General, Organic, and Biological Chemistry - 4th edition
4th Edition
ISBN: 9781259883989
Author: by Janice Smith
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 7.12, Problem 7.20PP
How much energy (in calories) is released when 50.0 g of water is cooled from
More Practice: Try Problems 7.93, 7.94.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Calculate the total energy, in kilojoules, that is needed to turn a 20 g block of ice at 0 degrees C into water vapor at 125 degrees C.
Must have 4 step process
5 points
Save Answ
Question 7
What mass of water would need to evaporate from your skin in order to remove 1.7 x 1o5) of heat from your body? The molar mass of H20 is 18.0 g/mol, its heat of fusion is 5.994 k/mol, and its
heat of vaporization is 40.7 kl/mol. The boiling point of water is 100°C.
O a. 58 g
O b. 420 g
OC 6.9 x 106 g
O d.7.5 x 104 g
O e. 75 g
What quantity of energy does it take to convert 0.100 kg ice at -20.°C to steam at 250.°C? Specific heat capacities: ice, 2.03 J/g °C;
liquid, 4.2 J/g.°C; steam, 2.0 J/g °C; AHvap = 40.7 kJ/mol; AHfus = 6.02 kJ/mol.
Energy =
kj
Submit Answer
Try Another Version
9 item attempts remaining
Chapter 7 Solutions
General, Organic, and Biological Chemistry - 4th edition
Ch. 7.1 - Prob. 7.1PCh. 7.2 - Convert each pressure unit to the indicated unit....Ch. 7.3 - Prob. 7.2PPCh. 7.3 - Prob. 7.2PCh. 7.3 - Prob. 7.3PPCh. 7.3 - Prob. 7.3PCh. 7.3 - Prob. 7.4PPCh. 7.3 - Prob. 7.4PCh. 7.3 - The pressure inside a 1.0-L balloon at 25C was 750...Ch. 7.4 - A sample of nitrogen gas contains 5.0 mol in a...
Ch. 7.4 - Prob. 7.7PPCh. 7.4 - Prob. 7.5PCh. 7.5 - Prob. 7.8PPCh. 7.5 - Prob. 7.6PCh. 7.6 - CO2 was added to a cylinder containing 2.5 atm of...Ch. 7.6 - Prob. 7.10PPCh. 7.6 - Prob. 7.7PCh. 7.7 - Prob. 7.8PCh. 7.7 - Prob. 7.9PCh. 7.7 - Prob. 7.11PPCh. 7.7 - Which species in each pair has stronger...Ch. 7.7 - Prob. 7.12PPCh. 7.7 - Prob. 7.11PCh. 7.8 - Prob. 7.13PPCh. 7.8 - Would you predict the surface tension of gasoline,...Ch. 7.9 - Prob. 7.13PCh. 7.10 - Prob. 7.14PPCh. 7.10 - The human body is composed of about 70% water. How...Ch. 7.10 - How much energy is required to heat 28.0 g of iron...Ch. 7.10 - Prob. 7.15PCh. 7.10 - Prob. 7.16PPCh. 7.10 - If the initial temperature of 120. g of ethanol is...Ch. 7.11 - Use the heat of fusion of water from Sample...Ch. 7.11 - Answer the following questions about water, which...Ch. 7.11 - Prob. 7.19PPCh. 7.12 - Answer the following questions about the graph...Ch. 7.12 - How much energy (in calories) is released when...Ch. 7.12 - How much energy (in calories) is required to melt...Ch. 7 - Prob. 19PCh. 7 - Prob. 20PCh. 7 - Prob. 21PCh. 7 - The compressed air tank of a scuba diver reads...Ch. 7 - Assume that each of the following samples is at...Ch. 7 - Use the diagrams in problem 7.23 to answer the...Ch. 7 - Prob. 25PCh. 7 - Prob. 26PCh. 7 - Prob. 27PCh. 7 - Prob. 28PCh. 7 - Prob. 29PCh. 7 - Prob. 30PCh. 7 - Prob. 31PCh. 7 - Prob. 32PCh. 7 - Prob. 33PCh. 7 - If you pack a bag of potato chips for a snack on a...Ch. 7 - Prob. 35PCh. 7 - Prob. 36PCh. 7 - Prob. 37PCh. 7 - Prob. 38PCh. 7 - Prob. 39PCh. 7 - Prob. 40PCh. 7 - Prob. 41PCh. 7 - Prob. 42PCh. 7 - Prob. 43PCh. 7 - Prob. 44PCh. 7 - Prob. 45PCh. 7 - Prob. 46PCh. 7 - Prob. 47PCh. 7 - Consider balloons A and B, which contain CH4 and...Ch. 7 - Prob. 49PCh. 7 - Prob. 50PCh. 7 - Prob. 51PCh. 7 - Prob. 52PCh. 7 - Prob. 53PCh. 7 - Prob. 54PCh. 7 - Prob. 55PCh. 7 - Prob. 56PCh. 7 - Prob. 57PCh. 7 - Prob. 58PCh. 7 - Prob. 59PCh. 7 - Prob. 60PCh. 7 - Prob. 61PCh. 7 - Prob. 62PCh. 7 - Prob. 63PCh. 7 - Prob. 64PCh. 7 - Which molecules are capable of intermolecular...Ch. 7 - Prob. 66PCh. 7 - Prob. 67PCh. 7 - Explain why the boiling point of A is higher than...Ch. 7 - Prob. 69PCh. 7 - Prob. 70PCh. 7 - Prob. 71PCh. 7 - Prob. 72PCh. 7 - Prob. 73PCh. 7 - Prob. 74PCh. 7 - Prob. 75PCh. 7 - Prob. 76PCh. 7 - Prob. 77PCh. 7 - Prob. 78PCh. 7 - Prob. 79PCh. 7 - Prob. 80PCh. 7 - Prob. 81PCh. 7 - How many calories of heat are needed to increase...Ch. 7 - Prob. 83PCh. 7 - If it takes 37.0 cal of heat to raise the...Ch. 7 - Prob. 85PCh. 7 - What phase change is shown in the accompanying...Ch. 7 - Prob. 87PCh. 7 - Which process requires more energy, melting 250 g...Ch. 7 - Consider the cooling curve drawn below a. Which...Ch. 7 - Prob. 90PCh. 7 - Draw the heating curve that is observed when...Ch. 7 - Prob. 92PCh. 7 - Use the following values to answer each part. The...Ch. 7 - Prob. 94PCh. 7 - Prob. 95PCh. 7 - Prob. 96PCh. 7 - Prob. 97PCh. 7 - Explain why you feel cool when you get out of a...Ch. 7 - Prob. 99CPCh. 7 - As we learned in Chapter 5, an automobile airbag...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Macmillan Learning How much heat energy is required to convert 88.5 g of solid ethanol at -114.5 °C to gaseous ethanol at 167.1 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g °C, and that of gaseous ethanol is 1.43 J/g °C. q= kJarrow_forwardPractice-How Much Heat Energy, in kJ, is Required to Vaporize 87 g of Acetone, C,H,0, (MM 58.08) at 25 °C? (AHvap = 31.0 kJ/mol)arrow_forwardAt -150°C a substance has a vapor pressure of 154 mmHg. What is the heat of vaporization in J/mol if it has a vapor pressure of 270 mmHg at 20°C? Answer to nearest whole number. Your Answer: Answerarrow_forward
- How much energy (in kļ) is needed to heat 5.03 g of ice from -20.3°C to 30.0°C? The heat of fusion of water is 6.01 kJ/(mol), and the heat capacity is 2.093 J/(g °C) for ice and 4.184 J/(g °C) for liquid water. Your answer should have 3 sig figs. Answer:arrow_forwardck 14 Question 12 of 23 View Policies Current Attempt in Progress A substance has a melting point of -25.0°C, an enthalpy of fusion of 1200 Jg¹; specific heats for the solid and the liquid are 3.00 and 6.20 Jg¹ C1, respectively. How much energy is needed to change 150 grams of the substance from a solid at -40.0°C to a liquid at +70.0°C? 7 Type here to search 2 Q A Z eTextbook and Media Save for Later @ 2 W S # x alt 3 4+ * 8 J 1 M a ( 9 K ▶11 ) O Attempts: 0 of 2 used Submit Answer O L P 12 alt { ^ @ + r -/1 E : = ? 1 DA 4x O insert ] ctrl pause 10:26 PM 8/30/2022 prt sc backspace 2arrow_forwardThe molar heat of vaporization of water at 25 °C is +43.9 kJ/mol. How many kilojoules of heat would be required to vaporize 6.75 g of water? i kJ eTextbook and Media Save for Later Attempts: 0 of 15 used Submit Answer MacBook Air DD 888 F6 F7 F8 FO F10 F4 F5 F2 F3 @ 23 &arrow_forward
- Calculate the heat absorbed when 28.9 g of some substance at 9.12 is completely melted. The molar heat of fusion for the substance is 6.47kJ • mol -1 and the molar mass is 19.51g • mol-1. Express answer I'm correct sig figsarrow_forwardQuestion 17 How much energy is needed to convert 54.9 grams of ice at 0.00°C to water at 75.0°C specific heat (ice) = 2.10 J/g°C specific heat (water) = 4.18 J/g°C heat of fusion = 333 J/g heat of vaporization = 2258 J/g OA. 26.9 kJ %3D B.35.5 kJ OC. 1.97 kJ OD. 141 kJ OE. 17.2 kJ A Moving to another question will save this response. DELLarrow_forwardA pressure cooker (InstaPot) works by increasing the temperature that water in food or cooking food boils at. If water is placed in a pressure cooker and the internal pressure rises to 3.50 atm, what will the boiling point of the water in the cooker be in oC ? The ΔHvap for water is 40.79 kJ/mol. Answer has 3 sig figs.arrow_forward
- C www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IibwdleAUz2IYCcR4NM7yr_IpMriNwxObE8iQddlu PMCg7x0md1wd4vxL1gn0GB0yoJJ7UtwiSOinuVIMFF... YouTube 1 82°F OSTATES OF MATTER Identifying phase transitions on a heating curve Translate A pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. Here is a graph of the results: 190. Explanation 170. temperature (°C) 130. Mostly cloudy 150. 110. 90. 70. Use this graph to answer the following questions: 0. What is the melting point of X ? 10. Check 20. heat added (kJ/mol) 30. 40. 50. 0°C (check all that annly) Q Search! 60. LOU e 3/5 4 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Aarrow_forwardQuestion 3 Calculate the amount of heat absorbed by 10.0 grams of ice at -15.0°C as it is Evaporating th %3D converted to liquid water at 50.0°C. The specific heat of H20(s) = 2.09 J/(g°C). The physics 1. a) using specific heat of H20(1) = 4.18 J/(g°C). The heat of fusion is 333 J/g. conservatic determine of fusion percenta determir 0.676KJ -0.1kg -56 C Che How O 0.170kJ con 155 he 5.73kJ O 2.83kJ Next Previousarrow_forwardEquations The heat energy associated with a change in temperature that does not involve a change in phase is given by q=msAT where q is heat in joules, m is mass in grams, s is specific heat in joules per gram-degree Celsius, J/(g · °C), and AT is the temperature change in degrees Celsius. The heat energy associated with a change in phase at constant temperature is given by q=mΔΗ where q is heat in joules, m is mass in grams, and AH is the enthalpy in joules per gram. Physical constants The constants for H₂O are shown here: ● ● Specific heat of ice: Sice = 2.09 J/(g. °C) Specific heat of liquid water: swater = 4.18 J/(g · °C) Enthalpy of fusion (H₂O(s)→H₂O(1)): AHfus = 334 J/g Enthalpy of vaporization (H₂O(1)→H₂O(g)): AHvap = 2250 J/garrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
Recommended textbooks for you
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY