reaction C: 2,Fe+ 6HC,HO2 2 Fe (C2H3O2)3 +3H2 (c) Reaction (c) can be classified as an...
Fe(C2H3O2)2 + H2O2 --> Fe(C2H3O2)3 Why does this oxidation result in a color change? How would the reaction change if you added 2 g of steel wool to the acetate and reduced the iron acetate solution down to 50 mL (evaporated off 100mL)?
1. Balance each of the following chemical equations: (6) (a)_2_C.H.0 + 10-2_CO2+_3_120 (b)_!_BBro+_2_HNO3– | 2_B(NO3)3 + _2_HBr (c)_2_Fe + _3_HC.H30 12_Fe(C.H30.)3 + 1 _H2 2. Consider the equations you just balanced in Question #1. (a) What TYPE of reaction is (a)? combustion (b) What TYPE of reaction is (b)? Single replacement (1) (c) Reaction (c) can be classified as an Oxidation-Reduction (Redox) reaction. Explain completely: what is being reduced and how) and what is being oxidized (and how) (3)
2. Fill in the table concerning the following redox reaction: N2 + 3H2 → 2NH3 What is the oxidation state of nitrogen in NZ ? What is the oxidation state of hydrogen in H2 ? What is the oxidation state of nitrogen in NH3? What is the oxidation state of hydrogen in NH3? What is being oxidized? What is being reduced? How do you know? What is the oxidizing agent? Reducing agent?
2 Fe + N2 + 4 H2O 2 Fe(OH)2 + N2H4 For the above redox reaction, assign oxidation numbers and use them to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent:
4. (6 pts.) Oxidation-Reduction Reactions: write out two ways you can identify the species that has been oxidized in a redox reaction: b. Identify the element reduced and the element oxidized in the following oxidation- reduction reactions. Fe(s) + CuCl2(aq) FeCl2(aq) + Cu(s) Element Oxidized: Element Reduced: C(s) + O2(g) → C02(g) Element Oxidized: Element Reduced:
hi, i understand how to solve this problem but how do we get 5 electrons in the reduction part. All the oxidation number make sense. I'm confused on where the 5 electrons came from. o0 EXPLANATION As always, when you need to analyze a redox reaction, it's a good idea to start by identifying what's reduced and what's oxidized: +7-2 +1 2+ 2+ MnO (aq) 8H (aq) + 5 Fe (aq) Mn (aq) 4H,O)5 Fe(ag) Assigning oxidation states tells you...
2. This chemical reaction is an oxidation reduction reaction. a. What is being oxidized in this reaction? b. What is being reduced in this reaction? c. What is the oxidizing agent?
Consider the following unbalanced equation. H1+(aq) + Fe(s) → H2(g) + Fe2+ (aq) (a) What are the following standard voltages? Includeţthe sign. Change the sign as allowed by the data in the table. standard oxidation potential for the oxidation half-cell .00 X V reduction potential for the reduction half-cell .44 X V potential for the entire cell (b) Select all that apply for the reaction under standard conditions. Hl+ is the substance being oxidized. Fe is the substance being oxidized....
For the following redox reaction, Fe3O4(s) + H2(g) + 3 Fe(s) + 4H2O(1) match the chemical species on the right that fits the description on the left. The species oxidized in the reaction. [Choose ] The species reduced in the reaction. [Choose ] The oxidizing agent. [Choose ] The reducing agent. [Choose ] Identify the oxidation state of each element in ammonium chlorate, NH4C104. N (Choose ) H [Choose ] СІ [Choose) о [Choose ]
LOCUOLO 3. Examine Eq. 3, above. Is this a redox reaction? If so, which element is being oxidized? Which element is being reduced? Explain your answer(s) by using the appropriate oxidation numbers. 21(aq) + 2NO3(aq) + 4H+ (aq) l(aq) + 2NO(aq) + 2H0()