MASTERING CHEMISTRY:THE CENTRAL SCIENCE
13th Edition
ISBN: 9781269712538
Author: Brown
Publisher: PEARSON
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Textbook Question
Chapter 5.7, Problem 5.12.2PE
Practice Exercise 2
Use Table 5.3 to calculate the enthalpy change for the combustion of 1 mol of ethanol:
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Practice Exercise 2
Write the equation corresponding to the standard enthalpy of
formation of liquid carbon tetrachloride (CCI4) and look up
AH for this compound in Appendix C.
Practice Exercise 1If the heat of formation of H2O1l2 is -286 kJ>mol, whichof the following thermochemical equations is correct?(a) 2 H1g2 + O1g2¡H2O1l2 ΔH = -286 kJ(b) 2 H21g2 + O21g2¡2 H2O1l2 ΔH = -286 kJ(c) H21g2 + 12 O21g2¡H2O1l2 ΔH = -286 kJ(d) H21g2 + O1g2¡H2O1g2 ΔH = -286 kJ(e) H2O1l2¡H21g2 + 12O21g2 ΔH = -286 kJ
Practice
TEXT ANSWER
A calorimeter holds 75 g water at 24.0°C. A sample of hot
silver is added to the water. The final temperature of the
water and silver is 28.0°C. What is the change in enthalpy
associated with the change in the water's temperature?
J
FC
Note: The specific heat of water is 4.18 gº
Use the formula ΔΗ = = - cm ^T
Show your work.
H
Normal
X₂ X²
2 Ix
Enter your answer here
:
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Chapter 5 Solutions
MASTERING CHEMISTRY:THE CENTRAL SCIENCE
Ch. 5.2 - Prob. 5.1.1PECh. 5.2 - Prob. 5.1.2PECh. 5.3 - Prob. 5.2.1PECh. 5.3 - Prob. 5.2.2PECh. 5.3 - Prob. 5.3.1PECh. 5.3 - Prob. 5.3.2PECh. 5.4 - Prob. 5.4.1PECh. 5.4 - Prob. 5.4.2PECh. 5.5 - Prob. 5.5.1PECh. 5.5 - Prob. 5.5.2PE
Ch. 5.5 - Practice Exercise 1 Suppose you have equal masses...Ch. 5.5 - Prob. 5.6.2PECh. 5.5 - Prob. 5.7.1PECh. 5.5 - Prob. 5.7.2PECh. 5.6 - Prob. 5.8.1PECh. 5.6 - Prob. 5.8.2PECh. 5.6 - Prob. 5.9.1PECh. 5.6 - Prob. 5.9.2PECh. 5.7 - Prob. 5.10.1PECh. 5.7 - Prob. 5.10.2PECh. 5.7 - Prob. 5.11.1PECh. 5.7 - Prob. 5.11.2PECh. 5.7 - Prob. 5.12.1PECh. 5.7 - Practice Exercise 2 Use Table 5.3 to calculate the...Ch. 5.8 - Prob. 5.13.1PECh. 5.8 - Practice Exercise 2 Given the following standard...Ch. 5.8 - Prob. 5.14.1PECh. 5.8 - Prob. 5.14.2PECh. 5 - Prob. 1DECh. 5 - Prob. 1ECh. 5 - Prob. 2ECh. 5 - Prob. 3ECh. 5 - Practice Exercise 2
Using Table 20.1, rank...Ch. 5 - Prob. 5ECh. 5 - Prob. 6ECh. 5 - Prob. 7ECh. 5 - Prob. 8ECh. 5 - Prob. 9ECh. 5 - Prob. 10ECh. 5 - Prob. 11ECh. 5 - Prob. 12ECh. 5 - Prob. 13ECh. 5 - Prob. 14ECh. 5 - Prob. 15ECh. 5 - Prob. 16ECh. 5 - Prob. 17ECh. 5 - Prob. 18ECh. 5 - Prob. 19ECh. 5 - Prob. 20ECh. 5 - Prob. 21ECh. 5 - Prob. 22ECh. 5 - Prob. 23ECh. 5 - Prob. 24ECh. 5 - Prob. 25ECh. 5 - Prob. 26ECh. 5 - Prob. 27ECh. 5 - In chemical kinetics, the entropy of activation is...Ch. 5 - Prob. 29ECh. 5 - Prob. 30ECh. 5 - Prob. 31ECh. 5 - The following data compare the standard enthalpies...Ch. 5 - Prob. 33ECh. 5 - Prob. 34ECh. 5 - Prob. 35ECh. 5 - What is the reducing agent in the following...Ch. 5 - Prob. 37ECh. 5 - Prob. 38ECh. 5 - Prob. 39ECh. 5 - Prob. 40ECh. 5 - Prob. 41ECh. 5 - Prob. 42ECh. 5 - Prob. 43ECh. 5 - The standard cell potential is 1.46 V for a...Ch. 5 - Prob. 45ECh. 5 - Prob. 46ECh. 5 - Prob. 47ECh. 5 - Prob. 48ECh. 5 - Prob. 49ECh. 5 - Practice Exercise 1
Which of the following...Ch. 5 - Prob. 51ECh. 5 - Prob. 52ECh. 5 - Prob. 53ECh. 5 - Prob. 54ECh. 5 - Prob. 55ECh. 5 - Prob. 56ECh. 5 - Prob. 57ECh. 5 - Prob. 58ECh. 5 - Prob. 59ECh. 5 - Prob. 60ECh. 5 - What is the connection between Hess’s law and the...Ch. 5 - Prob. 62ECh. 5 - 20.2 You may have heard that “antioxidants” are...Ch. 5 - Prob. 64ECh. 5 - Prob. 65ECh. 5 - Prob. 66ECh. 5 - Prob. 67ECh. 5 - Prob. 68ECh. 5 - Prob. 69ECh. 5 - Prob. 70ECh. 5 - Prob. 71ECh. 5 - Prob. 72ECh. 5 - 20.13
What is meant by the term oxidation?
On...Ch. 5 - Prob. 74ECh. 5 - Prob. 75ECh. 5 - Prob. 76ECh. 5 - Prob. 77ECh. 5 - Prob. 78ECh. 5 - Prob. 79ECh. 5 - Prob. 80ECh. 5 - Prob. 81ECh. 5 - Prob. 82ECh. 5 - Prob. 83ECh. 5 - Prob. 84ECh. 5 - Prob. 85ECh. 5 - The heat of combustion of ethanol, C2H5OH(l) is...Ch. 5 - Prob. 87ECh. 5 - Prob. 88ECh. 5 - Prob. 89ECh. 5 - The automobile fuel called E85 consists of 85%...Ch. 5 - Prob. 91AECh. 5 - Prob. 92AECh. 5 - Prob. 93AECh. 5 - Prob. 94AECh. 5 - 5.95 Consider a system consisting of the following...Ch. 5 - A sample of gas is contained in a...Ch. 5 - Prob. 97AECh. 5 - Prob. 98AECh. 5 - A house is designed to have passive solar energy...Ch. 5 - Prob. 100AECh. 5 - Prob. 101AECh. 5 - Prob. 102AECh. 5 - Burning methane in oxygen can produce three...Ch. 5 - Prob. 104AECh. 5 - Prob. 105AECh. 5 - The hydrocarbons acetylene (C2H2) and benzene...Ch. 5 - Prob. 107AECh. 5 - Three common hydrocarbons that contain four...Ch. 5 - Prob. 109AECh. 5 - The Sun supplies about 1.0 kilowatt of energy for...Ch. 5 - It is estimated that the net amount of carbon...Ch. 5 - Prob. 112IECh. 5 - Prob. 113IECh. 5 - Prob. 114IECh. 5 - Prob. 115IECh. 5 - Prob. 116IECh. 5 - Prob. 117IECh. 5 - The methane molecule, CH4, has the geometry shown...Ch. 5 - Prob. 119IE
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- Need help in chemistry problemarrow_forwardHomework 3 • Use standard enthalpies of formation from Table 7.2 to determine the enthalpy change at 25 °C for the following reaction. 2 Cl2(g) + 2H20(1) 4 HCI( g) + O2(g) AH° = ?arrow_forwardPractice Exercise 2 Carbon occurs in two forms, graphite and diamond. The en- thalpy of the combustion of graphite is -393.5 kJ /mol, and that of diamond is -395.4 kJ/mol: C(graphite) + O2(g) → CO2(8) AH = -393.5 kJ - C(diamond) + O2(8) CO2(8) AH = -395.4 kJ - %3D Calculate AH for the conversion of graphite to diamond: C(graphite) C(diamond) AH = ? - %3Darrow_forward
- Course dashboard A bomb calorimetry experiment is performed with xylose, C5H1005 (s), as the combustible substance. The data obtained are mass of xylose burned: 2.059g, heat capacity of calorimeter 4.728 kJ/ C, initial calorimeter temperature: 23.29°C; final calorimeter temperature 27.19°C. What is the heat of combustion of xylose, in kilojoules di per mole? aretle Lütfen birini seçin: O a. -2.38x103 kJ/mol b. -2.17x103 kJ/mol Uy O c. -5.64x10 kJ/mol Ka d. -1.82x103 kJ/mol O e. -1.34x103 kJ/molarrow_forwardSuppose 33 mL of 1.20 M HCl is added to 42 mL of a solution containing excess sodium hydroxide, NaOH, in a coffee-cup calorimeter. The solution temperature, originally 25.0C, rises to 31.8C. Give the enthalpy change, H, for the reaction: HCl(aq)+NaOH(aq)NaCl(aq)+H2O(l) Express the answer as a thermochemical equation. For simplicity, assume that the heat capacity and the density of the final solution in the cup are those of water. (In more accurate work, these values must be determined.) Also assume that the total volume of the solution equals the sum of the volumes of HCl(aq) and NaOH(aq).arrow_forwardA gas is enclosed in a system similar to that shown in Figure 6.9. More weights are added to the piston, giving a total mass of 2.20 kg. As a result, the gas is compressed, and the weights are lowered 0.250 m. At the same time, 1.50 J of heat evolves from the system. What is the change in internal energy of the system, U? The force of gravity on a mass m is mg, where g is the constant acceleration of gravity (g = 9.81 m/s2).arrow_forward
- number 3arrow_forwardPractice Exercise 1 Calculate AH for 2 NO(g) + O2(g) → N204(8), using the following information: N2O4(8) → 2 NO2(g) AH = +57.9 kJ %3D 2 NO(8) + O2(g) → 2 NO2(8) AH = -113.1 kJ %3D (a) 2.7 kJ (b) –55.2 kJ (c) –85.5 kJ (d) –171.0 kJ (e) +55.2 kJarrow_forwardExercise #96 Calculate the enthalpy of reaction, AHn, for the reaction between hydrogen chloride gas and fluorine using the reactions provided below. 4 HCI(g) + O,(g) → 2 H,O(1) + 2 Cl,(g) AH = -148.4 kJ AH = -285.8 kJ H2(g) + ½ O2(g) → H2O(1) AH = 600.0 kJ %3D HF(1) → ½ H2(g) + ½ F2(g) 2 HCI(g) + F2(g) 2 HF(1) + Cl, (g)arrow_forward
- E Knowledge Check Question 3 A chemist carefully measures the amount of heat needed to raise the temperature of a 1.75 kg sample of a pure substance from 22.2 °C to 45.4 °C. The experiment shows that 170. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits. -1 - 1 了.g ·K x10 I Don't Know Submit 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy CenterI IMG-4686.jpg Spring 2022 Sc....html Spring 2022 Sc....htmlarrow_forwardA common misconception is that the following chemical reaction occurs when water is boiled: 2H2O(l)2H2(g)+O2(g) instead of H2O(l)H2O(g) a What evidence do you have that the second reaction is correct? b How would the enthalpy of the wrong reaction compare with that of the correct reaction? c How could you calculate the enthalpy change for the wrong reaction (Chapter 6)?arrow_forwardRule: Do it with students and not for them Exercise 3 Calculate the change in enthalpy for the reaction of one mole of PbO2 from lead and oxygen at 550°C. Given: 1 Pb+ 02PbO, AH 298 = -219242 J.mol-1 Pb 3PbO + +10 0₂ = Pb304, AH 298 -76986 J.mol-1 PbO Pb304023PbO2, AH 298 -94977 J.mol-1 02 = Cp(Pb) 38.4 + 1.9 × 10-3T Cp(02) 28.6 +1.4 × 10-3T - 8.4 × 105T-2 = Cp(Pb) 76.2 4.6 × 10-³Tarrow_forward
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