
Concept explainers
How many moles of electrons are required to produce (a) 0.84 L of O2 at exactly 1 atm and 25°C from aqueous H2SO4 solution; (b) 1.50 L of Cl2 at 750 mmHg and 20°C from molten NaCl; (c) 6.0 g of Sn from molten SnCl2?
(a)

Interpretation:
Need to calculate the Faraday of electricity needed for the production of 0.84L of O2 with 1 atm pressure upon electrolysis of aqueous H2SO4 at 25oC.
Concept introduction:
Electrolysis of aqueous sulfuric acid i.e. acidified water resulted in the production of oxygen and hydrogen gas, which will be liberated at the anode and cathode respectively. The presence of H+ and SO-4 made the solution to be more conductivity. SO-4 is more stable to be inert at the anode.
Further the cell reaction can be written as shown below
Since volume and pressure of oxygen produced was given, by applying it into ideal gas equation we can calculate the number of mole of oxygen produced
The ideal gas equation can be given as follows.
On applying the number of moles of oxygen produced into stoichiometry of the reaction, the number of moles electron involved in the reaction can be calculated. In case of the given reaction 4 mole of electron was liberated during the production of one mole of oxygen. Since one Faraday is equal to one mole of electron, so 4 Faraday of electricity will be needed to produce one mole of oxygen.
Finally the Faraday of electricity utilized to produce the required amount of oxygen can be calculated according the formula
To find: Amount of Faraday of electricity need to produce 0.076L of O2 with pressure 755mmHg, at 298K, through electrolysis of water.
Answer to Problem 18.52QP
Ideal gas equation can be used to calculate the number of moles of oxygen produced, from that faraday of electricity needed will be calculated in successive steps (a)
Since one mole of oxygen need 4 Faraday of electricity, so the Faraday of electricity needed to produce
Faraday of electricity need to produce 0.84L of oxygen with pressure 1 atm was calculated as
Explanation of Solution
Ideal gas equation can be used to calculate the number of moles of oxygen produced
Since one mole of oxygen need 4 Faraday of electricity, so the Faraday of electricity needed to produce
Faraday of electricity need to produce 0.84L of oxygen with pressure 1 atm was calculated as
At first the number of moles of oxygen produced through electrolysis was calculated using ideal gas equation, from the given volume and pressure. Thus it was calculated as
The amount of electricity needed to produce 0.84L of oxygen with pressure of 1atm was determined to be
(b)

Interpretation:
Need to calculate the Faraday of electricity needed for the production of 1.50L of Cl2 with pressure 750 mmHg at 20oC by electrolysis of molten NaCl.
Concept introduction:
Electrolysis of molten sodium chloride was represented by the below equation. By using ideal gas equation, the number of moles of chlorine liberated at the anode can be calculated, provided the pressure and volume are known.
The ideal gas equation can be given as follows.
The equation we find that two mole of electron is needed to produce one mole of chlorine gas , Since one Faraday is equal to one mole of electron, The Faraday of electricity utilized to produce given amount of chlorine can be calculated according the formula
To find: Faraday of electricity need to produce 1.50 L of Cl2 with pressure 750mmHg, at 293K, through electrolysis of molten NaCl.
Answer to Problem 18.52QP
Ideal gas equation can be used to calculate the number of moles of chlorine gas produced, Further from the number of moles of chlorine; the faraday of electricity utilized will be calculated in successive steps (b)
Since one mole of chlorine need two Faraday of electricity, so the Faraday of electricity needed to produce
Faraday of electricity need to produce 1.50L of chlorine with pressure 750mm Hg was calculated as
Explanation of Solution
Ideal gas equation can be used to calculate the number of moles of oxygen produced
Since one mole of chlorine need two Faraday of electricity, so the Faraday of electricity needed to produce
The number of moles of chlorine produced through electrolysis was calculated using ideal gas equation, from the given volume and pressure it was calculated as
The amount of electricity needed to produce 1.5 L of chlorine with pressure of 750 mmHg was determined to be
(c)

