How much heat is required to convert 47.0 gof ethanol at -142 °C to the vapor phase at 78 °C?

Here's a formula you can follow The heat of combustion of 1 gram of ethanol equals -29,782 J, or…

Answered: How much heat is required to convert…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter11: Liquids And Solids

Section: Chapter Questions

Problem 11.98QE

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Similar questions

The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.
9.46 The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy would be needed to melt a 5.24-g sample of silicon at its melting point of 1693 K?
Why are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.
Is it possible to liquefy nitrogen at room temperature (about 25 C)? Is it possible to liquefy sulfur dioxide at room temperature? Explain your answers.
Calculate the grams of oxygen gas required to produce 7.60 kJ of heat when hydrogen gas burns at constant pressure to give liquid water, given the following: 2H2(g)+O2(g)2H2O(g);H=484kJ Liquid water has a heat of vaporization of 44.0 kJ per mole at 25C.
The vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.
Use Figure 11.7 to estimate the boiling point of carbon tetrachloride, CCl4, under an external pressure of 250 mmHg.
Follow the step-wise process outlined in Problem 31 to calculate the amount of heat involved in condensing 100.00 g of benzene gas (C6H6) at 80.00C to liquid benzene at 25.00C. Use Tables 8.1 and 8.2 for the specific heat, boiling point, and heat of vaporization of benzene.
Consider the data for substance X given in Exercise 117. When the temperature of 1.000 mole of X(g) is lowered from 100.0C to form X(l) at 50.0C. 28.75 kJ of heat is released. Calculate the specific heat capacity of X(g).
Explain why the enthalpies of vaporization of the following substances increase in the order CH4NH3H2O, even though all three substances have approximately the same molar mass.
The cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of vaporization of ethanol (ethyl alcohol), C2H5OH. C2H5OH(l)C2H5OH(g);H=? The standard enthalpy of formation of C2H5OH(l) is 277.7 kJ/mol and that of C2H5OH(g) is 235.1 kJ/mol.
Liquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.

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How much heat is required to convert 47.0 g of ethanol at -142 °C to the vapor phase at 78 °C?