Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 10, Problem 10.35PAE
What happens to the entropy of the universe during a spontaneous process?
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Chapter 10 Solutions
Chemistry for Engineering Students
Ch. 10 - Prob. 1COCh. 10 - . explain the concept of entropy in your own...Ch. 10 - Prob. 3COCh. 10 - . state the second law of thermodynamics in words...Ch. 10 - Prob. 5COCh. 10 - Prob. 6COCh. 10 - Prob. 7COCh. 10 - Prob. 8COCh. 10 - Prob. 9COCh. 10 - Prob. 10CO
Ch. 10 - Prob. 10.1PAECh. 10 - Prob. 10.2PAECh. 10 - Prob. 10.3PAECh. 10 - Prob. 10.4PAECh. 10 - Prob. 10.5PAECh. 10 - Use the web to learn how many pounds of plastics...Ch. 10 - On the basis of your experience, predict which of...Ch. 10 - In the thermodynamic definition of a spontaneous...Ch. 10 - 1f the combustion of butane is spontaneous, how...Ch. 10 - Identify each of the processes listed as...Ch. 10 - Identify each of the processes listed as...Ch. 10 - Athletic trainers use instant ice packs that can...Ch. 10 - Are any of the following exothermic processes not...Ch. 10 - Enthalpy changes often help predict whether or not...Ch. 10 - When a fossil fuel burns, is that fossil fuel the...Ch. 10 - Murphy's law is a whimsical rule that says that...Ch. 10 - Prob. 10.17PAECh. 10 - Prob. 10.18PAECh. 10 - Prob. 10.19PAECh. 10 - Some games include dice with more than six sides....Ch. 10 - How does probability relate to spontaneity?Ch. 10 - Prob. 10.22PAECh. 10 - For each pair of items, tell which has the higher...Ch. 10 - Prob. 10.24PAECh. 10 - Prob. 10.25PAECh. 10 - For each process, tell whether the entropy change...Ch. 10 - Without doing a calculation, predict whether the...Ch. 10 - For the following chemical reactions, predict the...Ch. 10 - Prob. 10.29PAECh. 10 - Prob. 10.30PAECh. 10 - Prob. 10.31PAECh. 10 - Prob. 10.32PAECh. 10 - According to Lambert, leaves lying in the yard and...Ch. 10 - Prob. 10.34PAECh. 10 - What happens to the entropy of the universe during...Ch. 10 - Prob. 10.36PAECh. 10 - One statement of the second law of thermodynamics...Ch. 10 - Prob. 10.38PAECh. 10 - How does the second law of thermodynamics explain...Ch. 10 - Prob. 10.40PAECh. 10 - Prob. 10.41PAECh. 10 - Which reaction occurs with the greater increase in...Ch. 10 - Which reaction occurs with the greater increase in...Ch. 10 - Methanol is burned as fuel in some race cars. This...Ch. 10 - Limestone is predominantly CaCO3, which can...Ch. 10 - Suppose that you find out that a system has an...Ch. 10 - Use tabulated thermodynamic data to calculate the...Ch. 10 - Prob. 10.48PAECh. 10 - Calculate S for the dissolution of magnesium...Ch. 10 - Calculate the standard entropy change for the...Ch. 10 - Through photosynthesis, plants build molecules of...Ch. 10 - Find websites describing two different attempts to...Ch. 10 - Prob. 10.53PAECh. 10 - Prob. 10.54PAECh. 10 - A beaker of water at 400 C(on the left in the...Ch. 10 - Describe why it is easier to use Gto determine the...Ch. 10 - Under what conditions does G allow us to predict...Ch. 10 - There is another free energy state function, the...Ch. 10 - 10.45 Calculate G at 45°C for reactions for which...Ch. 10 - 10.46 Discuss the effect of temperature change on...Ch. 10 - The reaction CO2(g)+H2(g)CO(g)+H2O(g) is not...Ch. 10 - Prob. 10.62PAECh. 10 - Prob. 10.63PAECh. 10 - For the reaction NO(g)+NO2(g)N2O3(g) , use...Ch. 10 - 10.51 The combustion of acetylene was used in...Ch. 10 - Natural gas (methane) is being used in...Ch. 10 - Silicon forms a series of compounds analogous to...Ch. 10 - Explain why Gf of O2 (g) is zero.Ch. 10 - Using tabulated thermodynamic data, calculate G...Ch. 10 - Using tabulated thermodynamic data, calculate G...Ch. 10 - Calculate G for the dissolution of both sodium...Ch. 10 - Phosphorus exists in multiple solid phases,...Ch. 10 - 10.59 The normal melting point of benzene, C6H6,...Ch. 10 - Prob. 10.74PAECh. 10 - Estimate the temperature range over which each of...Ch. 10 - Recall that incomplete combustion of fossil fuels...Ch. 10 - During polymerization, the system usually becomes...Ch. 10 - Prob. 10.78PAECh. 10 - Prob. 10.79PAECh. 10 - The recycling of polymers represents only one...Ch. 10 - Diethyl ether is a liquid at normal temperature...Ch. 10 - Calculate the entropy change, S , for the...Ch. 10 - Gallium metal has a melting point of 29.8°C. Use...Ch. 10 - Methane can be produced from CO and H2.The process...Ch. 10 - 10.85 Iodine is not very soluble in water, but it...Ch. 10 - The enthalpy of vaporization for water is 40.65 kJ...Ch. 10 - Determine whether each of the following statements...Ch. 10 - Nickel metal reacts with carbon monoxide to form...Ch. 10 - Polyethylene has a heat capacity of 2,3027 J g-1...Ch. 10 - A key component in many chemical engineering...Ch. 10 - The reaction shown below is involved in the...Ch. 10 - Using only the data given below, determine G for...Ch. 10 - The graph below shows G as a function of...Ch. 10 - Prob. 10.94PAECh. 10 - Prob. 10.95PAECh. 10 - Prob. 10.96PAECh. 10 - Prob. 10.97PAECh. 10 - Prob. 10.98PAECh. 10 - Thermodynamics provides a way to interpret...Ch. 10 - Prob. 10.100PAECh. 10 - 10.101 Fluorine reacts with liquid water to form...Ch. 10 - 10.102 Ammonia can react with oxygen gas to form...Ch. 10 - Prob. 10.103PAECh. 10 - 10.104 (a) When a chemical bond forms, what...
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- For each process, tell whether the entropy change of the system is positive or negative. Water vapor (the system) deposits as ice crystals on a cold windowpane. A can of carbonated beverage loses its fizz. (Consider the beverage but not the can as the system. What happens to the entropy of the dissolved gas?) A glassblower heats glass (the system) to its softening temperature.arrow_forwardWhat is entropy? Why is entropy important?arrow_forwardDefine the term entropy, and give an example of a sample of matter that has zero entropy. What are the units of entropy? How do they differ from the units of enthalpy?arrow_forward
- 9.20 State the first law of thermodynamics briefly in your own words.arrow_forwardOne 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?arrow_forwardAthletic 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.arrow_forward
- 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.arrow_forwardDefine the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universearrow_forwardCoal 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.arrow_forward
- What are the two ways that a final chemical state of a system can be more probable than its initial state?arrow_forwardExplain 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.arrow_forwardWhen a rocket is launched, the burning gases are the source of the motion. If the system is the rocket (including fuel), what is the sign of the work?arrow_forward
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