How much energy is required to heat 45.0 g H2O from a liquid at 70.0°C to a gas at 115°C? Also, annotate/label the amount of heat you are calculating on a heating curve. The following physical data may be useful. AHvap = 40.7 kJ/mol Cliq = 4.18 J/g.C Cgas = 2.01 J/g.C Heating Curve Diagram: Temperature (°C) 100°C 0°C (A) (B) (C) (D) (E)

How much energy is required to heat 45.0 g H2O from a liquid at 70.0°C to a gas at 115°C? Also, annotate/label the amount of heat you are calculating on a heating curve. The following physical data may be useful. AHvap = 40.7 kJ/mol Cliq = 4.18 J/g.C Cgas = 2.01 J/g.C Heating Curve Diagram: Temperature (°C) 100°C 0°C (A) (B) (C) (D) (E)

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

Find the total energy involved in converting 450.0g of water from -21°C to 35°C. Hvan Water = 40.7 KJ/mol Hrus Water = 6.01 KJ/mol Solid C =2.03 J/g°C water Liquid Cwater =4.184 J/g°C Gas Cwater 2.01 J/g°C O 235 KJ O 150 KJ O 85 KJ 255 KJ
Diethyl ether, used as a solvent for extraction of organic compounds from aqueous solutions, has a high vapor pressure which makes it a potential fire hazard in laboratories in which it is used. How much energy is released when 315.0 g is cooled from 153.0°C to 0.0°C? boiling point: 34.5°C Heat of vaporization: 351 J/g Specific heat capacity, (CH3)2O(l): 3.74 J/(g·K) Specific heat capacity, (CH3)2O(g): 2.35 J/(g·K) 145 kJ 158 kJ 116 kJ 63.1 kJ 21.1 kJ
thermometer. insulated container A sample of quartz, which has a specific heat capacity of 0.730 J-goC, is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 90.0 °C and the temperature of the water starts off at 25.0 °C. When the temperature of the water stops changing it's 27.1 °C. The pressure remains constant at 1 atm. water Calculate the mass of the quartz sample. Be sure your answer is rounded to 2 significant digits. 0 x10 X ? a sample a calorimeter do F
Use the information provided below to calculate the quantity of heat (in kJ) required to convert 63.01 g of substance A from an initial temperature of 54.44°C to a final temperature of -6.64°C. The molar mass of the substance is 27.1 g/mol. Melting Point of A = 1.686°C Heat of fusion = 11.19 kJ/mol Boiling point of A 108.5°C Heat of vaporization = 71.95 kJ/mol %3D Solid Liquid Gas Specific heat (J/g°C) 2.89 4.14 6.42 Report your answer to the tenths place and do not include units. Do not include a sign with your answer.
thermometer. A sample of aluminum, which has a specific heat capacity of 0.897 J·g *.°C*, is put into a calorimeter (see sketch at right) that insulated container contains 100.0 g of water. The aluminum sample starts off at 91.4 °C and the temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. water Calculate the mass of the aluminum sample. Be sure your answer is rounded to 2 significant digits. sample a calorimeter x10
Specific Heats of Substances Substance Specific Heat g-°C Brick 0.20 Ethanol 0.58 0.10 pooM Calculate the amount of heat, in calories, that must be added to warm 70.9 g of brick from 19.3 °C to 41.0 °C. Assume no changes in state occur during this change in temperature. heat added: cal Calculate the amount of heat, in calories, that must be added to warm 70.9 g of ethanol from 19.3 °C to 41.0 °C. Assume no changes in state occur during this change in temperature. heat added: cal
Which substance will have the largest temperature change if the same amount of heat is added to each of them?Gold, Au(s): specific heat = 0.0308 calories per gram degree Celsius.Water, H2O(l): specific heat = 1.00 calorie per gram degree Celsius.Copper, Cu(s): specific heat = 0.0920 calorie per gram degree Celsius.Ethanol, C2H5OH(l): specific heat = 0.588 calorie per gram degree Celsius
Calculate the energy content (in calories) of a 1.00 g of product that is placed inside a calorimeter having a heat capacity of 950 J/K. Data from the calorimeter indicated that the 3.0 L surrounding water had initial and final temperatures of 18.0 °C and 47.5 °C, respectively. Specific heat capacity of water: 4.18 J/g-K a. 2.6x10^4 cal b. 9.5x10^4 cal c. 8.8x10^4 cal d. 7.3x10^4 cal
You have 500 g of dry ice at a temperature of 50 K. How much energy would it take to produce carbon dioxide gas heated to a temperature of 400оC? Specific heat of CO2(s) = 0.709 J/g K Specific heat of H2O(s) = 2.040 J/g K Specific heat of CO2(g) = 0.850 J/g K Specific heat of H2O(l) = 4.184 J/g K Specific heat of H2O(g) = 2.010 J/g K Freezing point (CO2) = -78.5оC Freezing point (H2O) = 273.15 K Latent heat of sublimation (CO2) = 199 J/g Latent heat of fusion (H2O) = 334 J/g Latent heat of vaporization (H2O) = 2260 J/g