Calculate the volume of hydrogen produced at r.t.p. when a concentrated aqueous solution of sulfuric acid is electrolysed for 15.0 min using a current of 1.40A. (F=96500 Cmol-"; 1 mole of gas occupies 24.0 dm3 at r.t.p.)

Calculate the volume of hydrogen produced at r.t.p. when a concentrated aqueous solution of sulfuric acid is electrolysed for 15.0 min using a current of 1.40A. (F=96500 Cmol-"; 1 mole of gas occupies 24.0 dm3 at r.t.p.)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: How long would it take to titrate 1.00 mmol H2S with a current of 100.0 mA?

Q: The electrolysis cell shown here was run at a constant current of 0.021 96 A. On one side, 49.22 mL…

A: (a) The volume of H2 gas produced at STP is calculated using the combined gas law as shown below,…

Q: The cell potential of this electrochemical cell depends on the gold concentration in the cathode…

Q: (a) Following reactions occur at cathode during the electrolysis of aqueous silver chloride…

A: The feasibility of a reaction is determined by its Gibb’s free energy value’s sign. If it is…

Q: Write the Nernst equations for the variation of half-cell potentials with activities of species in…

Q: Calculate the equilibrium constant for the following reaction carried out in 1 M perchloric acid:…

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: Dear student, according to Bartleby guidelines, we can only solve the first question if multiple…

Q: A galvanic cell Cr(s)|Cr2+(aq) || Sn2+(aq)|Sn(s) is constructed using a completely immersed Cr…

A: Cr(s) is undergoing oxidation to Cr2+(aq) and Sn2+(aq) undergoing reduction to Sn(s) half-reactions…

Q: What volumes of H₂ (9) and O₂ (g) at STP are produced from the electrolysis of water by a current of…

Q: Copperplating is a technique in which copper metal is deposited electrolytically on a surface to…

A: The objective of this question is to calculate the time required to plate 1.50 g of copper metal…

Q: l'or the cell shown, the measured cell potential, Eell, is -0.3657 V at 25 °C. Pt(s) | H, (g, 0.717…

Q: at a temperature of 25 ° C the galvanic element Pt | ClO3- 0,001M, Cl- 0,01M pH = 3 || Mn2 + 0.0001M…

Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E°…

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

A: We have to calculate the time taken.

Q: Write the Nernst equations for the variation of half-cell potentials with activities of species in…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Q: The measured cell potential, Ecell, for the cell shown is –0.3549 V at 25 °C. Calculate the H*…

A: If standard reduction potential values of two half cells are given then the half cell with less…

Q: 11. What is the standard cell potential (E°cen) for a galvanic cell constructed from these two…

A: The cell reaction taking place is given as, => 2 Cr (s) + 3 Cu2+ (aq) ------> 2 Cr3+ (aq) + 3…

Q: With the values of ΔrG Cd2+(aq) = -77.2 kj mol-1, pH2=1 atm, assemble a galvanic cell and calculate…

A: We know ∆G0 = -nFEcell 0

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

Q: Calculate the amounts of Cu and Br: produced at the inert elecuvues by passing a current of 4.5 A…

A: Given: Current = 4.5 A The atomic weight of Cu =63.55 gThe atomic weight of Br2=159.8 gCharge of 1…

Q: A galvanic cell was prepared by immersing an anode and a cathode of the same material (of A type) in…

Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E…

Q: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

Q: Calculate the maximum work available from 20.0 g of aluminum in the following cell when the cell…

A: Electric work is product of charge passed through electric cell and cell potential. So, electrical…

Q: Calculate the voltage, Ere for the reaction at 25°C Ag (s) | AglO; (s) | Ag* (x M), HIO; (0.300 M)…

A: To calculate the concentration of IO3-

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

Q: Give the standard line notation for each cell.

A: In an electrochemical cell, the electrical energy is produced from the spontaneous cell reaction at…

Q: The cell potential of this electrochemical cell depends on the pH of the solution in the anode…

Q: The formation of Br2 from Br- was done by electrolyzing 1.0 M KBr solution between two Pt…

Q: Give the standard line notation for each cell. (a) 2 103 (аq) + 10 Cr** (ag) + 10 H* (аq) — 10 Cr*…

A: Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Q: Pt(s) Br (aq) (x M) | Br21) || BrO3¯(aq) (0.43 M), H*(aq) (1.00 M) | Br2(1) | Pt(s)

Q: 28 Calculate standard electrode potential and Gibbs free energy of the cell: Ga | Ga³+ || Ag* | Ag

A: For the given cell with the anode on the left and the cathode on the right, we can calculate the…

Q: seconds

Q: For the cell schematic below, identify values for n and Q, and calculate the cell potential, EAT Al…

A: The oxidation half-reaction in the given cell involves the oxidation of Al to Al³⁺ by the removal of…

Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E"…

Q: How many liters of O2 at 298 K and 1.00 bar are produced in 2.75 hr in an electrolytic cell…

A: given: Pressure (P) = 1.00 bar temperature (T) = 298 K Time (t) = 2.75 hour x 3600 = 9900 sec…

Q: The value of pOH of HCI solution at 25 °C if cell potential of the cell is 1.6655 v Pt/ H2(g. 1.0…

A: The electrode where reduction process takes place is called cathode and where oxidation takes place…

Q: For the cell shown, the measured cell potential, Ecet, is -0.3715 V at 25 °C. P(s) | H,(g.0.857 atm)…

A: Given- Ecell =-0.3715V PH2=0.857atm Concentration of Cd2+=1.00M

Q: Molten CaCl, can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: Given-> Current (I) = 2.99 ampere Weight of Ca= 23.5 gm

Q: Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box…

A: Interpretation - The half reactions at anode and cathode and expected decomposition potential are to…

Q: What is the full name and abbreviation for the group attached to the benzene ring below? 00 volle…

A: We have to give the full name and abbreviated name of the group attached to benzene ring.

