Rowan ChemSu22. A gas sample of a compound weighing 34.3 g (MW: 70.2 g/mol) at 127.2C is converted to the liquid phase at 44.6 C. What amount of heat (in J) is required to performthis process?Tb = 114 CHvap 2.44 kJ/molspecific heat of the gas is 4.3 g/J*molspecific heat of the liquid is 1.4 g/J*mol

Given information:- Mass of the gas sample = 34.3 g- Molar mass (MW) of the compound = 70.2 g/mol-…

Answered: Rowan ChemSu22. A gas sample of a…

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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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
4
Use the data below to calculate the total heat in kJ needed for the following processés. melting point at 1 atm specific heat of liquid sodium 1.38 J/g°C 97.80°C specific heat of solid sodium 1.23 J/g°C AHfus 2.60 kJ/mol Provide the numerical answer without units to the correct significant figures and in a 'non-exponential form, i.e., in a form where the exponent is zero and therefore not shown. For example, 0.444 rather than 4.44 x 101. 1. The energy in kJ needed to heat 20.00 g of solid sodium (22.99 g/mol) at -5.00°C to solid sodium at 97.80°C when the atmospheric pressure is 1 atm. 2. The energy in kJ needed to heat 20.00g of solid sodium (22.99 g/mol) at 97.80°C to liquid sodium at 97.80°C when the atmospheric pressure is 1 atm.
A 124.0 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 \deg C to 147.6 \deg C. ( heat capacity of liquid = 1.62 J/g. \deg C; heat capacity of gas = 1.04 J/g. \deg C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 \deg C) How much energy (in kJ) is absorbed/released to condense the gas?
5. When 10 g of diethyl ether is converted to vapor at its boiling point, how much heat is absorbed? (C4H100, AHvar = 15.7 kJ/mol, boiling point: 34.6°C) а. 20 КJ b. 0.2 KJ с. 2 КJ d. 200 KJ
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.
Calculate the heat change in joules for vaporization of 9.00 g of water at 100 ∘C.
The graph shown below is the hypothetical heating curve showing the temperature of 1 mol of a substance versus the amount of heat energy added to said substance. 120 110 100 90 E 80 9 70 60 C 50 В 40 30 A 20 10 0 10 20 30 40 50 60 70 80 90 100 Heat Input (kJ) a) Which line segment(s) correspond to the gas phase of the substance? O A В O C D E b) Which line segment(s) correspond to phase changes? A В O C D E Temp ("C)
Calculate the amount of heat (in kJ) required to raise the temperature of a 86.0 g sample of ethanol from 198.0 K to 300.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. 60.0 kJ 21.2 kJ 11.9 kJ 75.6 kJ 28.4 kJ
Determine the amount of heat (in kJ) required to convert 8.24 moles of liquid methanol at-22°C into gaseous methanol at 98°C. Use the following information on methanol to calculate the amount of heat for each of the steps. Melting Point =-98°C Boiling Point = 65°C Molar Heat Capacities: Ciquid = 81.1 J/mol °C Cgas = 43.9 J/mol °C AHucion 3.22 kJ/mol AHvaporization 37.3 kJ/mol Type your numeric answer and submit

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