Be sure to answer all parts. Balance the following skeleton reaction and identify the oxidizing and reducing agents: Include the states of all reactants and products in your balanced equation. You do not need to include the states with the identities of the oxidizing and reducing agents. Zn(s) + NO3 (aq) → Zn(OH),² (aq) + NH3(g) [basic] The oxidizing agent is The reducing agent is

Be sure to answer all parts. Balance the following skeleton reaction and identify the oxidizing and reducing agents: Include the states of all reactants and products in your balanced equation. You do not need to include the states with the identities of the oxidizing and reducing agents. Zn(s) + NO3 (aq) → Zn(OH),² (aq) + NH3(g) [basic] The oxidizing agent is The reducing agent is

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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Electrolysis is the process of using electrical current to cause a nonspontaneous reaction to occur. For example, water molecules do not readily decompose into hydrogen and oxygen. However, water can be decomposed using electrolysis according to the reaction 2 H₂O(1)→ 2H₂(g) + O₂(g) Because electrolysis involves the transfer of electrons, it is classified as a type of oxidation-reduction (redox) reaction. For the given reaction, identify which atoms are oxidized and which are reduced. Which atoms are oxidized? Both oxygen atoms in O₂(g). The oxygen atom in H₂O(1). Both hydrogen atoms in H₂(g). Both hydrogen atoms in H₂O(1). MacBook Pro Which atoms are reduced? Both hydrogen atoms in H₂(g). The oxygen atom in H₂O(1). Both hydrogen atoms in H₂O(1). Both oxygen atoms in O₂(g).
Which of the following is an oxidation-reduction reaction? OHCl(aq) + LiOH(aq) → LiCl(aq) + H₂O(1) Nal(aq) + AgNO3(aq) → Agl(s) + NaNO3(aq) Pb(C₂H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaC₂H3O₂(aq) Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g) All of these are oxidation-reduction reactions.
How do we solve this redox reaction?
1-Balance the following redox reaction occurring in an acidic solution. The coefficient of Cr2O72−(aq) is given. Enter the coefficients (integers) into the cells before each substance below the equation. 1 Cr2O72−(aq) + ___ Ti3+(aq) + ___ H+(aq) → ___ Cr3+(aq) + ___ TiO2+(aq) + ___ H2O(l) 2- The following chemical reaction occurs in a basic solution. NO3−(aq) + ClO−(aq) + H2O(l) → NO(g) + ClO2−(aq) + OH−(aq) How many moles of electrons are transferred when the equation is balanced using the smallest whole-number coefficients?
3Cr(NO₂), (aq) +2A1(s)-3Cr(s) + 2AI (NO₂), (ag) 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. 2AgNO, (ag) + CaCl, (aq) - 2 AgCI(1) + Cu(NO₂), (4) 2N, (e) + 50, (e)- 2N, 0, (e) redox reaction? O yes reducing O agent: oxidizing 0 agents redox reaction? O yes reducing 0 agent: oxidizing 0 agent redox reaction? yes reducing agent: oxidizing agent: no no O no 015 X Jalm
Specify which of the following are oxidation-reduction reactions, and if it is, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. If it is not, select No and leave the following boxes blank. Express your answers as a chemical formulas. Omit states-of-matter. Zn(s) + 2Ag* (aq) → 2 Ag(s) + Zn2+ * (aq) а. Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced No v b. HBr(g) + NH3 (g) → NH,Br(8) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes v С. GeCl4 (1) + 2H2O(1) → 4HC1(aq) + GeO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d. Si Br4 (1) + 2Ba(s) → 2BAB12 (s) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Ga(OH), (ag) - → GaO2 (ag) + 2H2O(1) е. Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Previous Next
c) Are the following Redox reactions or non-Redox reactions? If you determine that they are Redox, state which reactants have been Oxidised and which have been Reduced? Also remember to assign oxidation numbers for all atoms or ions on the reactant and product side to denote electron transfer for reactions identified as Redox. i) NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O (1) ii) Al(s) + Cu²+ (aq) → Al³+ (aq) + Cu(s) iii) Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) iv) 2Na(s) + Cl2(g) → 2NaCl(s)
Balance the following reaction in acidic solution. Cr2O, (ag) + HNO,(aq) → Cr* (aq) + NO, (aq) 3 Fill in the coefficients for the balanced overall equation. HNO, + -- v H* + -v Cr.O,* → -- ♥ NO, +- Cr3+ + Cr,O, - H.O --V
Complete and balance the following skeleton reaction and identify the oxidizing and reducing agents. Include the states of all reactants and products in your balanced equation. You do not need to include the states with the identities of the oxidizing and reducing agents. Br₂(1)→ BrO₂ (aq) + Br (ag) Part 1 of 3 The oxidizing agent is: Part 2 of 3 The reducing agent is: Part 3 of 3 X X The balanced equation is: ローロ X 00 [acidic] 000 Ar
Identifying oxidising and reducing agents.
Balance the following equation and write the sum of the coefficients of the reactants and products under acidic conditions. VO+2(aq) + Sn+2(aq) → V+3(aq) + Sn+4(aq) Group of answer choices 14 10 9 13 12 6 7 11 8
For the complete redox reactions given here, write the half-reactions and identify the oxidizing and reducing agents. Make sure your answer has the simplest coefficients. 4Fe + 3O2 → 2Fe2O3