goodmorning,, please do help me with my exercises please... because I will study this later.. thank you. I.Matching Type1. energy at motiona. Potential energyb. Second law of2. Energy is neither created nor destroyed3. Work done on the system4. Energy at restThermodynamicsc. Internal energyd. +95. physical property of a material that measures howmuch heat is required to raise the temperature of onegram of that material by 1 K6. Total Kinetic energy + Total Potential Energye. - 9f. Specific heat capacityg. Kinetic energy7. Heat added to the systemh. First law ofThermodynamicsi.- Wj.k. Molar heat capacity+ w

Answered: Image /qna-images/answer/b45413b9-08c8-45c9-bbed-98111cf1665f.jpg

I. Matching Type 1. energy at motion a. Potential energy b. Second law of 2. Energy is neither created nor destroyed 3. Work done on the system Thermodynamics c. Internal energy 4. Energy at rest 5. physical property of a material that measures how much heat is required to raise the temperature of one gram of that material by 1 K 6. Total Kinetic energy + Total Potential Energy d. +9 e. - 9 f. Specific heat capacity g. Kinetic energy 7. Heat added to the system h. First law of Thermodynamics i. - W j. k. Molar heat capacity + w

I. Matching Type 1. energy at motion a. Potential energy b. Second law of 2. Energy is neither created nor destroyed 3. Work done on the system Thermodynamics c. Internal energy 4. Energy at rest 5. physical property of a material that measures how much heat is required to raise the temperature of one gram of that material by 1 K 6. Total Kinetic energy + Total Potential Energy d. +9 e. - 9 f. Specific heat capacity g. Kinetic energy 7. Heat added to the system h. First law of Thermodynamics i. - W j. k. Molar heat capacity + w

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 11P

See similar textbooks

Similar questions

A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J/C g) are heated to 100.0C. The mixture of hot iron and aluminum is then dropped into 97.3 g water at 22.0C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
Define the terms system and surroundings. What does it mean to say that a system and its surroundings are in thermal equilibrium?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
The statement Energycan beneithercreatednor destroyedis sometimes used as an equivalent statement of the first law of thermodynamics. There areinaccuracies to the statement, however. Restate it tomake it less inaccurate.
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
Microwave ovens convert radiation to energy. A microwave oven uses radiation with a wavelength of 12.5 cm. Assuming that all the energy from the radiation is converted to heat without loss, how many moles of photons are required to raise the temperature of a cup of water (350.0 g, specific heat =4.18J/gC) from 23.0C to 99.0C?
Explain in your own words what is meant by the term entropy. Explain how both matter spread and energy spread are related to the concept of entropy.
9.42 Why is enthalpy generally more useful than internal energy in the thermodynamics of real world systems?
9.11 Analyze the units of the quantity (pressurevolume) and show that they are energy units, consistent with the idea of PV-work.
When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added to 100.0 g of 0.100 M AgNO3(aq) at 24.1 C in a calorimeter, the temperature increases to 25.2 C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat in joules produced.
Consider the combustion of propane: C3H8(g)+5O2(g)3CO2(g)+4H2O(l)H=2221KJ Assume that all the heat in Example 7-3 comes from the combustion of propane. What mass of propane must be burned to furnish this amount of energy assuming the heat transfer process is 60.% efficient?