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For Cyclic Voltammetry this data is given from 13 ul aliquot of a 0.1 mM concentration. From this determine its concentration.
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- Iron can be extracted from the iron(III) oxide found in iron ores (such as haematite) via an oxidation-reduction reaction with carbon. The thermochemical equation for this process is: 2 Fe2O3(s) + 3 C(s) → 4 Fe(l) + 3 CO2(9) ΔΗ = +467.9 kJDetermine the %w/w of Na2CO3 in a 2.7518 g sample that was titrated by 41.92 mL of 0.6108 M HCl. Na2CO3 mw = 105.99 g/mol A mineral was collected and weighed to be 15.001 g. The CrO4 content was determined by using 35.77 mL of a 0.9887 M HCl solution. Determine the %w/w of Cr2O3 content of the sample.Cr2O3 = 151.99 g/mol2 Na2CrO4 + 2 HCl→Na2Cr2O7 + 2 NaCl + H2O2+ Calculade the cnknown [Cu^I when Evell = 0. O50 V
- Which of the following is the strongest oxidizing agent. (E ° Fe^+3/Fe^+2 = 0.77, l^2(s) / I^-1 =0.54,Cu^+2 / Cu=0.34, Ag+ /Ag = 0.8 volts. a.Fe^+3 b. l^2 c. Ag^+ d. Cu^+2What is AG° in kJ for the following reaction at 298K? O2(g) + 4H*(aq) +4FE2+(aq) → 4Fe3+(aq) + 2H2O(1) E°cell = 0.04 V AG° = –NFE°, cell =-RT In(K) F = 96,485 C / mol e R = 8.314 J/mol K Answer with 3 significant figures and do NOT include units.Fine particles of metallic iron can be injected underground to remediate pollution of underground aquifers by the industrial solvent trichloroethane. In one experiment, 2400L of an aqueous emulsion containing ~480 kg of Fe(0) consumed 17.0 kg of trichloroethane in 5 months. Write a balanced reaction using H2O and H+ to complete the balancing. What percentage of injected iron was used by this reaction in 5 months? Fe + C2HCl3 ---> Fe2+ + C2H4 + Cl-
- Q1) a) What is i) a standard solution? ii)a reduction-oxidation (redox) reaction? b) A standard solution of hydrated Iron (II) sulphate, FeSO..xH20, as prepared by dissolving 5.8g of the salt in a volumetric flask making it to 250ml (250 cm), 25ml (25 cm') of this solution was acidified and found to react with 22.8ml (22.8 cm) of 0.018MPotassium permanganate solution. The half equation for the reaction are: Mn2+ 4H,O Feog) Fe2 (aq) + e ) What is the indicator for the titration of Iron(Il)sulphate and Potassium permanganate solution? i)indicate the colour at the end point if the permanganate is in the burette. )Why is it necessary to acidify the Iron(I)sulphate before titration ?Given: Zn 2+ (aq) + 2e Zn(s); E° = -0.76 V Cu²+ (aq) + 2e Cu(s); E° = 0.34 V Cr₂O7²- (aq) + 14H*(aq) + 6e2Cr³+ (aq) + 7H₂O(l); E° = 1.33 V Which of the following species is the strongest oxidizing agent?Write a balanced chemical reaction showing how the 2.96 g Cu dissolves in HNO3. Express your answer as a chemical equation. Identify all of the phases in your answer. Determine if HNO3 can dissolve each of the following metal samples. 3Cu (s) + 2NO3 (aq) + 8H+ (aq) →3Cu2+ (aq) + 2NO (g) + 4H20 (1) Submit Previous Answers Correct Part E Determine the minimum volume of 5.7 M HNO3 required to completely dissolve the sample. Express your answer using two significant figures. ? V = 5.4 mL Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part F Write a balanced chemical reaction showing how the 4.62 g Sn dissolves in HNO3. Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣφ ? OA chemical reaction does not occur for this question. Submit Request Answer Part G Determine the minimum volume of 5.7 M HNO3 required to completely dissolve the sample. Express your answer using two significant figures. ?
- R = 8.314 mol·K F = 96,485 mol AG° + RT · In(Q) AE° () · In(Q) AG ΔΕ %3D Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e → 2 H20 (I0) 1.229 Z2 (s) + 2 e - → 2Z (aq) 0.426 (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M2+ (aq) + 2 e Н2 (в) + 2 ОН" (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 M MZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 10 Oxidation will occur at the while reduction will occur at the Possible answers are "anode" and "cathode".= oft C W Write balanced half-reactions for the following redox reaction: Erosoft Microsoft 5.52.210.. O ELECTROCHEMISTRY Writing the half-reactions of a complex redox reaction in acidic ... esc 2+ Zn (aq)+Bi (aq)+6OH(aq) ► Zn(s)+BiO3(aq)+ 3 H₂O(1) reduction: oxidation: 0 Explanation < 3+ Check 0217 Q 103 SEV ♫ MacBook Pro ©20R = 8.314 mol·K F = 96,485 mot AG = AG° + RT · In(Q) ΔΕΔΕ-).In(O) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (1) 1.229 2 z" (aq) Z2 (s) + 2 e 3+ (aq) + 3 е 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e H2 (g) + 2 OH (aq) - 0.828 G (s) - 1.245 > M2+ (aq) + 2 e - 1.893 → M (s) A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate AG° in kJ/mol for this galvanic cell. Report your answer with 4 significant figures. You do not need to report units with your answer. If your value is negative, make sure to include a "-" symbol.
