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?

Expert Solution

queen_honey_blossom answered 2 years ago

_ 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?

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.

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...

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?

In the reaction: Fe^3+ + SCN^− ⇌ [Fe(NCS)]2+ The initial concentration of Fe^3+ was 0.109 and...

In the reaction: Fe^3+ + SCN^− ⇌ [Fe(NCS)]2+ The initial concentration of Fe^3+ was 0.109 and the initial concentration of SCN^− was 0.105. After equilibrium was established, the concentration of the complex was 0.09. What is the equilibrium constant?

consider the following reaction 2 Na+ 2 HCl= 2 NaCl + H2

If acidic H2O2 is mixed with Fe^2+, which reaction occurs: the oxidation of Fe^2+ to Fe^3+...

If acidic H2O2 is mixed with Fe^2+, which reaction occurs: the oxidation of Fe^2+ to Fe^3+ or the reduction of Fe^2+ to Fe? Give the balanced redox reaction for each possibility and explain your reason for selecting the reaction which will occur. Assume standard solution concentrations. For a) I have: red: H2O2 + 2H+ + 2e- ---> 2 H2O E=+1.78 V oxi Fe2+ ----> Fe3+ + e- E=-0.77V Ecell = 1.01V I'm stuck on b) but for the explanation I...

Using the initial concentrations of [Fe(H2O)6]^3+, SCN^-, and the equilibrium concentration of the [Fe(H2O)5SCN]^2+ complex, calculate...

Using the initial concentrations of [Fe(H2O)6]^3+, SCN^-, and the equilibrium concentration of the [Fe(H2O)5SCN]^2+ complex, calculate the equilibrium concentrations of both [Fe(H2O)6]^3+ and SCN^-. All mol/L. Ice table is needed. Initial concentrations of [Fe(H2O)6^3+: Initial concentrations of SCN: [Fe(H2O)5SCN]^2+ equilibrium: Fe(H2O)6 - SCN - EQ Fe(H2O)5SCN 0.390 1.54 23.42 0.390 3.12 35.99 0.390 4.84 58.09 0.390 6.25 74.81 0.390 7.96 98.97

The percent yield for the following reaction is 95.4% 2 Al + 6 HCl ----> 3...

The percent yield for the following reaction is 95.4% 2 Al + 6 HCl ----> 3 H2 + 2 AlCl3 What volume of 12.6 M HCl is needed to actually produce 30.0 g of H2? Assume Al is in excess.

Create/draw a clear and organized FLOWCHART for K+, Fe+2 or Fe+3, Ni+2, Cr+3, NO3- and PO4-3....

Create/draw a clear and organized FLOWCHART for K+, Fe+2 or Fe+3, Ni+2, Cr+3, NO3- and PO4-3. Discuss observations for any precipitate/color changes, what you would see if it was or wasn't there, etc.

Question