The vapor pressure of ethanol is 115 torr at 34.9°C. If ΔHvap of ethanol is 38.6 kJ/mol, calculate the temperature (in °C) when the vapor pressure is 760 torr.
When I plug everything in I get 1.888 = -4640 *(1/t2-3.247*10^-3) but my algebra is rusty and I don't get the same answer as the book. A detailed explanation would be greatly appreciated. Thanks!
lnP2/P1= -Hvap/R*(1/t2-1/t)
The vapor pressure of ethanol is 115 torr at 34.9°C. If ΔHvap of ethanol is 38.6...
The vapor pressure of ethanol is 115 torr at 34.9 oC and ΔHvap of ethanol is 38.6 kJ/mol, use this information and the Clausius-Clapeyron equation (shown below) to calculate the temperature in oC at which the vapor pressure is 760 torr (remember to convert temperatures to K in the equation (K = oC + 273). R = 8.314 J/mol·K. ( Please show each step, step BY step) I am having difficult with finding T2
The vapor pressure of a substance is 760.0 torr at 115°C and 14.6 torr at 45°C. What is ΔHvap of the substance?
a.) The vapor pressure of ethanol is 1.00 × 102 mmHg at 34.90°C. What is its vapor pressure at 55.7°C? (ΔHvap for ethanol is 39.3 kJ/mol.) answer in mmHg b.) Calculate the amount of energy (in kJ) necessary to convert 357 g of liquid water from 0°C to water vapor at 182°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g · °C, and for steam is 1.99 J/g ·°C....