**Redox Reaction: Ethylene Combustion**In this section, we analyze the redox reaction of the combustion of ethylene (C₂H₄). The balanced chemical equation is:\[ \text{C}_2\text{H}_4(g) + 3 \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) + 2 \text{H}_2\text{O}(g) \]**Oxidation States (OS) Analysis:**| Element | Initial OS | Final OS || ------- | ---------- | -------- || C | | || H | | || O | | |**Agents Identification:**- **Oxidizing Agent:** - Selected: C₂H₄ - Options: C₂H₄, O₂- **Reducing Agent:** - Selected: O₂ - Options: C₂H₄, O₂**Explanation:**- **Oxidizing Agent:** The species that gets reduced by gaining electrons during the reaction. In this setup, oxygen (O₂) is typically the oxidizing agent. - **Reducing Agent:** The species that gets oxidized by losing electrons. Ethylene (C₂H₄) is typically the reducing agent in this reaction.**Note:** The oxidation states need to be determined to understand the transfer of electrons and complete the table. This involves assigning the appropriate values based on standard rules for calculating oxidation states. For each of the reactions below, determine the initial and final oxidation states (OS) of each of the atoms as well as the oxidizing and reducing agents.a) \( \text{Mg (s)} + \text{NiCl}_2 \text{(aq)} \rightarrow \text{MgCl}_2 \text{(aq)} + \text{Ni (s)} \)| Element | Initial OS | Final OS ||---------|------------|----------|| Mg | 0 | 0 || Ni | +2 | +2 || Cl | 0 | 0 |### Oxidizing Agent- [ ] Mg - [x] NiCl₂### Reducing Agent- [x] Mg - [ ] NiCl₂This exercise involves determining the oxidation states of the elements in a redox reaction to identify the oxidizing and reducing agents. The options for oxidizing and reducing agents are presented as radio buttons.

An oxidizing agent is a substance that can oxidize other substances but itself gets reduced.On the…

For each of the reactions below, determine the initial and final oxidation states (OS) of each of the atoms as well as the oxidizing and reducing agents. a) Mg (s) + NiCl (aq) → MgCl₂ (aq) + Ni (s) Element Initial OS Final OS Mg Ni CI Oxidizing Agent 0 Reducing Agent +2 Mg NiCl₂ O Mg NiCl₂ 0 +2 0

For each of the reactions below, determine the initial and final oxidation states (OS) of each of the atoms as well as the oxidizing and reducing agents. a) Mg (s) + NiCl (aq) → MgCl₂ (aq) + Ni (s) Element Initial OS Final OS Mg Ni CI Oxidizing Agent 0 Reducing Agent +2 Mg NiCl₂ O Mg NiCl₂ 0 +2 0

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...

See similar textbooks

Similar questions

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
Identify the oxidation number of each element in each given compound.
-N 1 Osynthesis Oprecipitation c. Classify the reaction represented by the following unbalanced equation by as many methods as possible. Choose the correct balanced equation. FeCl₂ (aq) + AgNO3(aq) → Fe(NO3)2 (aq) + AgCl(s) (Select all that apply.) oxidation-reduction decomposition [Review Topics] Osingle-displacement Odouble-displacement FeCl₂ (aq) + 2AgNO3(aq) → Fe(NO3)2 (aq) + 2AgCl(s) FeCl₂ (aq) + 2AgNO3(aq) → Fe(NO3)2 (aq) + AgCl(s) (Select all that apply.) Doxidation-reduction Odecomposition Osynthesis Oprecipitation Osingle-displacement Odouble-displacement d. Classify the reaction represented by the following unbalanced equation by as many methods as possible. Choose the correct balanced equation. Al(s) + Br₂ (1)→→ AlBr3 (8) [References] 2Al(s) + 3Br2 (1)→ 2A1Br3 (8) Al(s) + 3Br2(1)→ AlBr3 (s)
Balance the following redox reaction in BASIC conditions. Once you complete the balancing use your workings to answer four questions on this quiz. Mn2+ (aq) + BiO3 → Biš+ (aq) + MnO4 (aq) (aq) In the final balanced BASIC reaction, which statement is true? There is no water in the final balanced reaction There are 7 water molecules on the reactant side There are 7 water molecules on the product side There are 14 water molecules on the reactant side There are 14 water molecules on the reactant side and 7 water molecules on the product side
By the half-reaction method the balanced equation of the following redox reaction is Fe+3 Fe(s) + Mg (aq) +2 (aq)+ Mg(s) O a. Fe*3(aq)+ 3 e -Fe(s) O b. Fe*3(aq)+ Mg(s) - Fe(s) + Mg*2 (aq) Oc 3 Fe*3(aq)+ 2Mg(s) - 3Fe(s) + 2Mg*2 (aq) O d. 2Fe*3 (ag) + 3Mg - 2FEG) + 3Mg*2 (aq) page ourse Syllabus Jump to
Identify whether each of the following reaction is a redox reaction. If it is so, by showing the change in oxidation numbers identify the oxidizing agent and reducing agent. 4 CaSO3 ⟶ 3 CaSO4 + CaS 2 KMnO4+ 3 H2O2 → 2 MnO2 + 2 KOH + 2 H2O + 3 O2
ter 8: EOC t Calculate the number of grams of solute in each of the following solutions. (a) 3.63 L of a 3.23 M HCI solution (b) 36.3 mL of a 14.6 M HNO3 solution (c) 37.3 mL of a 10.4 M AgNO3 solution (d) 1.57 L of a 3.2x10-³ M Na₂SO4 solution Submit Answer Try Another Version [References grams of HCI grams of HNO3 grams of AgNO3 grams of Na2SO4 5 item attempts remaining
Find the oxidation numbers
Consider the redox reaction 3 Ni² (aq) + 2 Co(s) → 2 Co³(aq) + 3 Ni(s) Which substance gets oxidized? Ni²+ Ni O Co³+ What is the oxidizing agent? Ni²+ Ni Co Which substance gets reduced? Ο Ni O Co³+ Co O Ni²+ What is the reducing agent? Co³+ Ni Co Ni²+
c. For the unbalanced redox reaction Cu + 10 ➜→ Cu²+ + 1₂ Which is oxidizing agent (oxidant)? Write the balanced redox net ionic equation when the reaction is conducted in an acidic solution.
Identify the reducing agent and the following reaction
This reaction represents the titration from today's lab. 2- 2 S₂03² + 1₂ → S406² +21 O In this reaction, [Select] ✓ [Select] S406 1- 12 S203 is the oxidizing agent and is the reducing agent.