Interpretation:
Need to calculate the Faraday of electricity needed for the production of 6g of Sn though electrolysis of molten SnCl2.
Concept introduction:
Electrolysis of molten stannous chloride will result in the formation of Tin (Sn) and chlorine gas and half-cell reaction at the anode and cathode was given below. In this two electrons were released by chloride ion at the anode and get liberated as chlorine gas, further stannous ion accept two electron and for tin metal
The ideal gas equation can be given as follows.
Since the mass of the metal produced was given, from that number of moles of Sn can be calculated. Further from the number of moles of Sn produced the Faraday of electricity can be calculated by the formula given below, since one Faraday is equal to one mole of electron. In the present case 2 moles of electrons are needed to reduce one mole of Sn2+
So
To find: Faraday of electricity need to produce 6 g of Tin, by electrolysis of molten SnCl2.
Answer to Problem 18.52QP
From the mass of tin produced during the electrolysis, the Faraday of electricity needed for reaction can be calculated in the following steps (c).
Since one mole of Sn2+ ion need two Faraday of electricity to, so the Faraday of electricity needed to produce
Explanation of Solution
From the molar mass calculation
Weight = 6g
Atomic Mass = 118.7g
Since one mole of Sn2+ ion need two Faraday of electricity, so the Faraday of electricity needed to produce
The number of moles of tin produced through electrolysis was calculated as
The Faraday of electricity need to produce 6g of Tin from by electrolysis of molten SnCl2 was identified as
Want to see more full solutions like this?
Chapter 18 Solutions
EBK CHEMISTRY
- Can the molecule on the right-hand side of this organic reaction be made in good yield from no more than two reactants, in one step, by moderately heating the reactants? ?A Δ O • If your answer is yes, then draw the reactant or reactants in the drawing area below. You can draw the reactants in any arrangement you like. • If your answer is no, check the box under the drawing area instead. Explanation Check Click and drag to start drawing a structure. 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibilit ku F11arrow_forward१ eq ine teaching and × + rn/takeAssignment/takeCovalentActivity.do?locator-assignment-take [Review Topics] [References] Write an acceptable IUPAC name for the compound below. (Only systematic names, not common names are accepted by this question.) Keep the information page open for feedback reference. The IUPAC name is In progress mit Answer Retry Entire Group 5 more group attempts remaining Cengage Learning | Cengage Technical Support Save and Exitarrow_forwardDraw the molecules.arrow_forward
- Draw the mechanism for the acid-catalyzed dehydration of 2-methyl-hexan-2-ol with arrows please.arrow_forward. Draw the products for addition reactions (label as major or minor) of the reaction between 2-methyl-2-butene and with following reactants : Steps to follow : A. These are addition reactions you need to break a double bond and make two products if possible. B. As of Markovnikov rule the hydrogen should go to that double bond carbon which has more hydrogen to make stable products or major product. Here is the link for additional help : https://study.com/academy/answer/predict-the-major-and-minor-products-of-2-methyl- 2-butene-with-hbr-as-an-electrophilic-addition-reaction-include-the-intermediate- reactions.html H₂C CH3 H H3C CH3 2-methyl-2-butene CH3 Same structure CH3 IENCESarrow_forwardDraw everything on a piece of paper including every single step and each name provided using carbons less than 3 please.arrow_forward
- Topics] [References] Write an acceptable IUPAC name for the compound below. (Only systematic names, not common names are accepted by this question.) Keep the information page open for feedback reference. H The IUPAC name isarrow_forward[Review Topics] [References] Write an acceptable IUPAC name for the compound below. (Only systematic names, not common names are accepted by this question.) Keep the information page open for feedback reference. The IUPAC name is Submit Answer Retry Entire Group 9 more group attempts remainingarrow_forwardPlease draw.arrow_forward
- A chromatogram with ideal Gaussian bands has tR = 9.0 minutes and w1/2 = 2.0 minutes. Find the number of theoretical plates that are present, and calculate the height of each theoretical plate if the column is 10 centimeters long.arrow_forwardAn open tubular column has an inner diameter of 207 micrometers, and the thickness of the stationary phase on the inner wall is 0.50 micrometers. Unretained solute passes through in 63 seconds and a particular solute emerges at 433 seconds. Find the distribution constant for this solute and find the fraction of time spent in the stationary phase.arrow_forwardConsider a chromatography column in which Vs= Vm/5. Find the retention factor if Kd= 3 and Kd= 30.arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning




