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 3 years ago

Consider these reactions where M represents a generic metal: 2M(s) + 6HCl(aq) ---->2MCl3(aq) + 3H2(g) Delta...

Consider these reactions where M represents a generic metal: 2M(s) + 6HCl(aq) ---->2MCl3(aq) + 3H2(g) Delta H1 = -569kj HCl(g) ----> HCl(aq) DeltaH2 = -74.8 H2(g) + Cl2(g) ----> 2HCl(g) Delta H3 = -1845kj MCl3(s) ----> MCl3(aq) Delta H4 = -405kj Use the above information to determine the enthalpy of the following reaction: 2M(s) + 3Cl2(g) ----> 2MCl3(s) What is Delta H for this reaction?

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?

Consider these reactions, where M represents a generic metal 1. 2M(s)+6HCl(aq)------>2MCl3(aq)+3H2(g) Delta H1=-749.0 KJ 2. HCl(g)------->HCl(aq)...

Consider these reactions, where M represents a generic metal 1. 2M(s)+6HCl(aq)------>2MCl3(aq)+3H2(g) Delta H1=-749.0 KJ 2. HCl(g)------->HCl(aq) Delta H2=-74.8 KJ 3. H2(g)+Cl2(g)------->2HCl(g) Delta H3=-1845.0 KJ 4. MCl3(s)-------->MCl3(aq) Delta H4=-298.0 KJ Use the information above to determine the enthalpy of the following reaction. 2M(s)+3Cl2(g)----->2MCl3(s) Delta H=???

identify the oxidizing agent in the reaction: Fe(s)+Cu(No3)2(aq)->Fe(NO3)2(aq)+Cu(s)

2X(s) + 6HCl (aq) ----> 2 XCl3 (aq) + 3 H2(g) a. Which reactant is oxidized...

2X(s) + 6HCl (aq) ----> 2 XCl3 (aq) + 3 H2(g) a. Which reactant is oxidized and which reactant is reduced? (Please explain) b. To prepare a HCl solution, 12.0 M concentrated HCl was diluted with water to make 250 mL of a 4.00 M HCl solution. How much, in mL, of concetrated acid was used? c. In an experiment, it was found that 25 mL of the diluted acid was required to react completely with the 4.80 g of...

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

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