Name: Lab Section: 1 2 3 4 5 6 7 8 Report: Redox Reactions 1. Consider...
6. Cellular respiration depends on a series of REDOX reactions. In today's lab, and in class, we learned that we can think of oxidation and reduction in terms of electronegativity and electron density. During oxidation, the oxidized species loses electron density. During reduction, the reduced species gains electron density. a. Knowing that, label the following with oxidizing agent reducing agent, oxidized product, and reduced product. They are not balanced equations (1 point each blank; 8 points total). -C-H + O=...
Which of the following statements concerning redox reactions is incorrect? Substance oxidized loses electrons Oxidizing agent is the substance reduced Reducing agent gains electrons Reducing agent is the substance oxidized Substance reduced gains electrons
PLEASE ANSWER EACH QUESTION OR DO NOT ANSWER AT ALL. THANK YOU! 4. Consider the following unbalanced net redox equation: HCI + KMnO, (aq) + H,02 (aq) -. MnC12 (aq) + O2 (g) + KCI in an acid solution a. Determine the oxidation state of each atom or ion in the above reaction: b. Which atom is being oxidized? Which atom is being reduced? C. Which species is the reducing agent? Which is the oxidizing agent? d. Write the net...
Redox reaction 9. Diarsenic trioxide and the nitrate ion undergo a redox (reduction-oxidation) reaction, as shown by the equation below. Note: The equation below is not balanced and does not need to be balanced: As2O3 (s) + NO3- (aq) → H3AsO4 (aq) + NO (6) a. (*) Determine the oxidation state of each individual atom shown in the equation above. (8 points): b. (i) State which substance is the oxidizing agent, which substance is the reducing agent, which substance is...
Consider the following redox reaction: Indicate what element is oxidized and what element is reduced as well as the oxidizing agent and reducing agent. If an element is part of a compound, indicate the element (including its oxidation number) that is oxidized or reduced as part of the compound. For example, if C is oxidized in CO, then you would write C2+ in CO. 2 A) _______ is oxidized and _______ is reduced. B) _______ is the oxidizing agent and _______ is the...
[References] Sc(s) + 3Ag+ (aq) + 3 Ag(s) + Sc3+ (aq) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced CE SC HBr(9) + NH3(g) + NH4Br(s) Redox? Oxidizing Agent in Reducing Agent Substance Oxidized Substance Reduced GeCl4 (1) + 2H2O(l) + 4HCl(aq) + GeO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d. Si C14 (1) + 2Ba(s) + 2BaCl2(8) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes 2 SiBr, Ba SiBa Al(OH).-...
Balance the following equation: 5. pur Tsa-1 य KCI KSO, + HO Cl + KS,O, + KOH For the reaction in question 5, list those elements which have changed oxidation number during the reaction, showing the oxidation number before and after the reaction. Which element is oxidized? Which is reduced? Which is the oxidizing agent? Which is the reducing agent? How many electrons are transferred per sulfur atom? How many totally in the reaction as shown? 6. 82V Balance the...
Іго, Electrochemistry Wolleet 1. Assign oxidation numbers to each element in the following compounds: a. VOCI b. Cuso c. CHOH). d. Mno, e. SO, 2. Given the following half reactions and their standard reduction potentials, i. Cl (g) + 2e- - 2 CI (aq) E' =+ 1.36 V ii. Niº (aq) + 2e - Ni (s) E' = -0.25 V iii. Ag (aq) + e- Ag () E' = +0.80 V Identify the chemical species most likely to be oxidized....
Consider the following reactions and determine which specie will be oxidized and which one will be reduced, also, determine the reducing agent, the oxidizing agent, which specie will be found at the anode and which one will be found at the cathode. How many moles of electrons are transferred and how many Faradays of energy will be required? 1. MnO, + NO, Mn + NO, Species oxidized Reduced Reducing Found at the Oxidizing Agent Agent Found at the anode cathode...
2CrO42- + 6F-+ 8 H2O3F2 + 2Cr(OH)3+ 10 OH- In the above redox reaction, use oxidation numbers 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:_________