Why is it that the heat of condensation isn't negative along with the amount of heat released in the cooling of water? I thought Delta H con =(-Delta H vap?) Im not sure what I'm missing please help explain and break it down for me pictures help as well thank you so0o much! :) Part A Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following. Keep in mind that the sign of the heat involved in Calculate the joules released when 155 g of steam condenses at 100 °C and the liquid cools to 10.0 °C. the state change is ignored. Express your answer to three significant figures and include the appropriate units. Link to sample problems on phase change calculations. ? Value Units Submit Request Answer Rate an steam Condensation 1559 15 59 water waten Caling 100°C 1559 10.0°C 100°C AT Amount of Heat released in condensation (4)= (AH Mass ot steam %3D vep = (2259.36JA( 155 9) %3D 350200.8 T 3.50 X10° J Amount of Heat released in cooling of wader (Ha) = m.Sehe AT H2 = 5.83 X10 J H2 = 0.583 X10 J

Why is it that the heat of condensation isn't negative along with the amount of heat released in the cooling of water? I thought Delta H con =(-Delta H vap?) Im not sure what I'm missing please help explain and break it down for me pictures help as well thank you so0o much! :) Part A Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following. Keep in mind that the sign of the heat involved in Calculate the joules released when 155 g of steam condenses at 100 °C and the liquid cools to 10.0 °C. the state change is ignored. Express your answer to three significant figures and include the appropriate units. Link to sample problems on phase change calculations. ? Value Units Submit Request Answer Rate an steam Condensation 1559 15 59 water waten Caling 100°C 1559 10.0°C 100°C AT Amount of Heat released in condensation (4)= (AH Mass ot steam %3D vep = (2259.36JA( 155 9) %3D 350200.8 T 3.50 X10° J Amount of Heat released in cooling of wader (Ha) = m.Sehe AT H2 = 5.83 X10 J H2 = 0.583 X10 J

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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Given that the heat of fusion of water is -6.02 kJ>mol, the heatcapacity of H2O(l) is 75.2 J>mol # K, and the heat capacity of H2O(s)is 37.7 J>mol # K, calculate the heat of fusion of water at -10°C.
How much heat (in kJ) must be added to change 11.6 g of H2O(s) at -8°C to steam at 110°C? The specific heat of H2O(s) is 2.09 J/g°C, of H2O(l) is 4.184 J/g°C, and of H2O(g) is 1.84 J/g°C. The heat of fusion of water is 334. 7 J/g and the heat of vaporization is 2259.4 J/g.
What amount of heat, in kJ, is required to convert 1.60 g of water at 67.0 °C to 1.60 g of steam at 100.0 °C? (specific heat capacity of water = 4.184 J/g °C; AHvap = 40.7 kJ/mol) %3D
A normal size ice cube has a mass of 50.0 g. How much energy will it take to melt the ice and then warm the water to 10.0 oC? Potentialy useful information: heat of fusion = 6.01 kJ/mol, specific heat = 4.184 J/g oC, heat of vaporization = 40.65 kJ/mol.
How much heat is released when 105 g of steam at 100.0 C is cooled to ice at -15.0 C? The enthalpyof vaporization of water is 40.67 kj/mol, the enthalpy of fusion for water is 6.01 kj/mol, the specific heatcapacity of liquid water is 4.18 J/g C and the specific heat capacity of ice is 2.02 J/g C.(q heating = m x C x ΔT, q phase change = ΔH vap x n)
A total of 537 cal of heat is added to 5.00 g of ice at -20.0 °C. What is the final temperature of the water? Tfinal = °C Specific heat of H₂O(s) Specific heat of H₂O(l) Heat of fusion for H₂O 2 2.087 J/(g. °C) 4.184 J/(g. °C) 333.6 J/g
The vapor pressure of ethanol is 1.00 x 10“ mmHg at 34.90°C. What is its vapor pressure at 59.75°C? ( AHan for ethanol is 39.3 kJ/mol.) vap mmHg
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How much energy is needed to turn 10.0 g of water at 25°C to steam ( = 6.01 kJ/mol; = 40.76 kJ/mol; c = 75.3 J/mol • °C)?
2. Calculate the amount of energy (in kilojoules) needed to heat 346 g of liquid water from 0°C to 182°C. Assume that the specific heat of water is 4.184 J/gᵒC over the entire liquid range and that the specific heat of steam is 1.99 J/gᵒC. (AHvap = 40.79 kJ/mol for water)
Direction: Use the heating curve of ethanol to answer the questions below. HEATING CURVE OF ETHANOL E mOILING F 78+ LIQUID B MELTINGC. -115+ SOLID TIME T'E'N'A Questions: 1. What point where ethanol begins to melt? 2. What is ethanol`s melting point? 3. What point where ethanol is all done melting? 4. Between what point where solid and liquid ethanol co-exist? 5. At what point is ethanol is all in its gas phase? 6. Between what point where liquid and gas ethanol co-exist? TEMPERATURE ("C)
4. Fill up the missing words in this statement. The boiling point of a non-polar substance is _______ because the intermolecular force is ________.Choices: high: strong, high: weak, low: strong, low: weak