Calčulate the energy change during a pha change.Given the following information for water, H,0 (at 1 atm), calculate the amount of heat in kJ needed (at 1atm) to vaporize a 46.9-g sample of liquid water at its normal boiling point of 100 °C.AHvap(100 °C) = 40.7 kJ/molAHfus (0.00 °C) = 6.01 kJ/molboiling point = 100 °C%3Dmelting point = 0.00 °Cspecific heat liquid = 4.18 J/g°CkJCheck & Submit AnswerShow ApproachWe now have the tools needed to calculate both the amount of thermal energy required to warm an objectin a particular physical state and the amount of thermal energy required to change the physical state of asubstance. Interactive Figure 5.3.6 shows the energy involved in heating 100-g samples of benzene andwater over a large temperature range.26tvA huluW

Given data, Vaporisation enthalpy =∆Hvap = 40.7 kJ/mol Fusion enthalpy =∆Hfus = 6.01 kJ/mol Mass of…

Given the following information for water, H20 (at 1 atm), calculate the amount of heat in kJ needed (at 1 atm) to vaporize a 46.9-g sample of liquid water at its normal boiling point of 100 °C. boiling point = 100 °C AHvap(100 °C) = 40.7 kJ/mol %3D melting point = 0.00 °C AHfus(0.00 °C) = 6.01 kJ/mol %3D specific heat liquid = 4.18 J/g°C kJ

Given the following information for water, H20 (at 1 atm), calculate the amount of heat in kJ needed (at 1 atm) to vaporize a 46.9-g sample of liquid water at its normal boiling point of 100 °C. boiling point = 100 °C AHvap(100 °C) = 40.7 kJ/mol %3D melting point = 0.00 °C AHfus(0.00 °C) = 6.01 kJ/mol %3D specific heat liquid = 4.18 J/g°C kJ

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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Please answer question 3.
What quantity of heat is required to convert 19.0 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (heat capacity of ethanol = 2.46 J/g • C; ∆Hvap = 39.3 kJ/mol)
Based on the thermodynamic properties provided for water, determine the amount of energy released for 130.0 g of water to go from 89.0 °C to -12.0 °C. Property Value Units Melting point 0.0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C
Converting a 5.00 g sample of liquid cyclohexane (C6H₁2) at 30.7 °C to vapor at 140.7 °C requires kJ of heat. molar mass = 84.16 g/mol melting point = 6.5 °C boiling point = 80.7 °C AHfus = 2.68 kJ/mol AHvap = 32.0 kJ/mol Csolid 1.2 J/g °C Cliquid 2.8 J/g °C Cgas = 0.90 J/g °C
Two 20.0 g ice cubes at -17.0 °C are placed into 235 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/ (mol·K) heat capacity of H,O(1) 75.3 J/ (mol·K) T = enthalpy of fusion of H,O 6.01 kJ/mol
Octane(C3H18) is a hydrocarbon found in crude oil. Thermochemical data for octane is provided below. The total change in enthalpy is 15.94 kJ when heating 0.2500 moles of octane from -70.00°C to 100.0°C. Determine the AHfusion. Melting point: -57.00 °C Boiling point: 126.0 °C J Csolid : 185.0 °C mol J Cliquid: 254.0 °C mol J Cgas: 250.0 °C mol AHvap: 34.40 kJ/ mol Molar mass: 114.23 g/mol 0.2693 kJ/mol 4.720 kJ/mol O 21.50 kJ/mol 0.2540 J/mol
Ee.72. The vapor pressure of water is 18.9 atm at 175 K, and the vapor pressure of water is 75.5 atm at 620.3 K. Calculate the enthalpy of vaporization in kJ/mol.
Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro
Some physical properties of water are shown below. melting point boiling point specific heat solid 2.05 J/g °C specfic heat liquid 4.184 J/g.°C specific heat gas 2.02 J/g °C ΔΗ° fusion 6.02 kJ/mol ΔΗ° vaporization 40.7 kJ/mol If 16.6 g of water at 80°C are mixed with 10.7 g of ice at 0.0°C, what is the final temperature of the mixture? °℃ 0.0°C 100.0°C
Ethanol (C2 H5 OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid ethanol at -50 °C? 3949 207.3 6.67 8.97 -12.5
Calculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to 99°C. The specific heat of liquid water is 1.00 cal/g °C
Consider the following data for ethanol, C2H5OH: Melting Point = -114°C Boiling Point = 78°C ΔHfusion = 5.0 kJ/mol ΔHvaporization = 42.6 kJ/mol Specific Heat of Liquid Ethanol = 2.5 J/g•°C Sketch a cooling curve that depicts ethanol vapor at 78°C being cooled until solid ethanol is formed at -114°C and then calculate the total amount of heat in kilojoules released when 55 grams of ethanol undergoes this process.