Redox Reactions refer to a set of chemical reactions which consist of an electron transfer and a change in oxidation state of the reactant species.
An Electrochemical Cell is an experimental system capable of either generative electrical energy from two half cells, or facilitating the chemical reaction between two half cells through the introduction of electrical energy.
The Electrochemical Potential is a measurement of the energy stored in the chemical potential of redox reactions.
A Battery in electrochemistry refers to an electrochemical cell with the capability of producing and storing electrical energy.
Corrosion, in electrochemistry, is the gradual destruction of an electrode caused by an electrochemical process.
Electrophoresis refers to the movement of dispersed charged particles under the influence of an applied uniform electric field.
(a) The following complexes I, II, and III represent model compounds for the molybdenum-containing enzymes involved in oxygen-atom transfer (OAT) reactions. In each case assign the formal oxidation state of the metal centre and clearly show your reasoning: **Please see the attached document for the diagrams.** (b) So
a) Comment on the applicability of [Fe2(S)2(SPh)4]^n shown below as a model for redox/spin states of [2Fe*2S] ferredoxin, given that the observed values of the effective magnetic moments are 0 and 1.75 for [Fe2(S)2(SPh)4]^-2 and [Fe2(S)2(SPh)4]^-3respectively b) Explaining your reasons, use the ^57Fe Mossbauer data below to
With how many grams of each reactant (glucose and vanadium pentoxide) did you start and with how many grams of each product were produced for the oxidation of glucose (C6H12O6) by vanadium pentoxide in an acidic solution. The products are CO2, V3+, and H2O. You place stoichiometric amounts of the reactants into an evacuated 2.0
Calculate the minimum energy required to produce molecular hydrogen from gas-phase water. Then compare this to the energy need to produce water electrochemically or photoelectrochemically. Finally, compare this to the energy needed to make this on a zirconia surface. Comment on why there are differences.
The active ingredient in many commercial liquid bleaches is sodium hypochlorite. The bottle lists the percentage of sodium hypochlorite as 6.0%. If the density of commercial bleach is 1.084 g/mL, how many mL of 0.150 M sodium thiosulfate is required to reach the end point in a titration similar to the one performed in this exper
Use the following pair of half-reactions to design a galvanic cell. Then write in the proper coefficient for each of the species involved in the overall reaction. Water molecules and protons are not shown in the half-reactions, but they may be needed to the overall reaction. N2(g)->N2H5+(aq) E=-.023V MnO4-(aq) -> Mn2+ (
1. Calculate the concentration of a Pb(NO3)2 in a solution made up of 49.1 mg of solid Pb(NO3)2 (MW=33.22) dissolved in 65.00 mL of water (MW=18.02). 2. Write balanced molecular, ionic, and net equations for the following reactions. a. KCN(aq) + MgCI2(aq) - KCL (aq) +Mg(CN)2(aq) b. Zn(NO3)2 (aq) +H3PO4(aq)
Want to verify answers for exam review. Question 1 Consider an electrochemical cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge: an Al(s) electrode in 1.0 M Al(NO3)3 solution a Pb(s) electrode in 1.0 M Pb(NO3)2 solution What is the balanced overall (net) cell rea
Last minute cram for finals tonight. I found these as pertains to my weak areas, so, just to see if I am doing ok, if I am wrong, please correct me-I can probably find where I went wrong! 1. What mass of solid CaO is needed to remove the sulfur dioxide from 1.0 x 106 m3 of air having an SO2 concentration of 1.5 x 10-9 M? Assu
1. Nickel commonly exists in the +2 and +3 oxidation states. If you are given a 1.47g sample of a mixture of the Ni(II) and Ni(III) salts; determine the % by weight of Ni(II) in the mixture if it required 20.31 mL of .050M KMnO4 to titrate to the end point. The unbalanced reaction is: Ni2+ + MnO4 Ni3+ + Mn2+ (acidi
Would it be a good idea for a person to take a couple of aspirin tablets before attending a cocktail party? Explain your reasoning. Response needs to be given in a 200-300 words essay. Include a reference as part of the response.
