You must show all of your work to receive full credit. Answers that do not have complete work and units will be marked incorrect. Part A Fill out the table below to determine the molar masses (in g mol-¹) and types of intermolecular forces for each compound. Compound Ethanol Formula 1-Propanol C3H₂OH C₂H5OH 1-Butanol C4H,OH Methanol CH3OH n-Hexane n-Pentane C5H12 ©2022 F'22/S'23 C6H14 Structure Molar mass How do intermolecular forces affect the evaporation rate of a solvent? Be very descriptive on how the intermolecular forces are affected by the intermolecular forces. H-bond? IMFS Present Chemistry I Lab Manual 223

You must show all of your work to receive full credit. Answers that do not have complete work and units will be marked incorrect. Part A Fill out the table below to determine the molar masses (in g mol-¹) and types of intermolecular forces for each compound. Compound Ethanol Formula 1-Propanol C3H₂OH C₂H5OH 1-Butanol C4H,OH Methanol CH3OH n-Hexane n-Pentane C5H12 ©2022 F'22/S'23 C6H14 Structure Molar mass How do intermolecular forces affect the evaporation rate of a solvent? Be very descriptive on how the intermolecular forces are affected by the intermolecular forces. H-bond? IMFS Present Chemistry I Lab Manual 223

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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Compare the boiling points of the various isomeric hydrocarbons shown in the table below. Notice the relationship between boiling point and structure; branched-chain hydrocarbons have lower boiling points than the unbranched isomer. Speculate on possible reasons for this trend. Why might the intermolecular forces be slightly different in these compounds? Compound Boiling Point (°C) 68.9 Hexane 3-Methylpentane 2-Methylpentane 2,3- Dimethylbutane 2,2- Dimethylbutane 63.2 60.3 58.0 49.7 The more branched structure has smaller exposed surface and hence weaker dispersion intermolecular forces. The more branched structure has larger exposed surface and hence weaker dispersion intermolecular forces. The more branched structure has larger exposed surface and hence stronger dispersion intermolecular forces. The more branched structure has smaller exposed surface and hence stronger dispersion intermolecular forces.
Based on the thermodynamic properties provided for water, determine the amount of energy needed for 2.00 kg of water to go from -16.0 °C to 69.0 °C. Property Melting point Boiling point AHfus AHvap Cp (s) Cp (1) Cp (8) kJ Value 0.0 100.0 6.01 40.67 37.1 75.3 33.6 Units °℃ °C kJ/mol kJ/mol J/mol. °C J/mol • °C J/mol. °C
Organic chemistry
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
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1) Justify your prediction for the T of 1-butanol. 2) discuss how well your experimental results matched your prediction for the T of 1-butanol. 3) Which of the alcohols measured has the strongest intermolecular forces? 4) Which of the alcohols measured has the weakest intermolecular forces? 5) Using your knowledge of intermolecular forces explain your response to questions #3 and #4 6) Look up the theoretical boiling point for each compound. Arrange the compounds by increasing boiling point. 7) Prepare a bar graph of your experimental results. Plot the number of carbons in the alcohol on the x-axis and the T on the y-axis.
A pure sample of Substance S is put into an evacuated flask. The flask is then heated steadily and the temperature measured as time passes. The results are graphed below, in the middle (in green). Identical experiments are now run on Substance Y and Substance Z. Substance Y is just like S except that it has a higher heat capacity in the solid phase C₂ (s). Substance Z is just like S except that it has a lower enthalpy of vaporization H. Select the graphs below, on the left and right, that show the results you expect for these new experiments. Substance Y •C₁ (s)) (higher Cp (Drag the slider to choose an image) temperature (°C) Substance S added heat (kJ/mol) Substance Z (lower H₂) (Drag the slider to choose an image) ³ 5
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