 H 14 l at K C 7 H 16 l at K All have the same entropy of formation For each of the following, determine which thermodynamic value best describes the situation: a.

An endothermic system. A system becomes more ordered. An exothermic system. A system undergoing a spontaneous process. A system becomes more randomized. A system undergoing a nonspontaneous process. An endothermic process that orders the system.

Never spontaneous Spontaneous at low temperature Spontaneous at high temperature Always spontaneous b. An exothermic process that randomizes the system. Never spontaneous Spontaneous at low temperature Spontaneous at high temperature Always spontaneous c. An endothermic process that randomizes the system. Never spontaneous Spontaneous at low temperature Spontaneous at high temperature Always spontaneous d. An exothermic process that orders the system.At what temperature will it change from spontaneous to non-spontaneous?

Approximately K. If the reaction quotient Q is greater than the equilibrium constant Kwhat is true about the Gibbs free energy? If Q is greater than K, the reaction has exceeded the equilibrium state. The reaction will be spontaneous if and only if the magnitude of the enthalpy is greater than the magnitude of the entropy times the temperature. The reaction will be spontaneous if and only if the magnitude of the enthalpy is greater than the magnitude of the entropy.

entropy practice worksheet

The reaction will be spontaneous if and only if the magnitude of the entropy is greater than the magnitude of the enthalpy times the temperature. Ifthe enthalpy, andthe entropy, are both negative, then the reaction will be spontaneous if and only if the magnitude of the enthalpy is greater than the magnitude of the entropy times the temperature.

The Gibb's free energy equation is used to determine the spontaneity of a reaction and is written as follows:. In order for a reaction to be spontaneous, Gibb's free energy must have a negative value.

Based on the equation, we can see that a positive enthalpy in combination with a negative entropy will always result in a positive value for Gibb's free energy. A reaction is spontaneous when Gibb's free energy is negative. As a result, we need to determine the temperature range where Gibb's free energy is less than zero.

Since we know the values for changes in enthalpy and entropy, we can plug them into the Gibb's free energy equation, and set it equal to zero. Since entropy is positive for this reaction, increasing the temperature will result in a more negative value for Gibb's free energy.

A galvanic cell results in a positive cell potential from a spontaneous reaction. Spontaneous reactions always have a negative Gibb's free energy.

Worksheet: Gibbs Free Energy

An equilibrium constant greater than one would indicate that the equilibrium concentration of products is greater than the equilibrium concentration of reactants, consistent with a spontaneous reaction.

We are given the constant value and the cell potential. The moles of electrons transferred is equal to the change in charge on the atoms in the reaction.

entropy practice worksheet

In this reaction, copper is reduced from a charge of to zero, requiring that is gained two moles of electrons. Notice that the value is negative. Galvanic cells are spontaneous, and will have negative Gibb's free energies at standard conditions.In this worksheet, we will practice calculating the change in the entropy of a system that results from various thermodynamic processes.

A cube of ice with a mass of fifty grams and at a temperature of 0. What is the change in entropy of the water in this process? What is the entropy change of the reservoir? A system consisting of The initial temperature of the gas was K. What is the change in entropy of the gas? Take universal gas constant to be 8. An ideal gas at a temperature of 3. Determine the entropy change per mole of the gas. A copper rod of cross-sectional area 5.

A piece of aluminum of mass 0.

Worksheet: Entropy Change in a Thermodynamic Process

The aluminum is dropped into a 1. After equilibrium is reached, what is the net entropy change of the system? A mass of water of g that has a temperature of 0. For the Carnot cycle in the figure, consider the efficiency to be 0. A rock of mass 4. Assume that the drag on the rock from the air is negligible. Calculate the change in entropy of the water in this process.

In an isochoric process, 5. What is the entropy change of the gas due to the heating?The following are common thermodynamic equations and sample problems showing a situation in which each might be used. How many liters of water can 6. The initial temperature and pressure of the ethane and water is 0. First we must find the amount of heat released by the ethane.

To do this, we calculate the number of moles of ethane gas using the ideal gas equation and multiply the molar heat of combustion by the number of moles. Then using the heat equation we can find the mass of water that would be raised to boiling with the given amount of heat. First, the kJ must be converted to J to match the units of the specific heat. Using basic algebra we solve for the mass, and since water has a density of 1.

A balloon filled with gas expands its volume by 2. If the pressure outside the balloon is 0. The specific heat capacity of copper is We now know how many joules of heat must be added to the copper wire to increase the temperature and we know how many joules of energy are given off by the heater per second. We divide to find the number of seconds. T 1 and T 2 refer to the temperatures in Kelvin. The heat of vaporization of liquid water is The gas constant that is most convenient to use is 8.

Therefore it is important to convert the kJ value of the heat of vaporization to J. Given a Carnot engine that absorbs J of energy from a tank of hot water with a final temperature of K, what is the initial temperature if J of work was done by the system? Using the ideal gas law and knowing four of the five variables, it is possible to solve for the fifth variable.

It is important to note that while the equation is mostly correct, but it is only perfectly accurate if the gas is ideal.


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