IX) Given the following information, which of the statements is true? Cu2+(aq) + e- → Cu+(aq) Eº = 0.34V 2 H+(aq) + 2 e- → H2(g) Eº = 0.0V Fe2+(aq) + 2 e- → Fe(s) Eº = - 0.44V Ni(s) → Ni2+(aq) + 2 e- Eº = 0.25V a) Cu+2(aq) is the strongest oxidizing agent b) Cu+2(aq) is the weakest oxi
Please see the attached file for further details. 9.23 Specify which compound in the following pairs of ionic compounds has the higher lattice energy: (a) KCI or MgO, (b) LiF or LiBr, (c) or NaCl. Explain your choice. See attachment. 9.24 Compare the stability (in the solid state) of the following pairs of compounds:
The cell shown above is a concentration cell. Both cells contain copper solutions and have copper electrodes. The only driving force for this cell is the difference in the concentration of the copper solutions. The system will react to equalize the concentration of the ions in both cells. Calculate ξ, the electromotive forc
Please see the attached file for complete questions. Question 1: Using and , calculate and for the following reaction: If this is a spontaneous reaction, will it be spontaneous at all temperatures? Question 2: Give the following battery: and and calculate . If you wanted to reduce your of your battery by
(there are six procedures with the same questions for each procedure) Procedure 1 LAB: Beaker #1: 150 ml CuSO4 Beaker #2: 150 ml SnCl2 Salt Bridge connects the two beakers electrode in CuSO4 is set to copper electrode in SnCl2 is set to tin volt meter reads .4761 Question: 1. Identify the cathode and anode in
1.) Compare two chemical reactions, one requiring simultaneous collision of three molecules and the other requiring a collision between two molecules. Assuming all else is equal, which reaction should be faster? Explain your answer. Can you provide an example? 2.) Why do foods cook faster in a pressure cooker relative to an o
1) Balance the following equation and determine the sum of the coefficients of the products. ___NO2- + ___MnO4- + ___ H2O à ___ NO3- + ___ MnO2 + ___ OH- A. 3 B. 4 C. 5 D. 6 E. 7 2) Balance the following redox equation and determine the sum of the coefficients of the reactants and products. ___ Br2 + ___
Aluminum is one of the most widely used metals. Aluminum is made by electrolysing aluminum oxide in a solvent called cryolite. Research the electolysis of aluminum and answer the followig questions: a) Identify the products of the anode and cathode half-reactions that occur during the electolysis of aluminum oxide. b) Why is i
1. One of the steps in the commercial process of converting ammonia to nitric acid is the conversion of NH3 into NO: 4NH3(g) + 5O2(g) ---> 4NO(g) + 6H2O(g) In a certain experiment, 2.25 g of NH3 reacts with 3.75 g of O2. a) Which is the limiting reactant? b) How many grams of NO form? c) How many grams of the excess react
1. Draw me a beaker for each of the following 3 solutions. Show (label) the particles that exist when 1 particle of each dissolves. You don't have to show the water molecules! H3P04 C12H22011 HCHOO 2. Balance the following redox reaction that occurs in basic solution. NO2- (aq) + Al (s) ---> NH3 (g) + Al02- (aq) 3. Descr
1. What is the standard electrode potential for the half reaction in which free ferric ion is reduced to elemental Iron? 2. Place the following chemical species in ascending order (in energetic terms) as electron acceptors under standard conditions. Fe3+ (reduced to Fe2+); Zn2+ (reduced to Zn); H+;Ag+;Cu2+ (reduced to Cu+)
Explain how the information from the IR spectrum will be used to solve this puzzle. There are 2 puzzles; answer that question for each of them. See attached file for full problem description.
Hi. Can someone please explain to me how to do the following question? I'm quite confused about how to do these. See attachment for better notation representation. Consider the following reaction at 25 degrees C, [Al3+] = 2.0 M and [Zn2+] = 1.0M 2 Al (s) + 3 Zn2+ (aq) -> 3 Zn (s) + 2 Al3+ (aq) a) Predict if the cell po
The following data were obtained for the reduction of metal ions A+ to metal A in a stirred solution at a 0.1 cm^2 electrode; the solution contained 0.01M A+. n(mV) -100 -120,-150, -180, -220, -280, -370, -500, -600 i(uA) -45.9, -62.6, -100, -170, -300, -510, -770, -965, -965 Calculate the exchange current density jo[uA/
1. Why did Mendeleev leave three blank spaces in his periodic table? 2. Why do elements in a group of the periodic table have similar properties? 3. List five different metals give examples of how each metal is used. 4. List five different nonmetals. Give examples of how each nonmetal is used. 5. Why would you expect to find
Both normal oxidation states of iron, Fe, will form low spin complex ions with cyanide (CN-); i.e., [Fe(CN)6]4 minus (aq) and [Fe(CN)6] 3 minus(aq). However the color of these ions is not the same. One ion is green-yellow (more yellow than green), which means it absorbs violet to blue light and the other is blood red in color,
Limonene, C10H16, a terpene found in citrus peel, absorbs only two moles of hydrogen forming p-menthane C10H20. Oxidation by permanganate converts limonene into structure A in the attached .jpg (ignore structures B and C for this problem). 1. How many rings, if any, are in limonene? 2. What structures are consistent wit
Write a balanced equation for the conversion of C6H5CHOHCH3 to methyl ketone in the presence of I2 and NaOH.
The haloform reaction using I2 and NaOH is referred to as the "iodoform" test for methylketones. The test also gives positive results for compounds containing the -CH(OH)CH3 group. This results from the oxidation of the alcohol to the methyl ketone in the first stage. Write a balanced equation for the conversion of C6H5CHOHCH3 t
Carbon Disulfide, CS2, is an important industrial substance. Its fumes can burn explosively in air to form sulfer dioxide and carbon dioxide. CF2(g) + O2(g) (arrow) SO2(g) + CO2(g) If 1.60 mol of CS2 burns with 5.60 mol of O2, how many mols of the excess reactant will still be present when the reaction is over.? Also .