2. Consider the following three reactions: 2 Fe (s) + 6HCl (aq) → 2 FeCl3 (aq)...

2. Consider the following three reactions: 2 Fe (s) + 6HCl (aq) → 2 FeCl3 (aq) + 3 H2 (g) ΔHA Fe2O3 (s) + 6HCl (aq) → 2 FeCl3 (aq) + 3 H2O (l) ΔHB 2H2 (g) + O2 (g) → 2 H2O (l) ΔHC a. Show how these equations must be summed together according to Hess’s Law to determine ∆H for the combustion of iron (target equation shown below). Also show clearly how the ∆H values of each of the three reactions must be manipulated to determine the enthalpy of combustion of iron. 4 Fe (s) + 3 O2 (g) → 2 Fe2O3 (s) ∆H = ?

Expert Solution

queen_honey_blossom answered 2 years ago

FeCl3(aq) + 3 NaOH (aq) ---- Fe(OH)3(s) + 3 NaCl(aq) Is this a redox reaction in...

FeCl3(aq) + 3 NaOH (aq) ---- Fe(OH)3(s) + 3 NaCl(aq) Is this a redox reaction in the reaction above? Explain.

_ FeCl3 (aq) + _ NaOH (aq) --> Fe(OH)3 (_) + _ NaCl (___) Balance the...

___ FeCl3 (aq) + ___ NaOH (aq) --> Fe(OH)3 (___) + ___ NaCl (___) Balance the reaction, and enter phases for the products. You do not need to submit this for this assignment, but it will help you solve the problem. A 0.532 M NaOH solution is added to 39.4 mL of a 0.398 M FeCl3 solution. What is the volume of NaOH in mL that must be added to completely react with the FeCl3 solution?

1. Can 0.250 mol NaOH consume all of the available FeCl3 (0.308 mol)? FeCl3(aq) + 3 NaOH(aq) → Fe(OH)3(s) + 3 NaCl(aq)

1. Can 0.250 mol NaOH consume all of the available FeCl3 (0.308 mol)? FeCl3(aq) + 3 NaOH(aq) → Fe(OH)3(s) + 3 NaCl(aq)2. Now consider the reaction when 45.0 g NaOH have been added. What amount of NaOH is this, and what amount of FeCl3can be consumed by it?

Balance following simple redox reaction Ca(s) + blank Fe+3(aq) blank + ca+2(aq) + Fe

Consider the following reaction : Fe3+ (aq) + SCN- (aq) ---> Fe(SCN)2+ (aq) Starting with 4.00...

Consider the following reaction : Fe3+ (aq) + SCN- (aq) ---> Fe(SCN)2+ (aq) Starting with 4.00 mL of .200 M Fe3+ (aq) in a cuvette, 0.10 mL increments of 0.00100 M SCN- (aq) will be added. Assume that because [Fe3+ (aq)] >> [SCN- (aq)], the [Fe(SCN)2+] concentration can be calculated from the limiting reagent, SCN-. Calculate [Fe(SCN)2+]. Volume .00100 M KSCN mL [Fe(SCN)2+] (M) .10 .20 .30 .40 .50 .60 .70 .80 .90 1.00

Consider an electrochemical cell based on the following overall reaction, Fe(s) + 2Ag+(aq)  Fe2+(aq) +...

Consider an electrochemical cell based on the following overall reaction, Fe(s) + 2Ag+(aq)  Fe2+(aq) + 2Ag(s) Fe2+(aq) + 2e– Fe(s), ℰ° = –0.44 V Ag+(aq) + e– Ag, ℰ° = 0.80 V Calculate the cell potential (in V) for this reaction at 25oC when the concentration of Ag+ ions is 0.050 M and the concentration of Fe2+ ions is 1.50 M. a. +1.32 V b. +1.50 V c. +1.20 V d. -1.32 V e. -1.20 V

2 fe + 6 hcl - 2 fecl3 + 3 h2 a. how much fe is...

2 fe + 6 hcl - 2 fecl3 + 3 h2 a. how much fe is required to generate 6 moles of h2 gas if 17.0 moles of hcl is added to enough iron that the hcl is completely used up, how many hydrogen will be produced? c. how much hcl is required to completely react with 2.8 moles of iron?

Consider the following reactions. reaction MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution Balance...

Consider the following reactions. reaction MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution Balance each equation under the specified conditions

Balance the following eqautions: Fe(s) + S(s) -> FeS(s) H2SO4(aq) + NaOH(aq) -> Na2SO4(aq) + H2O(I)...

Balance the following eqautions: Fe(s) + S(s) -> FeS(s) H2SO4(aq) + NaOH(aq) -> Na2SO4(aq) + H2O(I) Cu(s) + O2(g) -> Cu2O(s) FeCl3(aq) + NaOH(aq) -> Fe(OH)3(s) + NaCl(aq)

. Which of the following are redox reactions? I: 2 HF(aq) + Ca(OH)2(aq) → CaF2(s) +...

. Which of the following are redox reactions? I: 2 HF(aq) + Ca(OH)2(aq) → CaF2(s) + 2 H2O(l) II: 2 CH3OH(g) + 3 O2(g) → 2 CO2(g) + 4 H2O(l) III: 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) (1) Only I (2) Only II (3) I and III (4) II and III (5) I, II, and III

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