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Which of the following are TRUE statements regarding evaporation, boiling, and vapor pressure? Select as many...
Question 1 & 2. which of the following statements is true? the vapor pressure of a liquid _____ as the strength of its intermolecular forces increases. Question 1 Select one answer Which of the following statements is true? 10 points A. When heat is added to ice at 0 °C the ice begins to melt, but the temperature remains constant until all of the ice becomes liquid water. B. When heat is added to ice at 0°C the ice begins...
1.) If a molecule has a high vapor pressure… A) Then the molecule experiences strong intermolecular forces. B) Then the molecule experiences weak intermolecular forces. C) The molecule definitely experiences hydrogen bonding. D) There is not enough information to determine the strength of the intermolecular forces. 2.) A solution of ethanol in water has a boiling point of 100.55oC. What is the molality of the ethanol in the water? Boiling point for pure water = 100oC Kb = 0.51 oC...
Use the following vapor pressure data to answer the questions: VaporTemperature, Pressure, torr Liquid 400 63.5 CH3COoCH3 400 40.0 (1) In which liquid are the intermolecular attractive forces the strongest? (2) The vapor pressure of C2H;OH at 40.0 °C would be than 400 torr. Use the following vapor pressure data to answer the questions: VaporTemperature, Pressure, torr Liquid 400 63.5 CH3COoCH3 400 40.0 (1) In which liquid are the intermolecular attractive forces the strongest? (2) The vapor pressure of C2H;OH...
Question 3 (4 points) The vapor pressure of a liquid is dependent on: the temperature of the liquid and intermolecular forces of attraction in the liquid the temperature of the liquid and the surface area of the liquid only on the surface area of the liquid only the temperature of the liquid O only the forces of intermolecular attraction in the liquid Question 4 (4 points) If the atmospheric pressure over a sample of liquid is increased, the boiling point...
1.) If a molecule has a high vapor pressure… A) Then the molecule experiences strong intermolecular forces. B) Then the molecule experiences weak intermolecular forces. C) The molecule definitely experiences hydrogen bonding. D) There is not enough information to determine the strength of the intermolecular forces. 2.) A solution of ethanol in water has a boiling point of 100.55oC. What is the molality of the ethanol in the water? Boiling point for pure water = 100oC Kb = 0.51 oC...
11. Order the following from highest vapor pressure to lowest by ordering the expected strength of the intermolecular forces. Molecule Dominant form of intermolecular force Ranking of vapor pressure (1 = highest, 5 = lowest) CHA CH3OH H20 HO-CH2-CH2-OH H3C-O-CH3
Which of the following changes would increase the vapor pressure of a liquid? i. An increase in temperature ii. An increase in the intermolecular forces in the liquid iii. An increase in the size of the open vessel containing the liquid a) i and ii only b) i and iii only c) i only d) ii only e) iii only If the rate of evaporation from the surface of a liquid exceeds...
a) What is the effect of vapor pressure on a liquid’s boiling point? In your answer explain what two pressures must be equal in order for a substance to boil. How could you make a substance boil at a higher temperature? b) What is the difference between intermolecular and intramolecular forces (define each)? also give an example of each. c) Draw a diagram of NH2F molecules as they boil, and use Lewis Structures to label the most important intermolecular force and...
Consider the molecule below: o=s=o: Select ALL the intermolecular forces that are expected to be present between two of these molecules. Select as many answers as are applicable, however points will be deducted for incorrect guesses. Select one or more: Dispersion forces Dipole/dipole forces Hydrogen bonding Check What amount of thermal energy (in kJ) is required to convert 136 g of ice at -16 °C completely to water vapour at 217 °C? The melting point of water is 0°C and...
figure 1 Figure 2 Liquid ethanol mm P increasing P = equilibrium vapor pressure P=0 Add System comes to equilibrium ethanol Evacuated flask, pressure zero Molecules begin to vaporize, pressure increases Molecules leave and enter liquid at equal rates, pressure reaches steady-state value 34.6 °C 78.3°C 100 °C Normal boiling point Diethyl ether Vapor pressure (torr) Ethyl alcohol (ethanol) Water Ethylene glycol 100 20 40 60 80 Temperature (°C) Copyright 2009 Pearson Prentice Hall,Inc. Click on: (Figure 2) and study...