Answered: An electrical current of 3.0 A is used…

An electrical current of 3.0 A is used to deposit 0.5 g of nickel to a metal object, with Ni being reduced from the +2 oxidation state. [Ni =58.69 g/mol) Ni2 (ag+2eNi)

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: In the electrolysis of a solution containing Ni2 + (aq), metallic deposits Ni(s) on the cathode.…

A: The problem is asking us to calculate the mass of nickel that will form on the cathode during…

Q: What quantity of electric current is required to deposit 0.750 g of Pt(s) from a solution containing…

A: The number of moles of a substance is defined as the mass of the substance upon molar mass.The…

Q: Balance the redox reaction in acidic solution. Y(s) + XO2 (aq) → YO(s) + XH3(aq)

A: To solve this problem first we have to determine the oxidation state of each element then we will…

Q: Cadmium sulfide (CdS) is used in some semiconductor applications. Calculate the value of the…

A: Recall the given redox reactions,CdS + 2 e- → Cd + S2- ؏° = -…

Q: Using data from the Standard Reduction Potentials table, place the following in order of increasing…

Q: How much current is required to electroplate a metal surface with 0.432 g nickel metal from a…

Q: I Reactions please balance | Fe2+ MnO4!- Mn2+ Fe3+ oxidation, { el-s}: reduction, { el·'s}:

A: since you have posted a multiple question in a single session, we are entitiled to answer first…

Q: Consider solutions of Cr(NO3)3-9H2O in water. The solubility of Cr(NO3)3-9H₂O in water at 15 °C is…

A: Given that the solubility of Cr(NO3)3.9H2O in water is 208 g per 100 g of water at 15oC. Saturated…

Q: Balance the following oxidation - reduction reaction. Identify the oxidizing and the reducing agent.…

A: Oxidation/reducing agent means adding of oxygen and reduction /oxidising agent means removal of…

Q: Balance the following redox equations by the half-reaction method: 2+ (a) Mn²+ + H₂O₂ →→ MnO₂ + H₂O…

Q: For a particular redox reaction Cr is oxidized to CrO4 and Fe is reduced to Fe Complete and balance…

Q: n the electrolysis of a solution containing Ni2+(aq) , metallic Ni(s) deposits on the cathode.…

Q: a) Which metal can be oxidized in a Sn2+ solution, but not in one of Fe2+? b) Choose the best…

A: a) Nickel, Cadmium and Cobalt b) Pb+2 c) Al

Q: Balance the following redox reaction in basic solution. SO;²- (aq) + Cr2O,7-(aq) → Cr³*(aq)+…

A: Given that : We have to balance the following redox reaction in basic solution : SO32-(aq) +…

Q: The equilibrium constant, Kc, was found to be 1.3 x 10^3 at 24.6 C for the reaction.…

A: Here we are required to find the reduction potential of half reaction of X.

Q: Based on the following reduction potential data, which is the strongest oxidizing agent? E+0.800 V…

A: Oxidising agent A compound that reduces itself and oxidises the other compound.

Q: How many grams of chromium metal can be electroplated from a mixture containing Cr+3 ions using a…

A: 46.6 gExplanation:

Q: Use the E° values to determine whether the reaction: Ni (s) + Mn2+ -> Ni2+ + Mn (s) will occur…

Q: What is the equilibrium constant for the following redox reaction? Cu2+ + 2Li Cu + 2Lit Litte Cu²+ +…

A: Given, Cu2+ + 2 Li ------> Cu + 2Li+ Standard reduction potential are given, Li+ + e- ---> Li…

Q: Consider the redox reaction: Fe(CN)- + Ag(s) + Br¯ = Fe(CN);- + AgBr(s) a) Identify the oxidizing…

A: Given redox reaction: Fe(CN)63-+Ag(s)+Br-⇌Fe(CN)64-+AgBr(s)

Q: What is the cell potential, E, given that [Mg2+] = 1.5 M and [Ni2+] = 0.2 M?

Q: [5] Balance the following redox reaction in acidic solution. CIO3 (aq) + C[(aq) → Cls (aq)

Q: APPENDICE B: Potentiels de réduction standards pour demi-réactions choisies E°red (V) 1,23…

Q: following redox reaction(in acidic solution). State oxidation and reduction half reactions.

A: The reaction, in which an atom loses an electron, is called an oxidation reaction. The reaction in…

Q: 1.A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: 2) Balance the following redox equation by the half reactions method. NO3 - (ag) + Cr3+(ag)→ NO(g) +…

A: Redox reactions are the combination of reduction and oxidation reactions. The type of reaction in…

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

Guided Problem 4
An electrical current of 3.0 A is used to deposit 0.5 g of nickel to a metal
object, with Ni being reduced from the +2 oxidation state. [NI = 58.69 g/mol]
(aq i
+2eN

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 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

Explore relative reducing/oxidizing ability. Use the half-reactions shown below to answer the following questions. Half-reaction Cl2(g) + 2e->>2Cl(aq) E° (V) 1.360V Ni2+(aq) + 2e- →Ni(s) -0.250V Mn2+(aq) + 2e- →Mn(s) -1.180V (a) Identify the strongest oxidizing agent and the weakest oxidizing agent. Enter formulas: Strongest OA Weakest OA (b) Identify the strongest reducing agent and the weakest reducing agent. Strongest RA Weakest RA
Give the equilibrium constant for the following reaction at 298 K.
A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -1.09 V (minus 1.09 V).
Balance the following redox reaction under acidic conditions. H2S() + NO3 (aq) → S8(s) + NO(2) (ba) What is the number of electrons gained in the reduction half reaction? 05 16 03 02 ace Soltic
plz explain step by step in detail
Solder is an alloy containing the metals tin and lead. A particular sample of this alloy weighing 1.50 g was dissolved in acid. All of the tin was then converted to the +2 oxidation state. Next, it was found that 0.368 g of Na2Cr2O7 was required to oxidize the Sn2+ to Sn4+ in an acidic solution. In the reaction, the chromium was reduced to Cr3+ ion.1. Write a balanced net ionic equation for the reaction between Sn2+ and Cr2O72- in an acidic solution.2. Calculate the number of grams of tin that were in the sample of solder.3. What was the percentage by mass of tin in the solder? Can you answer these questions for me and sort of explain how you got the answer. Redox reactions are giving me the blues.
Sa+4 is the strongest oxidizing of 7) Calculate the equilibrium constant for the reaction at 25°C. 3 Zn(s) + 2 Fe³(aq) = 3 Zn¹²(aq) + 2 Fe(s)
A current of 9.7 A and a voltage of 4.5V are used in the electroplating. How many grams of chromium (52 g/mol) can be plated if the current is run for 42 minutes? Cr2O72- (aq) + 14H+ (aq) + 12e- → 2Cr(s) + 7H2O