What happens to the carbon marked with an arrow in the reaction shown below? :0 2 (1) (1) : OH Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Its oxidation state increases (becomes less negative) and is oxidized during the reaction b Its oxidation state decreases (becomes more negative) and is reduced during the reaction Its oxidation state increases (becomes less negative) and is reduced during the reaction d Its oxidation state decreases (becomes more negative) and is oxidized during the reaction

What happens to the carbon marked with an arrow in the reaction shown below? :0 2 (1) (1) : OH Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Its oxidation state increases (becomes less negative) and is oxidized during the reaction b Its oxidation state decreases (becomes more negative) and is reduced during the reaction Its oxidation state increases (becomes less negative) and is reduced during the reaction d Its oxidation state decreases (becomes more negative) and is oxidized during the reaction

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter3: Equation, The Mole, And Chemical Formulas

Section: Chapter Questions

Problem 3.49QE: One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack...

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One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack emissions is by reaction with ammonia gas, NH3. The products of the reaction, N2 and H2O, are not toxic. Write the balanced equation for this reaction. Assign an oxidation number to each element in the reactants and products, and indicate which element is oxidized and which is reduced.
Identifying oxidizing and reducing agents Decide of the ro ng agent and the formula of the oxidizing agent. er each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction redox reaction? O yes O no 2N, (e) + 50,(e) → 2N,0,6) reducing agent: oxidizing agent: redox reaction? O yes O no Fe(s) + CuSo, (aq) FeSo, (aq) + Cu (s) reducing agent: oxidizing agent: redox reaction? O yes O no co,(e) + 2H,0(1) - H,o (ag) + HCo (ag) reducing agent: oxidizing agent: Explanation Check O 2020 McGraw-Hill Education. All Rignts Resanved ms of t O Type here to search hp
Complete and balance the following redox reaction in acidic solution TeO2(aq) + NO(g) → Te(s) + NO₂ (aq) 4- 3 2 ப + 2+ 3+ 4+ 1 2 3 4 5 6 7 8 6 0 ப 1 ☐ 2 ப ப 3 ☐ 4 ☐ 5 ☐ 6 07 ☐ 8 9 + (s) (1) (g) (aq) H+ N Te e O H₂O+ H OH H₂O
Adding an oxidation state to each element in each reaction and use the change in oxidation state to determine which element is being oxidized and which is being reduced. a) CH4(g) + 2H2S(g) = CS2(g) + 4 H2(g) b) 2 H2S(g) = 2 H2(g) + S2(g) c) C6H12O6(s) + 6 O2(g) = 6 CO2(g) + 6 H2O(g)
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(1)+3 H,(9) 4 HF (9)+SiO,(s) → SiF,(0)-2 H,O(g) COo)+H,O(9) - CO,6)+H,(9) Na, CO,(s)-H,PO(30) - Na, HPO,(a4)÷CO,0)-H,OM Submit Assig Continue 2021 McGraw-H Education. All Rights Reserved Terms of Use Prviy 99 Type here to search
Determine the oxidation state of the element "X" in the compounds below and identify if the change represents oxidation or reduction. Xo,²-→ X,0;²- Your answer should follow the format: a) oxidation state of X in reactant compound b) oxidation state of X in the product compound c) does the change represent oxidation or reduction?
When the following skeletal equation is balanced under basic conditions, what are the coefficients of the species shown? 3 Si+2 HXe04 →2 Xe + 3 SiO32- Water appears in the balanced equation as a reactant (reactant, product, neither) with a coefficient of o (Enter 0 for neither.) Which species is the oxidizing agent? HXеO4
Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent. redox reaction? yes no () 70, (g) + 2CH,CH,( - 4co, (g) + 6H,0(g) reducing agent: oxidizing agent: redox reaction? yes no co,(g) + 2H,0(1) → H,0°(aq) + HCO, (aq) reducing agent: oxidizing agent: redox reaction? yes no Fe(s) + CuSo,(aq) Feso, (aq) + Cu (s) reducing agent: oxidizing agent:
Decide whether each chemical reaction in the table below is a redox reaction. If it is a redox reaction, wrote dish the formula of the reducing agent and the formula of the oxidizing agent.
Consider the following redox reaction: Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g) Which of the following statements are true? (Check all correct answers.) Group of answer choices The oxidation state of each Cl atom in FeCl2 is -2 Chlorine (Cl) is being reduced Fe(s) is being oxidized The oxidation state of iron in FeCl2 is +2 Hydrogen is being reduced The oxidation state of hydrogen in H2(g) is +1
For each reaction in the table below, write the chemical formulae of any reactants that will be oxidized in the second column of the table. Write the chemical formulae of any reactants that will be reduced in the third column. reactants oxidized reactants reduced reaction s, (6) + 8Fe(s) 8FES (s) 4Cu(s) + 0, (3) → 2Cu, O (s) 3C1, (3) + 2A1 (s) → 2AICI, (s)
7A-5. For each of these single displacement reactions:(1) Write a balanced molecular equation, including all physical states. Use the solubility rulesprovided on the Course Resources page.(2) Write a balanced total ionic equation, including all physical states and charges forindividual ions.(3) Write a balanced net ionic equation, including all physical states and charges forindividual ions.(4) State what is oxidized and briefly explain how you can tell.(5) State what is reduced and briefly explain how you can tell.a. barium and manganese(II) acetate