Please don't provide handwritten solution ..... Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can.ChangeIs this change spontaneous?O Yes.O No.A gas condenses to a liquid, neither absorbing nor releasing heat.O Can't decide with information given.Two liquids mix, neither absorbing nor releasing heat.Yes.O No.O Can't decide with information given.During an exothermic chemical reaction, four moles of gaseous reactants areturned into two moles of gaseous products.O Yes.O No.O Can't decide with information given.X

Step 1:A spontaneousreactionis one that, in the specific circumstances of the reaction, favors the…

Answered: Read the descriptions of physical or…

Living By Chemistry: First Edition Textbook

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ChapterU5: Fire: Energy , Thermodynamics, And Oxidation-reduction

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Problem 15RE

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9.20 State the first law of thermodynamics briefly in your own words.
The second law of thermodynamics is sometimes paraphrased as: you can't break even. Explain. Because energy cannot be created out of nothing. Because some energy is lost in all energy transactions. Because some energy is gained in all energy transactons.
You have a large balloon containing 1.0 mol of gaseous water vapor at 80 C. How will each step affect the internal energy of the system? (a) The temperature of the system is raised to 90 C. (b) The vapor is condensed to a liquid, at 40 C.
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.
Athletic trainers use instant ice packs that can be cooled quickly on demand. Squeezing the pact breaks an inner container, allowing two components to mix and react. This reaction makes the pack become cold. Describe the heat flow for this spontaneous process.
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.
An exothermic reaction is carried out in a coffee-cup calorimeter. Which of the following statements is/are NOT true for the process? (a) The temperature of the water increases. (b) Heat is absorbed by the water. (c) The enthalpy of the products is higher than the enthalpy of the reactants. (d) qH2o=qrxn (e) qrxn0 (f) qrxn+qH2o=0
Draw a cylinder with a movable piston containing six molecules of a liquid. A pressure of 1 atm is exerted on the piston. Next draw the same cylinder after the liquid has been vaporized. A pressure of one atmosphere is still exerted on the piston. Is work done on the system or by the system?
xplain why aluminum cans make good storage containers for soft drinks. Styrofoam cups can be used to keep coffee hot and cola cold. How can this be?
Coal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.
9.58 For the reaction C2H2(g)+2H2(g)C2H6,H=136 kJ. What are the ratios that can be defined between moles of substances and energy?
One statement of the second law of thermodynamics is that heat cannot be turned completely into work. Another is that the entropy of the universe always increases. How are these two statements related?

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