Use the References to access important values if needed for this question. 2HNO3 + 3Ni+ 6H*→2NO + 3Ní*+ 4H,0 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: 9 more group attempts remaining Submit Answer Retry Entire Group Previous Next

Use the References to access important values if needed for this question. 2HNO3 + 3Ni+ 6H→2NO + 3Ní+ 4H,0 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: 9 more group attempts remaining Submit Answer Retry Entire Group Previous Next

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Choose all of the statements from below which are true about oxidation and reduction. Ooxidation and reduction are opposite processes with respect to bookkeeping electrons. O Oxidation is what happens when an element in a substance increases its oxidation number. Electrons appear on the right side of an oxidation half reaction. An oxidant is an oxidizing agent, which becomes reduced during the course of a redox reaction. O Reduction is what happens when an element in a substance decreases its oxidation number. Electrons appear on the left side of a reduction half reaction. A reductant is an reducing agent, which becomes oxidized during the course of a redox reaction. K
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QUESTION 5 For the reaction below, determine the stoichiometric coefficient on the hydrogen ion in the balanced redox reaction in acid solution. In compounds, the oxidation state of O is 2-. Assume X is a diatomic element and that M is a metal that can have multiple oxidation states. This question is not multiple choice, you will input the integer answer to this question. MO 3 (aq) + X 3+ (aq) → X 4+(aq) + M 3+ (aq)
An atom changes its oxidation number from -5 to -3. Was it oxidized or reduced? Did it gain or lose electrons? How many electrons did it take to do this?
For each chemical reaction listed in the table below, decide whether the highlighted atom is being oxidized or reduced. highlighted atom is being... reaction neither oxidized nor reduced oxidized reduced CH(9)+H,O(g) → CO(g)+3 H,(g) CO(g)+H,O(9) → CO,(9)+H,(9) N(9)+3 H,(9) → 2 NH3(9) 4 HF(g)+ SiO,(s) → SiF,(9)+2 H,O(9)
For the following reaction, identify the element that was oxidized, the ele- ment that was reduced, and the oxidizing agent. Give an explanation for each answer. N 2) + O2«) → N,Os«) Answer in complete sentences.
Give the oxidation number of sulfur in each of the following. S8, BaSO4, Na2S, H2SO3
2PH3 + 3N0₂2P + 3N0₂ + 3H₂0 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:
3Cl2 + 2MnO2+ 8OH-2MnO4- + 6Cl-+ 4H2O 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: