How much energy (in kJ) does it take to turn 42.00 g of octane (C3H18) at 99.95°C into a gas at 164.87°C? Use the following reference table to help answer this question: Melting Point -46.53°C Boiling Point 124.05°C AHfus 27.548 kJ/mol AHvap 49.342 kJ/mol Cs, solid 33.03 J/g-K Cs, liquid 338.46 J/g-K 77.05 J/g-K gas

How much energy (in kJ) does it take to turn 42.00 g of octane (C3H18) at 99.95°C into a gas at 164.87°C? Use the following reference table to help answer this question: Melting Point -46.53°C Boiling Point 124.05°C AHfus 27.548 kJ/mol AHvap 49.342 kJ/mol Cs, solid 33.03 J/g-K Cs, liquid 338.46 J/g-K 77.05 J/g-K gas

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 39QRT

See similar textbooks

Similar questions

A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0C. The reaction is 2Na(s)+2H2O(l)2NaOH(aq)+H2(g)H=368kJ Assuming no heat loss to the surroundings, will the ice melt? Assuming the final mixture has a specific heat capacity of 4.18 J/gc, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.
The molar heat of fusion of sodium metal is 2.60 kJ/mol, whereas its heat of vaporization is 97.0 kJ/mol. a. Why is the heat of vaporization so much larger than the heat of fusion? b. What quantity of heat would be needed to melt 1.00 g sodium at its normal melting point? c. What quantity of heat would be needed to vaporize 1.00 g sodium at its normal boiling point? d. What quantity of heat would be evolved if 1.00 g sodium vapor condensed at its normal boiling point?
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.
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.
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.
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.