Chemistry: Atoms First
Chemistry: Atoms First
2nd Edition
ISBN: 9780073511184
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
Question
Book Icon
Chapter 12, Problem 12.65QP
Interpretation Introduction

Interpretation:

The heat required to convert 866 g of ice at -15°C to steam at 146°C should be calculated.

Concept Introduction:

Specific heat of a substance refers to the quantity of heat per unit mass of substance that rises the temperature of the substance by one degree Celsius.  The quantity of heat added and the specific heat is related as follows –

q = m×s×ΔTwhere q = heat added          m = mass of the substance           s  =  specific heat of the substance        ΔT =  change in Temperature 

Molar heat of vaporization is the heat energy required to boil one mole of a substance at its boiling point.

Molar heat of fusion is the heat energy required to melt one mole of the substance at its melting point.

Expert Solution & Answer
Check Mark

Answer to Problem 12.65QP

The heat required to convert 212.8 g of ice at -15°C to steam at 138°C is calculated as 758.32 kJ.

Explanation of Solution

Calculate the heat required to warm ice to melting point.

given data:  mass of ice, m = 866 gspecific heat of ice, s = 2.03 J/g .°CT1 = -15°C, T2 = 0°C ; ΔT = T2-T1= 0°C -(-15°C) = 15°C           heat required to warm ice to its melting point ,            q1 = m s ΔT = 866 g× 2.03 J/g .°C× 15°C                = 26.4 kJ

The ice is warmed from -15°C to its melting point 0°C which are initial and final temperature respectively.  Specific heat of ice is known and the parameters are substituted in the equation q = m ××ΔT, where ‘q’ correlates to the heat utilized in the process of warming ice from -15°C to its melting point 0°C.

Calculate the heat required to convert ice to liquid water at its melting point.

mass of water = 866 gmolar mass of water = 18.02 g/molno.of moles of water = mass of watermolar mass of water                                 =  866 g18.02 g/mol=48.06 molwe know,heat required to convert one mole of ice to liquid water at 0°C = 26.4 kJ/mol.therefore,heat required to convert 48.06 mol of ice to liquid water at 0°C,q4 = 6.0 kJ/mol × 48.06 mol = 288.36 kJ

Mass of water is converted to number of moles.  The heat required to convert one mole of ice to liquid water at its melting point is known which is termed as molar heat of fusion.  The number of water in given mass of ice (water) is obtained by multiplying with the standard value.

Calculate the heat required to heat water from 0°C to its boiling point 100°C.

known data:  mass of ice, m = 866 gspecific heat of water, s = 4.184 J/g .°CT1 = 0°C, T2 = 100°C ; ΔT = T2-T1= 100°C - 0°C = 100°C       heat required to warm ice to its melting point ,        q3 = m s ΔT = 866 g× 4.184 J/g .°C× 100°C            = 362.3 kJ

Water is heated from its melting point 0°C  to its boiling point 100°C which are initial and final temperature respectively.  Specific heat of water is known and the parameters are substituted in the equation q = m ××ΔT where ‘q’ correlates to the heat utilized in the process of heating ice from its melting point 0°C to its boiling point 100°C.

Calculate the heat required to convert 866 g water to steam at its boiling point.

mass of water = 866 gmolar mass of water = 18.02 g/molno.of moles of water = mass of watermolar mass of water                                 =  866 g18.02 g/mol=48.06 mol

we know,heat required to convert one mole of water to steam at 100°C = 40.79 kJ/mol.therefore,heat required to convert 48.06 mol of water to steam at 100°C,q4 = 40.79 kJ/mol × 48.06 mol = 1.96kJ

Mass of water is converted to number of moles.  The heat required to convert one mole of water to steam at its boiling point is known which is termed as molar heat of vaporization.  The number of water in given mass of ice (water) is obtained by multiplying with the standard value.

Calculate the heat required to raise the temperature of steam from 100°C to 146°C.

known data:  mass of ice, m = 866 gspecific heat of Steam, s = 1.99 J/g .°C T1 = 100°C, T2 = 146°C ; ΔT = T2-T1= 146°C - 100°C = 46°C heat required to warm ice to its melting point ,            q5 = m s ΔT = 866 g× 1.99 J/g .°C× 46°C                = 79.3 kJ.

The temperature of steam has to be risen from 100°C  to 138°C which are initial and final temperature respectively.  Specific heat of steam is known and the parameters are substituted in the equation q = m ××ΔT where ‘q’ correlates to the heat utilized in the process of rising the temperature of steam.

Calculate the total heat energy utilized to convert 866 g of ice at -15°C to steam at 146°C

q = q1+q2+q3+q4+q5q = 26.4 kJ + 288.36 kJ + 362.3 kJ +1.96 kJ + 79.3 kJ = 758.32 kJ

The total heat energy utilized to convert 866 g of ice at -15°C to steam at 146°C is equivalent to sum of the heat energy required in the processes of required to warm ice to melting point, convert ice to liquid water at its melting point, heating water from 0°C to its boiling point 100°C, converting  water to steam at its boiling point and rising the temperature of steam from 100°C to 146°C.

Conclusion

The heat required to convert 866 g of ice at -15°C to steam at 146°C was calculated.

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 12 Solutions

Chemistry: Atoms First

Ch. 12.3 - The density of sodium metal is 0.971 g/cm3 and the...Ch. 12.3 - Prob. 12.3.1SRCh. 12.3 - Prob. 12.3.2SRCh. 12.4 - How many of each ion are contained within a unit...Ch. 12.4 - Referring to Figure 12.23, determine how many of...Ch. 12.4 - Referring to Figure 12.23, determine how many of...Ch. 12.4 - Prob. 3PPCCh. 12.4 - The edge length of the NaCl unit cell is 564 pm....Ch. 12.4 - Prob. 4PPACh. 12.4 - NiO also adopts the face-centered cubic...Ch. 12.4 - The metal iridium (Ir) crystallizes with a...Ch. 12.4 - Prob. 5PPACh. 12.4 - Copper crystallizes in a face-centered cubic...Ch. 12.4 - Given that the diameter and average mass of a...Ch. 12.5 - (a) Calculate the amount of heat deposited oil the...Ch. 12.5 - Calculate the amount of energy (in kilojoules)...Ch. 12.5 - Determine the final state and temperature of 100 g...Ch. 12.5 - Prob. 6PPCCh. 12.5 - Prob. 12.5.1SRCh. 12.5 - Prob. 12.5.2SRCh. 12.6 - Using the following phase diagram, (a) determine...Ch. 12.6 - Use the following phase diagram to (a) determine...Ch. 12.6 - Prob. 7PPBCh. 12.6 - Prob. 7PPCCh. 12.6 - Prob. 12.6.1SRCh. 12 - Explain why liquids, unlike gases, are virtually...Ch. 12 - What is surface tension? What is the relationship...Ch. 12 - Prob. 12.3QPCh. 12 - Prob. 12.4QPCh. 12 - Prob. 12.5QPCh. 12 - Prob. 12.6QPCh. 12 - Prob. 12.7QPCh. 12 - Why does the viscosity of a liquid decrease with...Ch. 12 - Why is ice less dense than water?Ch. 12 - Prob. 12.10QPCh. 12 - Prob. 12.11QPCh. 12 - Prob. 12.12QPCh. 12 - Prob. 12.13QPCh. 12 - Predict which of the following liquids has greater...Ch. 12 - Prob. 12.15QPCh. 12 - Vapor pressure measurements at several different...Ch. 12 - The vapor pressure of liquid X is lower than that...Ch. 12 - Prob. 12.18QPCh. 12 - Prob. 12.19QPCh. 12 - Define the following terms: crystalline solid,...Ch. 12 - Prob. 12.21QPCh. 12 - Classify the solid states in terms of crystal...Ch. 12 - Prob. 12.23QPCh. 12 - Define X-ray diffraction. What are the typical...Ch. 12 - Prob. 12.25QPCh. 12 - What is the coordination number of each sphere in...Ch. 12 - Calculate the number of spheres that would be...Ch. 12 - Prob. 12.28QPCh. 12 - Barium metal crystallizes in a body-centered cubic...Ch. 12 - Prob. 12.30QPCh. 12 - Europium crystallizes in a body-centered cubic...Ch. 12 - Crystalline silicon has a cubic structure. The...Ch. 12 - Prob. 12.33QPCh. 12 - Prob. 12.34QPCh. 12 - Prob. 12.35QPCh. 12 - Prob. 12.36QPCh. 12 - Shown here is a zinc oxide unit cell. What is the...Ch. 12 - Describe and give examples of the following types...Ch. 12 - Prob. 12.39QPCh. 12 - A solid is hard, brittle, and electrically...Ch. 12 - A solid is soft and has a low melting point (below...Ch. 12 - Prob. 12.42QPCh. 12 - Which of the following are molecular solids and...Ch. 12 - Prob. 12.44QPCh. 12 - Prob. 12.45QPCh. 12 - What is a phase change? Name all possible changes...Ch. 12 - What is the equilibrium vapor pressure of a...Ch. 12 - Use any one of the phase changes to explain what...Ch. 12 - Define the following terms: (a) molar heat of...Ch. 12 - Prob. 12.50QPCh. 12 - What can we learn about the intermolecular forces...Ch. 12 - The greater the molar heat of vaporization of a...Ch. 12 - Prob. 12.53QPCh. 12 - A closed container of liquid pentane (bp = 36.1C)...Ch. 12 - What is critical temperature? What is the...Ch. 12 - Prob. 12.56QPCh. 12 - How do the boiling points and melting points of...Ch. 12 - Prob. 12.58QPCh. 12 - Prob. 12.59QPCh. 12 - Prob. 12.60QPCh. 12 - Which of the following phase transitions gives off...Ch. 12 - Prob. 12.62QPCh. 12 - Prob. 12.63QPCh. 12 - Prob. 12.64QPCh. 12 - Prob. 12.65QPCh. 12 - Prob. 12.66QPCh. 12 - Prob. 12.67QPCh. 12 - How is the rate of evaporation of a liquid...Ch. 12 - Explain why steam at 100C causes more serious bums...Ch. 12 - The following compounds, listed with then- boiling...Ch. 12 - Prob. 12.71QPCh. 12 - Prob. 12.72QPCh. 12 - Explain how waters phase diagram differs from...Ch. 12 - The blades of ice skates are quite thin, so the...Ch. 12 - A length of wire is placed on top of a block of...Ch. 12 - Prob. 12.76QPCh. 12 - A phase diagram of water is shown. Label the...Ch. 12 - Prob. 12.78QPCh. 12 - Prob. 12.79QPCh. 12 - Prob. 12.80QPCh. 12 - Prob. 12.81QPCh. 12 - Prob. 12.82QPCh. 12 - The average distance between base pairs measured...Ch. 12 - A CO2 fire extinguisher is located on the outside...Ch. 12 - What is the vapor pressure of mercury at its...Ch. 12 - Prob. 12.86QPCh. 12 - The liquid-vapor boundary line in the phase...Ch. 12 - Prob. 12.88QPCh. 12 - Prob. 12.89QPCh. 12 - A student is given four solid samples labeled W,...Ch. 12 - Prob. 12.91QPCh. 12 - The diagram shows a kettle of boiling water....Ch. 12 - The south pole of Mars is covered with solid...Ch. 12 - The properties of gases, liquids, and solids...Ch. 12 - The standard enthalpy of formation of gaseous...Ch. 12 - Prob. 12.96QPCh. 12 - Under the same conditions of temperature and...Ch. 12 - The distance between Li+ and Cl is 257 pm in solid...Ch. 12 - Heat of hydration, that is, the heat change that...Ch. 12 - The fluorides of the second period elements and...Ch. 12 - Calculate the H for the following processes at...Ch. 12 - Prob. 12.102QPCh. 12 - Prob. 12.103QPCh. 12 - Ozone (O3) is a strong oxidizing agent that can...Ch. 12 - A sample of limestone (CaCO3) is heated in a...Ch. 12 - Carbon and silicon belong to Group 4A of the...Ch. 12 - Prob. 12.107QPCh. 12 - A 1.20-g sample of water is injected into an...Ch. 12 - What are the advantages of cooking the vegetable...Ch. 12 - A quantitative measure of how efficiently spheres...Ch. 12 - The phase diagram of helium is shown. Helium is...Ch. 12 - The phase diagram of sulfur is shown. (a) How many...Ch. 12 - Prob. 12.113QPCh. 12 - Argon crystallizes in the face-centered cubic...Ch. 12 - Given the phase diagram of carbon, answer the...Ch. 12 - Prob. 12.116QPCh. 12 - Swimming coaches sometimes suggest that a drop of...Ch. 12 - Prob. 12.118QPCh. 12 - Why do citrus growers spray their trees with water...Ch. 12 - Calcium metal crystallizes in a face-centered...Ch. 12 - A student heated a beaker of cold water (on a...Ch. 12 - The compound diclilorodifluoromethane (CCl2F2) has...Ch. 12 - Iron crystallizes in a body-centered cubic...Ch. 12 - Sketch the cooling curves of water from about 110C...Ch. 12 - Prob. 12.125QPCh. 12 - A sampleof water shows the following behavior as...Ch. 12 - A closed vessel of volume 9.6 L contains 2.0 g of...Ch. 12 - The electrical conductance of copper metal...Ch. 12 - Assuming ideal behavior, calculate the density of...Ch. 12 - Explain why drivers are advised to use motor oil...Ch. 12 - Prob. 12.131QPCh. 12 - Silicon used in computer chips must have an...Ch. 12 - Prob. 12.133QPCh. 12 - Prob. 12.1KSPCh. 12 - Prob. 12.2KSPCh. 12 - Prob. 12.3KSPCh. 12 - Prob. 12.4KSP
Knowledge Booster
Background pattern image
Recommended textbooks for you
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY