Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
bartleby

Concept explainers

bartleby

Videos

Textbook Question
Book Icon
Chapter 6, Problem 137CP

You have a l.00-mole sample of water at −30.°C and you heat it until you have gaseous water at 140.°C. Calculate q for the entire process. Use the following data.

Specific heat capacity of ice = 2.03 J/ ° C g Specific heat capacity of water = 4.18 J/ ° C g Specific heat capacity of steam = 2.02 J/ ° C g

H 2 O ( s ) H 2 O ( l ) Δ H fusion = 6.02 KJ/mol ( at 0 ° C ) H 2 O ( l ) H 2 O ( g ) Δ H vaporization = 40.7 KJ/mol ( at 100 . ° C )

Expert Solution & Answer
Check Mark
Interpretation Introduction

Interpretation: The amount of heat required to convert 1.00 mol of H2O(s) at -30°C to H2O(g) at 140°C should be determined.

Concept Introduction:

The heat capacity C is defined as the relation of heat absorbed to the temperature change. It can be given by,

                                           C = Heat absorbedTemperature change......(1)

Require heat for an one gram of substance raise to its temperature by one degree Celsius is called specific heat capacity.

Absorbed heat (J)=Specific heat capacity×Temperature change(c)×mass ofsubstance (g)......(2)

For the above equation heat is:

                                    S = q×M×T.....(1)

                                                      q is heat (J)

                                                      M is mass of sample (g)

                                                      S is specific heat capacity (J/°C·g.)

                                                      T is temperature change (C)

For the process no heat loss to the surroundings means then the heat is

                   (absorbed)-q×M×ΔT=-q×M×ΔT(released)......(3)'

Answer to Problem 137CP

Answer

The amount of heat required to convert 1.00 mol of H2O(s) at -30°C to H2O(g) at 140°C is 56.9kJ.

Explanation of Solution

Explanation

Record the given data:

                 Specific heat capacity of ice = 2.03J/°C· g

                 Specific heat capacity of water = 4.18 J/°C · g

                 Specific heat capacity of steam = 2.02J/°C· g

     Sample water is l.00 mole

                  Initial temperature is - 30°C

                  Final temperature is - 140°C.

                    H2O(s) H2O(l)ΔΗfusion=6.02kJ/mol(at0°C)H2O(l)H2O(g)ΔΗvaporization=40.7kJ/mol(at100°C)

To calculate the required to heat H2O(s) from -30°C to 0°C.

                      q(1)=2.30J°C.g×18.2g×(0-(-30))°C=1.1×103J

  • The given values are plugging in equation (1) to give the required to heat H2O(s) from -30°C to 0°C.
  • Required heat for vaporization of 1 mole of water is 1.1×103J.

To calculate the required heat (q) to convert 1 mol H2O(s) at 0°C  into 1 mol H2O(l) at 0°C.

                          q(1)=1.00mol×6.02×103J/mol=6.02×103J

  • The given enthalpy of fusion is multiplied by the mole of water to give required heat (q) to convert 1 mol H2O(s) at 0°C into H2O(l) at 0°C.
  • Required heat (q) to convert 1 mol H2O(s) at 0°C  into H2O(l) at 0°C is 6.02×103J.

To calculate the required to heat H2O(l) from 0°C to 100°C.

                      q(3)=4.18J°C.g×18.2g×(100-0)°C=7.53×103J

  • The given values are plugging in equation (1) to give the required to heat H2O(l) from 0°C to 100°C.
  • Required to heat H2O(l) from 0°C to 100°C is 7.53×103J.

To calculate the required to convert 1 mol H2O(l) at 100°C into 1 mol H2O(g) at 100°C.

                   q(4)=1.00mol×40.7×103J/mol=4.07×104J

The given enthalpy of vaporization is multiplied by the mole of water to give required to convert 1 mol H2O(l) at 100°C into 1 mol H2O(g) at 100°C.

To calculate the required to heat H2O(g) from 100°C to 140°C.

                          q(5)=2.30J°C.g×18.2g×(140100)°C=1.5×103J

  • The given values are plugging in equation (1) to give required to heat H2O(g) from 100°C to 140°C.
  • Required to heat H2O(g) from 100°C to 140°C is 1.5×103J.

To calculate the amount of heat required to convert 1.00 mol of H2O(s) at -30°C to H2O(g) at 140°C.

                           qtotal=q1+q2+q3+q4+q5qtotal=1.1×103J+6.02×103J+7.53×103J+4.07×104J+1.5×103J=5.69×104J= 56.9kJ

Conclusion

Conclusion

The heat required to convert 1.00 mol of H2O(s) at -30°C to H2O(g) at 140°C was calculated by using given specific heat capacities of water and temperatures and enthalpies and the amount of heat required to convert 1.00 mol of H2O(s) at -30°C to H2O(g) at 140°C was found to be 56.9kJ.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 6 Solutions

Chemistry

Ch. 6 - What is meant by the term lower in energy? Which...Ch. 6 - A fire is started in a fireplace by striking a...Ch. 6 - Liquid water turns to ice. Is this process...Ch. 6 - Consider the following statements: ''Heat is a...Ch. 6 - Consider 5.5 L of a gas at a pressure of 3.0 atm...Ch. 6 - Consider 5.5 L of a gas at a pressure of 3.0 atm...Ch. 6 - What if energy was not conserved? How would this...Ch. 6 - Hesss law is really just another statement of the...Ch. 6 - In the equation w = P V, why is there a negative...Ch. 6 - Consider an airplane trip from Chicago, Illinois,...Ch. 6 - How is average bond strength related to relative...Ch. 6 - Assuming gasoline is pure C8H18(l), predict the...Ch. 6 - What is the difference between H and E?Ch. 6 - The enthalpy change for the reaction...Ch. 6 - Explain why oceanfront areas generally have...Ch. 6 - The equation for the fermentation of glucose to...Ch. 6 - Explain why H is obtained directly from coffee-cup...Ch. 6 - The enthalpy of combustion of CH4(g) when H2O (1)...Ch. 6 - The enthalpy change for a reaction is a state...Ch. 6 - Standard enthalpies of formation are relative...Ch. 6 - The combustion of methane can be represented as...Ch. 6 - Why is it a good idea to rinse your thermos bottle...Ch. 6 - Prob. 26QCh. 6 - What is incomplete combustion of fossil fuels? Why...Ch. 6 - Explain the advantages and disadvantages of...Ch. 6 - Prob. 29ECh. 6 - Which has the greater kinetic energy, an object...Ch. 6 - Consider the following diagram when answering the...Ch. 6 - A gas absorbs 45 kJ of heat and does 29 kJ of...Ch. 6 - Calculate E for each of the following. a. q = 47...Ch. 6 - A system undergoes a process consisting of the...Ch. 6 - If the internal energy of a thermodynamic system...Ch. 6 - Calculate the internal energy change for each of...Ch. 6 - A sample of an ideal gas at 15.0 atm and 10.0 L is...Ch. 6 - A piston performs work of 210. L atm on the...Ch. 6 - Consider a mixture of air and gasoline vapor in a...Ch. 6 - As a system increases in volume, it absorbs 52.5 J...Ch. 6 - A balloon filled with 39.1 moles of helium has a...Ch. 6 - One mole of H2O(g) at 1.00 atm and 100.C occupies...Ch. 6 - One of the components of polluted air is NO. It is...Ch. 6 - The reaction SO3(g)+H2O(l)H2SO4(aq) is the last...Ch. 6 - Are the following processes exothermic or...Ch. 6 - Are the following processes exothermic or...Ch. 6 - The overall reaction in a commercial heat pack can...Ch. 6 - Consider the following reaction:...Ch. 6 - Consider the combustion of propane:...Ch. 6 - Consider the following reaction:...Ch. 6 - For the process H2O(l) H2O(g) at 298 K and 1.0...Ch. 6 - For the following reactions at constant pressure,...Ch. 6 - Consider the substances in Table 7-1. Which...Ch. 6 - The specific heat capacity of silver is 0.24 J/Cg....Ch. 6 - A 500-g sample of one of the substances listed in...Ch. 6 - It takes 585 J of energy to raise the temperature...Ch. 6 - A 30.0-g sample of water at 280. K is mixed with...Ch. 6 - A biology experiment requires the preparation of a...Ch. 6 - A 5.00-g sample of aluminum pellets (specific heat...Ch. 6 - Hydrogen gives off 120. J/g of energy when burned...Ch. 6 - A 150.0-g sample of a metal at75.0C is added to...Ch. 6 - A 110.-g sample of copper (specific heat capacity...Ch. 6 - In a coffee-cup calorimeter, 50.0 mL of 0.100 M...Ch. 6 - In a coffee-cup calorimeter, 100.0 mL of 1.0 M...Ch. 6 - A coffee-cup calorimeter initially contains 125 g...Ch. 6 - In a coffee-cup calorimeter, 1.60 g NH4NO3 is...Ch. 6 - Consider the dissolution of CaCl2:...Ch. 6 - Consider the reaction...Ch. 6 - Quinone is an important type of molecule that is...Ch. 6 - The energy content of food is typically determined...Ch. 6 - The heat capacity of a bomb calorimeter was...Ch. 6 - The combustion of 0.1584 g benzoic acid increases...Ch. 6 - The enthalpy of combustion of solid carbon to form...Ch. 6 - Combustion reactions involve reacting a substance...Ch. 6 - Given the following data calculate H for the...Ch. 6 - Prob. 78ECh. 6 - The bombardier beetle uses an explosive discharge...Ch. 6 - Calculate H for the reaction...Ch. 6 - Given the following data...Ch. 6 - Given the following data...Ch. 6 - Give the definition of the standard enthalpy of...Ch. 6 - Write reactions for which the enthalpy change will...Ch. 6 - Use the values ofHf in Appendix 4 to calculate H...Ch. 6 - Use the values of Hf in Appendix 4 to calculate H...Ch. 6 - The Ostwald process for the commercial production...Ch. 6 - Calculate H for each of the following reactions...Ch. 6 - The reusable booster rockets of the space shuttle...Ch. 6 - The space shuttle Orbiter utilizes the oxidation...Ch. 6 - Consider the reaction...Ch. 6 - The standard enthalpy of combustion of ethene gas,...Ch. 6 - Water gas is produced from the reaction of steam...Ch. 6 - Syngas can be burned directly or converted to...Ch. 6 - Ethanol (C2H5OH) has been proposed as an...Ch. 6 - Methanol (CH3OH) has also been proposed as an...Ch. 6 - Some automobiles and buses have been equipped to...Ch. 6 - Acetylene (C2H2) and butane (C4H10) are gaseous...Ch. 6 - Prob. 99ECh. 6 - The complete combustion of acetylene, C2H2(g),...Ch. 6 - It has been determined that the body can generate...Ch. 6 - One way to lose weight is to exercise! Walking...Ch. 6 - Three gas-phase reactions were run in a...Ch. 6 - Nitrogen gas reacts with hydrogen gas to form...Ch. 6 - Combustion of table sugar produces CO2(g) and H2O(...Ch. 6 - Prob. 106AECh. 6 - A serving size of six cookies contains 4 g of fat,...Ch. 6 - Calculate H for the reaction...Ch. 6 - The enthalpy of neutralization for the reaction of...Ch. 6 - Given the following data: NO2(g) NO(g) + O(g)H =...Ch. 6 - If a student performs an endothermic reaction in a...Ch. 6 - In a bomb calorimeter, the reaction vessel is...Ch. 6 - The bomb calorimeter in Exercise 102 is filled...Ch. 6 - Consider the two space shuttle fuel reactions in...Ch. 6 - Consider the following equations:...Ch. 6 - Given the following data...Ch. 6 - At 298 K, the standard enthalpies of formation for...Ch. 6 - Using the following data, calculate the standard...Ch. 6 - A sample of nickel is heated to 99.8C and placed...Ch. 6 - Given: 2Cu2O(s) + O2(g) 4CuO(s)H = 288 kJ Cu2O(s)...Ch. 6 - Calculate H for each of the following reactions,...Ch. 6 - Consider a balloon filled with helium at the...Ch. 6 - In which of the following systems is(are) work...Ch. 6 - Which of the following processes are exothermic?...Ch. 6 - Consider the reaction...Ch. 6 - A swimming pool, 10.0 m by 4.0 m, is filled with...Ch. 6 - In a coffee-cup calorimeter, 150.0 mL of 0.50 M...Ch. 6 - Calculate H for the reaction...Ch. 6 - Which of the following substances have an enthalpy...Ch. 6 - Consider 2.00 moles of an ideal gas that are taken...Ch. 6 - For the process H2O(l)H2O(g) at 298 K and 1.0 atm,...Ch. 6 - The sun supplies energy at a rate of about 1.0...Ch. 6 - The best solar panels currently available are...Ch. 6 - On Easter Sunday, April 3, 1983, nitric acid...Ch. 6 - A piece of chocolate cake contains about 400...Ch. 6 - The standard enthalpies of formation for S(g),...Ch. 6 - You have a l.00-mole sample of water at 30.C and...Ch. 6 - A 500.0-g sample of an element at 195C is dropped...Ch. 6 - When 1.00 L of 2.00 M Na2SO4 solution at 30.0c is...Ch. 6 - The preparation of NO2(g) from N2(g) and O2(g) is...Ch. 6 - Nitromethane, CH3NO2, can be used as a fuel. When...Ch. 6 - A cubic piece of uranium metal (specific heat...Ch. 6 - A gaseous hydrocarbon reacts completely with...
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
SEE MORE QUESTIONS
Recommended textbooks for you
Text book image
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Text book image
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Text book image
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY