under standard conditions. Al (s) + Fe3+ (aq)  →  Fe (s)  + Al3+ (aq)     spontaneous     nonspontaneous

Q: QUESTION 28 For the following reaction, all of the reactants and products are in their standard…

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Q: Consider the following redox reaction: Cu(s) + 2 Ag* 2 Ag(s) + Cu2+ What is true about AG if…

A: Since the relationship is given by  ΔG = ΔG0 + RTln(K) where R = gas constant  T = temperature in K…

Q: Calculate the standard reaction free energy (AGO) for the following unbalanced redox reaction in…

A: Here we are required to find the not only the cell potential of the given electrochemical reaction…

Q: Use standard reduction potentials to find the equilibrium constant for the following reaction at 25…

A: The equilibrium constant K is defined as the ratio of the concentrations of the products to the…

Q: How many hours would it take to electroplate 16.0 grams of magnesium if a constant current of 8.2…

A: For the first question, we have to find the time in hours that are required to electroplate 16.0…

Q: Consider three hypothetical metals: "X", "Y" and "Z". The following reactions proceed spontaneously…

A: We know that, a substance which has large reduction potential value, reduced more easily. Z + X2+ =…

Q: Determine the temperature of a reaction if K = 1.2 x 10 when AG° = +16.2 kJ/mol. %3D

A: The Gibbs free energy and the equilibrium constant are related by the following equation: ∆Go = -RT…

Q: Complete and balance the following redox reaction in acidic solution. Be sure to include the proper…

A: It is based on the concept of Redox reaction Here we are required to balance the redox reaction…

Q: Calculate the value of ΔG° for the reaction.

A: By using relationship between E° and ∆G° we can calculate ∆G° for the reaction. ∆G° = -nFE°  Where n…

Q: - Calculate the Ecell and K value for the redox reaction given below. 2A13*(aq) + 3Be(s) → 2Al(s) +…

A: E°cell = E°red (cathode) - E°red (anode)andEred (cathode)>  Ered (anode)were,E°cell = standard…

Q: Consider the following reaction at 298K. Hg2+ (aq) + Co(s)→→→ Hg(t) + Co²+ (aq) The standard Gibbs…

A: Given-> ∆G° = -219.06 KJ = -219.06 × 1000 J = -219060 J

Q: Spontaneous reactions must occur under standard state conditions , yes or no

A: A reaction is categorized into two parts: spontaneous and non-spontaneous reactions. A spontaneous…

Q: [COC14]¯ (alc) + 6H,O(alc) [Co(H,O),J?+ (alc) + 4C1¯(alc) deep blue rose pink

A: Exothermic: Heat is evolved. This is when product is more stable than the reactant   Endothermic:…

Q: Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and…

A: Answer -

Q: The standard EMF for the cell using the overall cell reaction below is +0.57 V: 2AI (s) + 312 (s)…

A: Answer:Relation between standard Gibbs free energy change and standard cell potential will be used…

Q: A solution is prepared by dissolving 22.7 g of Al2(S04)3 in water. What current would be needed to…

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Q: According to the data below, which species will reduce Zn2+ but not Mg2+? Half-Reaction Zn2*(aq) + 2…

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Q: Balance the following chemical equation:   _ Cr2O3(s) + _ Si(l) \rightarrow→ _ Cr(l) + _ SiO2(s)…

A: Balancing of a chemical reaction

Q: The following reaction occurs in a new battery called the super iron battery. In this reaction,…

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Q: For the half-reaction Cl2(g) + 2 e------>2 Cl-(aq), what are the standard conditions for the…

A: The given reaction is, Cl2(g) + 2 e------>2 Cl-(aq)

Q: Week 7 Assignment: Electrochemistry Electrolysis of Aqueous Salts Refer to this table of standard…

A: Answer: Electrolytic cell is a type of cell that converts electrical energy into chemical energy via…

Q: each reaction, write the chemical formulae of the oxidized reactants in the space provided. Write…

A: Oxidation is defined as increase in oxidation state of the element.It can also be defined as…

Q: Liquid mercury is mixed with a paste of acidic manganese IV oxide. determine the redox reaction and…

A: The objective of this question is to determine the redox reaction of liquid mercury and Manganese…

Q: The free energy change for the following reaction at 25 °C, when [Pb2+] = 1.17 M and [Ni2+] =…

A: The energy which are used in reaction  to  do work is known as Gibbs free energy.

Q: Which one of the following reactions will occur spontaneously? Group of answer choices Zn+2 (aq) +…

A: Given  Zn+2 (aq) + 2Ag(s) → Zn(s) + 2Ag+ Fe2+(aq) + Ni(s) → Fe(s) + Ni2+(aq) Br2(l) + Sn(s) →…

Q: Calculate ΔG˚, in kJ, for the following reaction at 25˚C. 3 Cu(s)  2 NO3-(aq) + 8 H+(aq) → 3…

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Q: 15. Using the standard reduction potential chart in your textbook, find Ecell for the following…

A: Given Zn(s)  + CuCl2(aq)   →  ZnCl2(aq)  +  Cu(s) Oxidation state of element in reactant and…

Q: Eºcell = ___ V for the galvanic cell shown below under standard conditions.   Report your answer…

A: Given- Cell notation and value of E0 -                           Al(s) | Al3+(aq) || Cu2+(aq) |…

Q: What is the amperage of a current if it takes 6.00 hours of the current passing through a 2.0 M…

A: The solution of the given question is

Q: Balance the equation and calculate the E∘cell of the given reaction Rb(s) + Hg2+(aq) ------> Rb+…

A: Given- Rb(s)+Hg+2(aq) ->Rb+(aq)+Hg(s) Answer may differ slightly because values of standard…

Q: 15. What is the shorthand notation that represents the following galvanic cell reaction? 2 Fe2+(aq)…

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Q: Calculate the standard free-energy change at 25 ∘C for the following reaction:…

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Q: A cell is described as stated below. Cu(s) | FeCl3(aq) | Cu(s) Match the entities present in…

A: Electrochemistry

Q: Consider the following half reaction: Na*(aq) + e¯ → Na(s). For this reaction, E°(red) = -2.7 V. If…

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Q: For each of the following reactions: 1) identify the oxidation and reduction half-equations, and 2)…

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

Q: Use half-reaction potentials to predict whether the following reaction are spontaneous or…

A: Given: T=298.15K2H2​S(g)​+O2(g)​→2H2​O(l)​+2S(s)​Step 1: Write the half-reaction. Include the H2O,…

Science behind corrosion-test

Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.

Corrosion

Corrosion is defined as an activity that transforms refined metals into more chemically stable forms such as oxide, hydroxide, carbonate, or sulfide. It refers to the slow decomposition of things (typically metals); thanks to chemical and/or electrochemical reactions with their surroundings. Corrosion engineering is the science of preventing and controlling corrosion.