Q: In a galvanic cell, the cathode consists of a Ag*(1.00 M)|Ag half-cell. The anode is a platinum…

A: Introduction: Galvanic cell is an electrochemical cell in which currents are generated though…

Q: Determine the Cell potential (volts, V) of a spontaneous galvanic cell rxn under the conditions; 2…

Q: Given the following standard electrode potentals: Ag°(aq) + e¯ = Ag(s) N,(g) + 5H°(aq) + 4e° =…

A: Consider the given values as; Ag+ aq + e- ⇌ Ag s…

Q: An aqueous sodium chloride solution is electrolyzed using a current of 4.42 A. How much time (min)…

A: An aqueous sodium chloride solution is electrolyzed using a current of 4.42 A. How much time (min)…

Q: A galvanic cell was prepared by immersing A type) in a solution containing a low solub concentration…

Q: Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

Q: (a) Predict the products of electrolysis in each of the following:(i) An aqueous solution of AgNO3…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

ll中国移动 4G
11:40 PM
© 1 26% O
electrochemistry homework
2. 简答题
Calculate the volume of hydrogen produced at r.t.p.
when a concentrated aqueous solution of sulfuric acid
is electrolysed for 15.0min using a current of 1.40A.
(F= 96500 Cmol-1; 1 mole of gas occupies 24.0 dm³
at r.t.p.)
输入答案
2/2
答题卡
提交
<上一题
(+

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

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

Calculate the potential of the cell when; [I- ] = 0.75 M, pH = 8.90, T = 300 K, P(H2 ) = 60 torr. Of course (R = 8.314 J/mol.K) and (F = 96500 J/V.mol). If E∘cell = -1.36v
21) Given that the standard reduction potential for O₂(g) + 4H (aq) + 4e → 2 H₂O(1) is +1.229 V, the value of Ecell for O₂(g) + 2 H₂(g) → 2 H₂O(1) at pH 3.00 and all gases at standard pressure (1 bar) is: A) 0.00 V B) +1.229 V C) +1.407 V D) +0.929 V E) +1.051 V
The half-cell potential for the reactionO2 (g)+ 4H+ (aq) 4e → 2H2O (l)is 1.03V at 310K when activities of O2 and H2O are equal 1. What is the pH of this solution?
The measured cell potential, Ecel, for the cell shown is -0.3573 V at 25 °C. Calculate the H* concentration. PI(s) | H, (g,0.855 bar) |H* (aq. ? M) || Cd²*(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell and their respective standard reduction potential values, E", are given. 2H"(aq) + 2e H,(g) Cd (aq) + 2e Cd(s) E = 0.00 V E = -0,403 V 2.45 x10-6 [H*) = Incorect
(a) Determine the mass of Na,S2O3.5H20 required to prepare 0.1N solution in 50 ml volume. (b) Compare combustion of Anthracene and Xylene in sufficient supply of air. Which one will produce more carbon rich sooty flame and why? (c) Consider electrode potential data given in Question 4 (c). Predict which two electrodes combination will give maximum potential. Provide justification. (d) Explain two industrial applications of acidic buffer solutions. (e) Discuss the importance of Hess law with suitable example.
When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of Oz is 2.21 atm, [K2Cr2O7) = 0.642 M, the [Cr3+] = 0.963 M, and the pH was measured to be 8.42 then what is the cell potential at 25°C? O2(g) + Cr3+ *(aq) → H202(aq) + Cr20-2" (aq)
Write the Nernst equations for the variation of half-cell potentials with activities of species in the following half-cells: (a) Cr₂O,2-, Cr³+ | Pt; (b) saturated calomel electrode; (c) quinone, hydroquinone | Pt; (d) H* | CH4, CO₂, Pt.
How many seconds does it takes to produce 5,0 L of aluminum sulfide, Cr2S3 measured at 0.95 atm and 23 °C by electrolysis of molten chromic sulfide, using a current of 1.5 A.
For the cell below, the standard potential is Eocell = 1.62 V ( F =96500 C/mole e-)( 1VC=1J) Mg(s) | Mg2+ (1M) || Zn 2+ (1M) | Zn (s)Calculate ΔGo for the cell at standard conditions in kJ. Select one: a. -1.62 kJ b. -313 kJ c. -3.13 x 105 kJ d. -156 kJ
Molten ScCl3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be performed at a current of 2.96 A in order to produce 17.8 g Sc? S
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half- cell: Pt(s) | H2 (g, 1.0 bar) | H+(aq, 1.0 mol L-1) | Au3+(aq, ? mol L-1) | Au(s) What is the concentration of Au3+ in the solution if is Ecell is 1.24 ? Express your answer using two significant figures and don't include the exponent (e.g. if your answer is 2.5×10-4, only write 2.5)
An aqueous LaI3 solution is electrolyzed under 1 bar pressure using platinum electrodes.(a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C I2(s) + 2 e- 2 I-(aq) 0.535 O2(g) + 4 H3O+(aq) + 4 e- 6 H2O(l) 1.229 2 H2O(l) + 2 e- H2(g) + 2 OH-(aq) -0.828 La3+(aq) + 3 e- La(s) -2.370 Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential? _______V