12:52 Sun, 16 June bb.Question 8IncorrectMark 0.00 outof 1.00Remove flagGiven the equationH2O(l) → H2O(g) AH = 40.7 kJ (at 100 °C)Calculate the heat required to convert 3.00grams of liquid water (H2O(l)) at 100 °C to vapor(H2O(g)).a.1254 JOb. 122.1 kJ xC.6.78 kJd. 6078 kJYour answer is incorrect.The correct answer is:6.78 kJ16...bL བ༥.53% ☁=о

Answered: 12:52 Sun, 16 June bb. Question 8…

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...

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1. Determine the amount of heat required to convert 500.0 g of liquid ethanol at 25.0°C into gaseous ethanol at 125°C. Use the following information on ethanol (CHOH) to calculate the amount of heat for each of the steps.Melting Point = −117°C Boiling Point = 78.3°C Molar Heat Capacities:C =113 J/mol °CC = 420 J/mol °CΔH = 5.02 kJ/molΔH = 39.3 kJ/mol Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a. 507.7 kJ b. 493.7 kJ c. 707.7 kJ d. 642.7 kJ 2. Use the following information on Na to determine the total amount of heat required to convert 150.0 g of solid Na at 48.0°C into gaseous Na at 883°C.Melting Point = 98.0°CBoiling Point = 883°C Molar Heat Capacities:C = 23.7 J/mol °CC =37.5 J/mol °CΔH = 2.64 kJ/molΔH = 97.9 kJ/mol Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a. 855 kJ b. 192 kJ c. 149 kJ d. 225 kJ
How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The following physical data may be useful.ΔHfus = 7.27 kJ/molCliq = 2.16 J/g°CCgas = 1.29 J/g°CCsol = 1.65 J/g°CTmelting = -95.0°C
7. Consider the following reaction: CH4 (g) +4 Cl₂ (g) → CCl4 (g) + 4 HCt (g) When 1.65 L C₂ (g) at STP reacts with sufficient CH. (g) via the given equation, 7.30 kJ of heat is released. The standard enthalpy of formation for CH4 (g) is - 74.8 kJ/mol and that of HCt (g) is-92.3 kJ/mol. Calculate the standard enthalpy of formation for CCl4 (g)? ANSWER: - 102 kJ/mol 7. Consider the following reaction: CH4 (g) +4 Cl₂ (g) → CCl4 (g) + 4 HCt (g) When 1.65 L Cl₂ (g) at STP reacts with sufficient CH4 (g) via the given equation, 7.30 kJ of heat is released. The standard enthalpy of formation for CH4 (g) is - 74.8 kJ/mol and that of HCl (g) is-92.3 kJ/mol. Calculate the standard enthalpy of formation for CCl4 (g)? ANSWER: -102 kJ/mol
In their Memoir on Heat, published in 1783, Lavoisier andLaplace reported, “The heat necessary to melt ice is equalto three quarters of the heat that can raise the same massof water from the temperature of the melting ice to that ofboiling water” (English translation). Use this 18th-centuryobservation to compute the amount of heat (in joules)needed to melt 1.00 g ice. Assume that heating 1.00 gwater requires 4.18 J of heat for each 1.00°C throughoutthe range from 0°C to 100°C.
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Calculate the quantity of energy required to convert 72.8 g of H₂O(s) at 0.0 °C to H₂O(g) at 100.0 °C. The enthalpy of fusion of ice at 0 °C is 333 J/g; the enthalpy of vaporization of liquid water at 100 °C is 2256 J/g; the specific heat capacity of liquid water is 4.184 J/g. K. Energy = J
A 46.81 g46.81 g sample of a substance is initially at 25.7 °C.25.7 °C. After absorbing 1415 J1415 J of heat, the temperature of the substance is 177.9 °C.177.9 °C. What is the specific heat (?) of the substance?
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3. Would the following processes be exothermic or endothermic? a. solid liquid b. gas → liquid c. liquid → solid d. NaOH 7 Nạo Hoai -AH e. liquid → gas
What is the total enthalpy change during the process in which 100.0 g of water at 50.0 °C is cooled to ice at -30.0 °C ? (Assume P = 1.0 atm). Note: COOLING is an EXOTHERMIC PROCESS!!! AH WILL BE NEGATIVE! Solution S.H. water = 4.18 J/g °C Temperature AHfus = 6.01 kJ/mol 50.0 °C 0.0 °C 1 -30.0 °C 2 3 S.H. ice = 2.03 J/g °C 100.0 g H₂O = 5.552 mol H₂O 18.01 g/mol ΔΗ, = SH x Υ x ΔΤ AH₁ = (4.18 J/g °C)(100.0 g)(0.0 - 50.0 °C) == - 20900 J - 20.9 kJ Energy (J) Thus the total enthalpy change is: AH₂ = -AHfus XY AH₂ = -(6.01 kJ/mol)(5.552 mol) = -33.4 kJ ΔΗ, = SH x Υ x ΔΤ AH3 = (2.03 J/g °C)(100.0 g)(- 30.0 - 0.00 °C) = 6090 J = - 6.09 kJ -20.9 kJ-33.4 kJ - 6.09 kJ = - 60.4 kJ
A 25.4-g sample of water at 290. K is mixed with 47.3 g water at 350. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.

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