A battery harnesses a chemical reaction to extract energy in the form of useful electrical work. (a) A certain battery runs a toy truck and becomes par- tially discharged. In the process, it performs a total of 117.0 J of work on its immediate surroundings. It also gives off 3.0 J of heat, which the surroundings absorb. No other work or heat is exchanged with the sur- roundings. Compute q, w, and AU of the battery, making sure each quantity has the proper sign. (b) The same battery is now recharged exactly to its origi- nal condition. This requires 210.0 J of electrical work from an outside generator. Determine q for the battery in this process. Explain why q has the sign that it does.

A battery harnesses a chemical reaction to extract energy in the form of useful electrical work. (a) A certain battery runs a toy truck and becomes par- tially discharged. In the process, it performs a total of 117.0 J of work on its immediate surroundings. It also gives off 3.0 J of heat, which the surroundings absorb. No other work or heat is exchanged with the sur- roundings. Compute q, w, and AU of the battery, making sure each quantity has the proper sign. (b) The same battery is now recharged exactly to its origi- nal condition. This requires 210.0 J of electrical work from an outside generator. Determine q for the battery in this process. Explain why q has the sign that it does.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

When 18.5 g of HgO(s) is decomposed to form Hg(l) and O2(g), 7.75 kJ of heat is absorbed at standard-state conditions. What is the standard enthalpy of formation (ΔH°f) of HgO(s)?
Ammonium dichromate is sometimes known as Vesuvian Fire, because of its use in demonstrations of tabletop "volcanoes". Using the given data, calculate the heat of reaction for the following reaction: (NH4)½Cr207(s) –→ Cr2O3(s) + N½(g) +4H,O(g) AH (k mol) AG U mol K) ... Species mol") Nitrogem Ng) 191.5 Ng) NH,(g) 472.704 153.19 455.579 -46.11 192.3 -16.5 NH,(aq) NH,"(aq) - 80.29 III.3 -26.50 -132.51 113.4 -79.31 N,HC) 50.63 121.2 149.2 (NH),AsO/aq) -1268 NH,Br(s) -270.83 113 -175.2 NH,C6) NH,Caq) NH,HCO,6) -314.4 94.6 -201.5 -300.2 -847 12.1 -666 NH,I(s) -201.4 117 -113 NH,NO,) -3656 151.1 -184.0 (NH),SO) -1180.85 220.1 -901.67 NF(g) NO(g) NOg) -125 260.6 -83.3 90.25 210.7 86.57 33.2 240.0 31.30 N,Og) 82.05 219.7 104.2 N,O,(g) 83.72 321.28 139.46 N,Odg) 9.16 304.2 97.82 N,O(g) 356 115 -43.1 178 114 NOCIG) 52.59 264 66.36 HNO(0 -174.1 155.6 -80.79 HNO(g) -135.1 266.2 -74.77 HNO, (aq) -206.6 146 -110.5 Hydrogen H(g) 218.0 114.6 203.3 H(g) H,O() 130.6 -285.8 69.91 -237.2 -241.8 188.7…
A cylinder of volume 0.270 m3 contains 10.1 mol of neon gas at 17.7°C. Assume neon behaves as an ideal gas. (a) What is the pressure of the gas? Pa (b) Find the internal energy of the gas. (c) Suppose the gas expands at constant pressure to a volume of 1.000 m3. How much work is done on the gas? (d) What is the temperature of the gas at the new volume? (e) Find the internal energy of the gas when its volume is 1.000 m3. (f) Compute the change in the internal energy during the expansion. (g) Compute AU - W. (h) Must thermal energy be transferred to the gas during the constant pressure expansion or be taken away?
1a only
Define standard enthalpy of formation (AH?;).
When chemical A and chemical B are mixed together, and endothermic reaction below occurs:4A(aq) + 3B(s) --> 2C(aq)To find the enthalpy of this reaction, a scientist pours 155 mL of a 0.33 M solution A into abeaker and measures the temperature to be 20.1 ̊C. To this same beaker the scientist thenadds 3.75 g of substance B with stirring (molar mass of B is 33 g/mol), and finds thetemperature to now be 16.3 ̊C. Calculate the molar enthalpy of this reaction for every mole ofC produced.
Please answer it. Thanks!
The metabolism of glucose, C6H12O6, produces H2O (l) and CO2 (g). The heat released in the process is converted into useful work with an efficiency of 70%. Calculate the mass of glucose metabolized by a 58.0 kg person when climbing a mountain with a summit of 1450 m. Suppose the work done on the ascent is four times that of just lifting 58.0 kg from 1450 m. (ΔfHom (glucose) = - 1273.3 kJ / mol).
It has been determined that the body can generate 5500 k) of energy during one hour of strenuous exercise. Perspiration is the body's mechanism for eliminating this heat. What mass of water would have to be evaporated through perspiration to rid the body of the heat generated during 4 hours of exercise? (The heat of vaporization of water is 40.6 kJ/mol.) Mass = kg
Q5 a)A chemical reaction is run in which 465 Joules of heat are generated and the internal energy changes by -27 Joules. Calculate w for the system. w = Joules b)A chemical reaction is run in which 571 Joules of work is done by the system and the internal energy changes by + 95 Joules. Calculate q for the system. q = Joules c)A chemical reaction is run in which 365 Joules of heat are generated and 390 Joules of work are done by the system. Calculate the change in the internal energy of the chemical system.U = Joules
How much work (energy) is required to lift a 173 g object by a height of 71.0 feet? The earth's gravitational constant is g = 9.80 m/s2.
As a routine safety procedure, acids and bases should be stored separately in a laboratory. Concentrated hydrochloric acid is 12.0 M and the molarity of 25% ammonium hydroxide is 13.4 M. Both are sold in 2.50L bottles. If there were an accident and the two bottles broke and the acid and base mixed, how much heat would evolve? State your answer as a positive value. NH4OH(aq) + HCI(aq) → NH4CI(aq) + H2O(1) AH° = -50.49 kJ Heat = ! kJ %3D