rite a balanced equation for the reaction m and zinc metal to yield zinc(I) and chromium(III) in acidic olution. [SHOW ALL STEPS] 7n2+ (ag) + Cr3+(aq)
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![Question 11
Write a balanced equation for the reaction between the dichromate
ion and zinc metal to yield zinc(I) and chromium(III) in acidic
solution. [SHOW ALL STEPS]
Zn(s) + Cr20,2 (aq) --> Zn²+ (aq) + Cr3+(aq)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F490c259b-4d83-40a4-832c-fbb4e5c86208%2F83d260f8-6018-4087-8067-370dfacc59a4%2Fy2u13h8_processed.jpeg&w=3840&q=75)
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- The iodine produced when excess of KI was added to the solution containing 0.1259 g K2Cr2O7 required a 41.26 mL titration with Na2S2O3 required a 41.26 mL titration with Na2S2O3. P.S. Be able to answer numbers 3 and 4 ONLY. 1. Determine if it is basic or acidic and write the balance redox reaction for the reaction of dichromate ion with iodide ion in acidic medium. Unbalance equation: Cr2O72- (aq) + I- (aq) → Cr3+ + I2 (aq) 2. Determine if it is basic or acidic and write the balance redox reaction of iodine with sodium thiosulfate in acidic medium. Unbalance equation: S2O3 2- (aq) + I2 (aq) → S4O6 2- (aq) + I- (aq) 3. (i) What are the oxidizing agents in #1 and #2? (ii) What is the stoichiometric ratio between dichromate and thiosulfate? 4. Calculate the molar concentration of the thiosulfate solution.Given the trend for metal activity below: Al > Cr > Ni > H2 > Pt Which of the following is FALSE? Select one: a. Cr metal will react when placed in an Al3+ solution. b. Pt metal will be produced when Ni metal was placed in Pt+ solution. c. No reaction will be observed when H2 gas was bubbled into a Ni2+ solution. d. Bubbling will be observed when Al metal was placed in H+ solution.Iron corrodes to produce rust, Fe2O3, but other corrosionproducts that can form are Fe(O)(OH), iron oxyhydroxide,and magnetite, Fe3O4. (a) What is the oxidation numberof Fe in iron oxyhydroxide, assuming oxygen’s oxidationnumber is -2? (b) The oxidation number for Fe in magnetitewas controversial for a long time. If we assume thatoxygen’s oxidation number is - 2, and Fe has a uniqueoxidation number, what is the oxidation number for Fein magnetite? (c) It turns out that there are two differentkinds of Fe in magnetite that have different oxidationnumbers. Suggest what these oxidation numbers are andwhat their relative stoichiometry must be, assuming oxygen’soxidation number is -2.
- Does the cell voltage increase or decrease when 5 mL of 6 MNH3was added to the half-cell containing dilute Cu(NO3)2solution? Explain why. (Note: Cu2+forms complex ion Cu(NH3)42+)Chemistry Each of the following reducing agents react with VO2+: Zn, Sn, S2O32- , Fe2+. Using the oxidation potentials below and the reduction potentials for vanadium listed on the first page of this experiment, predict the final oxidation state of VO2 + when it is mixed with each reducing agent. Reduction Agent Half-Reaction Potential Zn Zn ----> Zn2+ + 2 e- + 0.76 V Sn Sn ---> Sn2+ + 2 e- + 0.14 V S2O32- S2O32- + 3 H2O ---> 2 H2SO3 + 2 H+ + 4 e- -0.40 V Fe2+ Fe2+ ---> Fe3+ + e- -0.77 V Reduction potentials for vanadium: VO2+ + 2H+ + e- ---> VO2+ + H2O E° = 0.99 V VO2+ + 2H+ + e- ---> V3+ + H2O E° = 0.34 V V3+ + e- ---> V2+ E° = -0.26 VA current of 15.0 A is passed through a solution of CrCl2 for 45 min.(a) How many grams Cr is deposited on the cathode?(b) Calculate the volume of Cl2(g) that is obtained at the anode at 1.00 atm and 273 K. CATEGORY: Chemistry
- The cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?Calculate [Ag+] in a zinc/silver cell (reaction below) when the concentration of Zn ion is [Zn2+] = 0.020 M and Ecell = 1.593 VA 0.25 M sodium chloride solution was prepared from analytical grade NaCl. Brian immersed a silver (Ag) electrode into the solution prepared. Solve the following problems. a) Calculate the concentration of silver in this solution. Given Ksp of AgCl is 1.82 x 10-10. b) Calculate the electrode potential of silver electrode using reduction potential below. Ag+ + e- ↔ Ag(s) E° = 0.799 V AgCl(s) ↔ Ag(s) + Cl¯ E° = 0.222 V
- Does the cell voltage increase or decrease when 5 mL of 6 MNH3 was added to the half-cell containing dilute Cu(NO3)2 solution? Explain why. (Note: Cu2+forms complex ion Cu(NH3)42+)2 attempts left Be sure to answer all parts. To improve conductivity in the electroplating of automobile bumpers, a thin coating of copper separates the steel from a heavy coating of chromium. (a) What mass of Cu is deposited on an automobile trim piece if plating continues for 1.25 h at a current of 7.6 A? (b) If the area of the trim piece is 50.0 cm2, what is the thickness of the Cu coating?(d of Cu = 8.95 g/cm3)Write a balanced half-reaction for the oxidation of chromium ion Cr+3 to dichromate ion Cr2O7-2 in basic aqueous solution. Be sure to add physical state symbols where appropriate.