5. What occurs when solid A, at 50.0°C, is place in liquid B, at 80.0°C? A Heat energy flows from A to B as the average kinetic energy of the particles in A decreases B Heat energy flows from A to B as the average kinetic energy of the particles in A increases C Heat energy flows from B to A as the average kinetic energy of the particles in B decreases D Heat energy flows from B to A as the average kinetic energy of the particles in B increases

5. What occurs when solid A, at 50.0°C, is place in liquid B, at 80.0°C? A Heat energy flows from A to B as the average kinetic energy of the particles in A decreases B Heat energy flows from A to B as the average kinetic energy of the particles in A increases C Heat energy flows from B to A as the average kinetic energy of the particles in B decreases D Heat energy flows from B to A as the average kinetic energy of the particles in B increases

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.63QE: A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form...

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9.45 What happens to the temperature of a material as it undergoes an endothermic phase change? If heat is added, how can the temperature behave in this manner?
9.95 How much heat is required to convert 250 g of water from liquid at 23°C: into steam at 107°C? (The necessary heat capacities and enthalpy changes can be found in the chapter or online.)
Gas A2 reacts with gas B2 to form gas AB at a constant temperature. The bond energy of AB is much greater than that of either reactant. What can be said about the sign of H? SSurr? S? Explain how potential energy changes for this process. Explain how random kinetic energy changes during the process.
9.41 Under what conditions does the enthalpy change equal the heat of a process?
Use Appendix L to find the standard enthalpies of formation of oxygen atoms, oxygen molecules (O2), and ozone (O3). What is the standard state of oxygen? Is the formation of oxygen atoms from O2 exothermic? What is the enthalpy change for the formation of 1 mol of O3 from O2?
Draw a diagram like Figure 2.11 that illustrates the change in enthalpy for the chemical reaction C s 2H2 g CH4 g Which is exothermic by 74.8 kJ/mol.
n Section 10.7, two characteristics of enthalpy changes for reactions are listed. What are these characteristics? Explain why these characteristics are true.
An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?
For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7kJ: a.What quantity of heat is required to produce 1 mole of mercury by this reaction? b.What quantity of heat is required to produce 1 mole of oxygen gas by this reaction? c.What quantity of heat would be released in the following reaction as written? 2Hg(l) + O2(g) 2HgO(s)
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9.49 Hvap=31.3 kJ/mol for acetone. If 1.40 kg of water were vaporized to steam in a boiler, how much acetone (in kg) would need to be vaporized to use the same amount of heat?