Which of the following is NOT a valid mass balance equation for
the titration of Fe2+ with Ce4+, as described by the reaction
below?
a) [Fe2+] = [Ce4+]
b) cFe = [Fe2+] + [Fe3+]
c) [Ce3+] = [Fe3+]
d) cCe = [Ce3+] + [Ce4+]
[Fe2+] = [Ce4+] is not a valid mass balance equation because these two are reactant , in which one is getting oxidized and the other is getting reduced. SoThey don't need to have same concentration as the concentration of both are independent of each other.
In all the other cases mass balance expression is correct.
So our answer is option - A
Which of the following is NOT a valid mass balance equation for the titration of Fe2+...
Which of the following is NOT a valid mass balance equation for the titration of Fe2+ with Ce4+, as described by the reaction below? Fe2 (aq) Ce3t (ag)Fe3+ Ce4+ '(aq) (aq) CFe [Fe2+][Fe3] CCe [Ce3 ][Ce4*] O Fe2 [Ce4+] O [Ce3] Fe3
In a potentiometric titration of iron with cerium, the reaction is Fe2+ + Ce4+ --> Ce3+ + Fe3+. After collecting data it was found that 0.8925 grams of iron could be titrated with 20.95 milliliters of 0.04945 Molarity cerium(IV) to reach an end point with a potential of 0.806 Volts. Using the Nernst equation [Ecell = {E^o (Fe) - 0.0592 log {(21.05 - Volume added)/Volume added}} - Eref], calculate values of formal electrode potentials for reduction of iron...
Can you please explain this question ? During a titration it was determined that 30.00 mL of a 0.100 M Ce4+ solution was required to react completely with 20.00 mL of a 0.150 M Fe solution. Which reaction occurred? +CeO+2H+ C. Ce4+Fe2+Fe3+ Ce3+ D. Ce4+2Fe2+2Fe3+Ce2+ E. Ce4+ + 2Fe2+ → 2Fe4+ + Cs2+ +2e
The concentration of a Fe2+ solution is determined by titrating it with a 0.1462 M solution of Ce4+. The balanced net ionic equation for the reaction is shown below. Ce4+(aq) + Fe2+(aq) Ce3+(aq) + Fe3+(aq) In one experiment, 16.48 mL of the 0.1462 M Ce4+ solution is required to react completely with 25.00 mL of the Fe2+ solution. Calculate the concentration of the Fe2+ solution.
3. For the cell represented by Pt|Fe3+(0.25 M), Fe2+(0.025 M)||Ce4+(0.035 M), Ce3+(0.050 M)|Pt E o (Fe3+/Fe2+ = +0.771V, Eo Ce4+/Ce3+ = + 1.44V a) Draw the complete cell represented by the above line diagram and label all the components. b) Write the half-cell reactions and complete redox reaction of the cell. c) Calculate the standard cell potential. d) Calculate the cell potential at the non-standard conditions provided above. e) Was the cell reaction spontaneous?
balance the following equation: Feº + HCl → Fe2+ +.... Fe2+ + H2O2 → Fe3+ + H20 +.....
3) In an acid-base reaction, what is transferred from the acid to the base? A) an oxidizing agent B) an oxygen atom C) an OH-ion D) an electron E) a hydrogen cation, H+ 4) Classify the following reaction: Ce4+ (aq) + Fe2+(aq) → Ce3+ (aq) + Fe3+ (aq) A) oxidation - reduction B) acid - base C) decomposition D) precipitation E) combustion
You are titrating 100.0 mL of 0.0400 M Fe2+ in 1 M HCIO4 with 0.100 M Ce4+ to give Fe3+ and Ce3+ using Pt and calomel electrodes to find the endpoint. (a) Write the balanced titration reaction. > (b) Complete the two half reactions for the Pt electrode. Ce té E° = 1.70 V Fe +e = E° = 0.767 V [Fe2+11 1 - 0.241 E= 0.767 – 0.05916) (c) From the list in the column at the right, select...
Balance the reaction below in acidic aqueous solution, using the oxidation number method. In the balanced equation, what is the coefficient of Fe2+? ClO3– + Fe2+ → Cl– + Fe3+ Question 4 options: A) 5 B) 6 C) 8 D) 1 E) 7
Balance the following redox reaction in acidic solution by inputting the correct coefficients. Fe2+ + O2 → Fe3+ + H2O If H+ or H2O is not present as reactant or product, select "0" as the coefficient for the purposes of this question. You must also explicitly label a coefficient as "1" if only one molecule is present. Important: You MUST simplify all "like terms" on both sides of the chemical equation before selecting your answer: having the same compound on...