The vapor pressure of ethanol at 34.7 °C is 100.0 mm Hg, and the heat of vaporization of ethanol is 41.8 kJ·mol-1. What is the vapor pressure of ethanol at 65.0 °C? What is the boiling point of ethanol at 1 atm (1 atm = 760 mm Hg)?
The vapor pressure of ethanol at 34.7 °C is 100.0 mm Hg, and the heat of...
4. Liquid ammonia has a vapor pressure of 109 mm Hg at-66°C and a heat of vaporization of 2.46 x 10 J/mol. a) Estimate the normal boiling point of ammonia. b) Estimate the ratio of the vapor pressure at -66°C to that at -45°C 4. Liquid ammonia has a vapor pressure of 109 mm Hg at-66°C and a heat of vaporization of 2.46 x 10 J/mol. a) Estimate the normal boiling point of ammonia. b) Estimate the ratio of the...
1) The vapor pressure of liquid antimony is 400 mm Hg at 1.84×103 K. Assuming that its molar heat of vaporization is constant at 115 kJ/mol, the vapor pressure of liquid Sb is _____ mm Hg at a temperature of 1.81×103 K. 2) The normal boiling point of liquid acetone is 329 K. Assuming that its molar heat of vaporization is constant at 29.0 kJ/mol, the boiling point of CH3COCH3 when the external pressure is 1.21 atm is ______ K.
Ethanol,CH3CH2OH , has a vapor pressure of 59 mm Hg at 25 °C. What quantity of energy as heat is required to evaporate 115 mL of the alcohol at 25 °C? The enthalpy of vaporization of the alcohol at 25 °C is 42.32 kJ/mol. The density of the liquid is 0.7849 g/mL.
A liquid has a vapor pressure of 100 mm Hg at 25 degrees celsius. If the heat of vaporization is 15 kj /mol, what is the normal boiling point?
The vapor pressure of ethanol is 54.68 mm Hg at 25°C. How many grams of estrogen (estradiol). C18H2402, a nonvolatile, nonelectrolyte (MW 272.4 g/mol), must be added to 272.5 grams of ethanol to reduce the vapor pressure to 53.15 mm Hg? ethanol CH3CH OH = 46.07 g/mol gestrogen Submit Answer Try Another Version 3 item attempts remaining Identify the point(s) on the following diagram where the addition of heat will cause the temperature of the sample to increase . H...
The vapor pressure of ethanol at 34.7 degrees Celsius is 100mmHg, and Hvap= 38.6 kJ/mol. What is the normal boiling point temperature of ethanol.
The vapor pressure of substance X is 100. mm Hg at 1080.°C. The vapor pressure of substance X increases to 600. mm Hg at 1220.°C. Determine the molar heat of vaporization of substance X using the derived form of the Clausius-Clapeyron equation given below. (Include the sign of the value in your answer.) ____ kJ/mol
DATA Temperature (°C) Temperature (K) /T (K) Vapor Pressure (mm Hg) In (Vapor Pressure) 299.0K 302.2 K 30% 30q.2K 0.003344 D.003210 o -1 -l -I 149.U |い·3· 1912 0T.2 1. Plot In(Vapor Pressure) vs. 1/T using a spreadsheet program like Excel. Include the correlation coefficient and the lincar regression equation for the best-fit straight line through the points.dsa Attach the graph to this report. I Iniar regresstoneqvation035 Calculate the heat of vaporization for ethanol based on the slope obtained from...
The vapor pressure of ethanol is 54.68 mm Hg at 25°C. How many grams of saccharin, C7H5NO3S, a nonvolatile, nonelectrolyte (MW = 183.2 g/mol), must be added to 247.0 grams of ethanol to reduce the vapor pressure to 54.03 mm Hg ? ethanol = CH3CH2OH = 46.07 g/mol.
The vapor pressure of ethanol is 54.68 mm Hg at 25°C. How many grams of chlorophyll, C55H72MgN4O5, a nonvolatile, nonelectrolyte (MW = 893.5 g/mol), must be added to 206.4 grams of ethanol to reduce the vapor pressure to 53.60 mm Hg ? ethanol = CH3CH2OH = 46.07 g/mol. .............g chlorophyll