Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 20.5, Problem 2RC
Interpretation Introduction
Interpretation: It should be determined for the following fuel provides the greatest amount of energy per gram.
Concept Introduction:
A fuel having higher calorific values is considered to be a good fuel.
Hydrogen gas has the highest calorific value of 150 KJ/g among all the fuels.
So the Hydrogen as is considers be an extremely good fuel.
But however, hydrogen gas is not used as a fuel in homes and industries.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
(a) What quantity of charge (in coulombs) is a fully charged 1.34-V zinc–mercuric oxide watch battery theoretically capable of furnishing if the mass of HgO in the battery is 0.50 g?(b) What is the theoretical maximum amount of work (in joules) that can be obtained from this battery?
Copper from a 200.0 mL solution of copper (II) sulfate is plated on to the cathode of an electrolytic cell. (a) Hydronium ions are generated at one of the electrodes. Is this electrode the anode or cathode? (b) How many moles of H3O+ are generated if a current of 0.120 A is applied to the cell for 30.0 h? (c) If the pH of the solution was initially 7.0, what will be the pH of the solution after the electrolysis? Assume no change in the volume of solution.
19. (a) Write a balanced equation for the reaction that occurs in a car battery when the ignition key is
turned on. (b) Suppose that constant current of 450 A flowing through the engine for at least 10.0
seconds is needed to start a pick-up truck. How many grams of lead are consumed during this time?
(c) If the battery operates at 12 V of potential, how much energy (in kJ) is produced?
Chapter 20 Solutions
Chemistry & Chemical Reactivity
Ch. 20.1 - Prob. 1RCCh. 20.1 - Prob. 2RCCh. 20.2 - Prob. 1RCCh. 20.2 - Prob. 2RCCh. 20.3 - Prob. 1RCCh. 20.3 - Prob. 2RCCh. 20.3 - Prob. 3RCCh. 20.4 - Prob. 1RCCh. 20.4 - Prob. 2RCCh. 20.4 - 3. Which of the following is a renewable energy...
Ch. 20.5 - Prob. 1RCCh. 20.5 - Prob. 2RCCh. 20.6 - Prob. 1QCh. 20.6 - Prob. 1RCCh. 20.7 - Prob. 1QCh. 20.7 - Prob. 2QCh. 20 - In the discussion on the composition of air,...Ch. 20 - Prob. 2PSCh. 20 - Prob. 3PSCh. 20 - Dinitrogen monoxide, N2O (commonly called nitrous...Ch. 20 - Prob. 5PSCh. 20 - Prob. 6PSCh. 20 - Prob. 9PSCh. 20 - Although there are a number of...Ch. 20 - Prob. 12PSCh. 20 - Prob. 13PSCh. 20 - Prob. 14PSCh. 20 - Prob. 15PSCh. 20 - Prob. 17PSCh. 20 - The enthalpy of combustion of isooctane (C8H18),...Ch. 20 - Energy consumption in the United States amounts to...Ch. 20 - Prob. 20PSCh. 20 - Prob. 23PSCh. 20 - Prob. 25PSCh. 20 - Prob. 28PSCh. 20 - In methane hydrate the methane molecule is trapped...Ch. 20 - Prob. 30PSCh. 20 - Prob. 31PSCh. 20 - Prob. 32PSCh. 20 - Prob. 33PSCh. 20 - Prob. 34PSCh. 20 - Prob. 35GQCh. 20 - Prob. 36GQCh. 20 - Prob. 37GQCh. 20 - Prob. 38GQCh. 20 - Prob. 40GQCh. 20 - Prob. 41ILCh. 20 - Prob. 42ILCh. 20 - Define the terms renewable and nonrenewable as...Ch. 20 - Prob. 44SCQCh. 20 - Prob. 45SCQCh. 20 - Prob. 46SCQCh. 20 - Prob. 47SCQCh. 20 - What is the likelihood that hydrogen (H2) will...Ch. 20 - Prob. 49SCQCh. 20 - Which sulfur compounds are atmospheric pollutants?...
