Given the known heat of vaporization (delta H vap) of water is 44.01 kJ/mole, findthe percent error using the experimentally determined delta H vap of 44.42kJ/mole. Express with units of % in the units box.

The experimental value given = 44.42 KJ/mol and since the real value is = 44.01 KJ/mol hence the…

Answered: Given the known heat of vaporization…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter11: Intermolecular Forces And Liquids

Section: Chapter Questions

Problem 66SCQ

See similar textbooks

Similar questions

Chloroform, CHCl3, a volatile liquid, was once used as an anesthetic but has been replaced by safer compounds. Chloroform boils at 61.7C and has a heat of vaporization of 31.4 kJ/mol. What is its vapor pressure at 37.2C?
Why does sweating cool the human body?
What mass (g) of ethanol, CH3CH2OH(), can be vaporized at its boiling point of 78.4 C by transfer of 500. kJ to the liquid? The vapH of ethanol is 38.6 kJ/mol at this temperature.
Give only typing answer with explanation and conclusion 1. Given the known heat of vaporization (delta H vap) of water is 44.01 KJ/mole, find the percent error using the experimentally determine delta H vap of 41.55 Kj/mole. express with units of % hint: percent = - experimental value - known value/known value x 100%
Complete the following table. Calculate the vapor pressure, mm Hg, for each run. Vaporpressure, Pvapor = Pequil - Pinitial. Enter T and Pvapor from the preceding table in the following table. Complete the table by calculating the temperature in degrees Kelvin, the inverse of the temperature in degrees Kelvin, construct a graph of the natural logarithm of the measured vapor pressure,ln(Pvapor), versus1Twhere T is the average Kelvin temperature using the data from the four vapor pressure determinations.
A 337.2 g sample of acetone gas with a temperature of 56.0°C is converted to a liquid with a temperature of 56.0°C. How much heat is involved? Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°C
What would be the final temperature of thesystem is 70 grams of lead at 150 degrees C is dropped into 30 grams of water at 20 degrees C in an insulated container? Specific heat of liquid water is 4.18 J/g*degC Specific heat of lead (solid) is 0.128 J/g*deg C --- I keep coming up wtih an absurb number and wonder if I'm and missing a heat of vaporizaton somewhere. I'm looking for the solution. I was basing this on: (70g)(0.128J/g*deg C)[(150 -x)deg C] = (30g)(4.18J/g*deg C)[(x+20)deg C)]. I'm missing something! Thanks, Heather (middle name)
The vapor pressure of CCl3FCCl3F at 300 KK is 856 torrtorr. If 11.5 gg of CCl3FCCl3F is enclosed in a 1.0 LL container, calculate the number of moles of CCl3FCCl3F in the gas phase. Express your answer using two significant figures.
A 791.0 g sample of acetone sitting in the lab has a temperature of 21.7°C. How much heat would be involved in lowering the temperature of the acetone to -200.0°C? Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°C
A phase is a physical property of which describes the distance of molecules of matter. Phase also describe the arrangement of molecules in a system Which statement is true? none of teh statements is true only the second statement is true only the first statement is true Both statements are true
1. Suppose the sun were used as a heat source to warm some water in a solar-heated house or swimming pool. How much (solar) energy (in both kcal and kJ) is stored in a filled 750-liter water tank when the temperature of the water is raised from 25EC to 65EC? 2. How many kcal are needed to convert 20 g of ice at 0EC to steam at 100EC? 3. What would be the final temperature of the water resulting from the addition of 20 g of steam at 100EC to 80 g of ice at 0EC?
How much heat in KJ is needed to convert 150 grams of frozen acetone at -100oC to vapor at 80oC. Molecular weight of acetone= 58.08 g/mole Boiling point of acetone = 56 oC melting point of acetone = -95oC density of Acetone = 0.7845 g/mL Specific heat of acetone (liquid) = 2.57 J/g oC Specific heat of acetone (gas) = 1.60 J/g oC Specific heat of acetone (lsolid) = 1.65 J/g oC Heat of vaporization = +31.3 kJ/mol heat of fusion = 5.7 kJ/mol q1 = q2 = q3 = q4 = q5 = qtotal =

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Chemistry for Today: General, Organic, and Bioche…

Chemistry

ISBN:

9781305960060

Author:

Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Publisher:

Cengage Learning

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

SEE MORE TEXTBOOKS

Given the known heat of vaporization (delta H vap) of water is 44.01 kJ/mole, find the percent error using the experimentally determined delta H vap of 44.42 kJ/mole. Express with units of % in the units box.