Knowledge Booster
Similar questions
- A lead storage battery delivers a current of 6.00 A for one hour and 22 minutes at a voltage of 12.0 V. (a) How many grams of lead are converted to PbSO4? (b) How much electrical energy is produced in kilowatt hours?arrow_forwardZinc is produced by electrolytic refining. The electrolytic process, which is similar to that for copper, can be represented by the two half-reactions Zn(impure,s)Zn2++2eZn2++2eZn(pure,s) For this process, a voltage of 3.0 V is used. How many kilowatt hours are needed to produce one metric ton of pure zinc?arrow_forwardAn electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?arrow_forward
- An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?arrow_forwardConsider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)arrow_forwardA voltaic cell consists of a copper electrode in a solution of copper (II) ions and a palladium electrode in a solution of palladium (II) ions. The palladium is the cathode and its reduction potential is 0.951 V. (a) Write the half-reaction that occurs at the anode. (b) If E° is 0.609 V, what is the potential for the oxidation half- reaction? (c) What is Keq for this reaction?arrow_forward
- An electrolysis cell contains a solution of 0.10 M NiSO4. The anode and cathode are both strips of Pt foil. Another electrolysis cell contains the same solution, but the electrodes are strips of Ni foil. In each case a current of 0.10 A flows through the cell for 10 hours.(a) Write a balanced equation for the chemical reaction that occurs at the anode in each cell.(b) Calculate the mass, in grams, of the product formed at the anode in each cell. (The product may be a gas, a solid, or an ionic species in solution.)arrow_forward21.30 Consider the following voltaic cell: Voltmeter Zn Со Salt bridge 1 M Co2+ (a) In which direction do electrons flow in the external circuit? (b) In which half-cell does reduction occur? (c) In which half-cell do electrons leave the cell? (d) At which electrode are electrons generated? (e) Which electrode is positively charged? (f) Which electrode increases in mass during cell operation? (g) Suggest a solution for the anode electrolyte. (h) Suggest a pair of ions for the salt bridge. (i) For which electrode could you use an inactive material? (i) In which direction do cations within the salt bridge move to maintain charge neutrality? (k) Write balanced half-reactions and an overall cell reaction.arrow_forwardWhen chlorine gas is bubbled through an aqueous solution of NaBr, chloride ions and liquidbromine are the products of the spontaneous reaction. For this cell, (a) Draw a sketch of the cell, labeling the anode, the cathode, and the direction of electron flow. (b) Write the half-reaction that takes place at the anode and at the cathode. (c) Write a balanced equation for the cell reaction. (d) Write an abbreviated notation for the cell.arrow_forward
- Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold as this metal naturally has a yellow tone. If 1.91 g of rhodium is deposited at the cathode when a current of 6.65 A passes through an electrolytic cell for 1620 seconds, what is the oxidation state of rhodium in the aqueous solution? (MW of rhodium=102.91 g/mol; Faraday constant = 96485 C/mol e`). Oxidation number in this case refers to the charge of the ion. Input the value of the oxidation number (no symbols included).arrow_forwardAn aqueous solution of copper sulphate, CuS04 was electrolysed between platinum electrodes using a current of 0.1287 ampere for 50 minutes. [Atomic mass of Cu = 63.5 g mol-1](a) Write the cathodic reaction.(b) Calculate:(i) Electric charge passed during electrolysis (ii) Mass of copper deposited at the cathode [Given: 1F = 96,500 C mol-1]arrow_forwardAluminum metal is produced by electrolysis of Al2O3 in molten cryolite (Na3AlF6). (a) If the electrolytic cell operates at 3.0 V and 1.5 x 10° A, how many grams of aluminum can be produced in 1.0 hour of continuous electrolysis? (b) How long does it take to produce 1.00 kg of aluminum? (c) How many kWh of energy is consumed to produce 1.00 kg of aluminum? 7.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning