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) + NiCl₂ (aq) Element Mg Ni CI - Oxidizing Agent » MgCl,(aq) → Ni(s) Initial OS I Final OS

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) + NiCl₂ (aq) Element Mg Ni CI - Oxidizing Agent » MgCl,(aq) → Ni(s) Initial OS I Final OS

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

Consider the following reaction: Zn(s) + Co(NO3)2(aq) --> Co(s) + Zn(NO3)2(aq) The Zn atom is the in this reaction. precipitant oxidizing agent O spectator ion limiting reagent reducing reagent
Assign oxidation states to all of the species in the following redox reaction. For the reactants, identify electron loss or gain, the species oxidized, the species reduced, the oxidizing agent and the reducing agent. Oxidation state Electron loss or gain Oxidized or reduced Reducing or oxidizing agent Mg(s) ♥ ◊ ŵ +2Fe³+ (aq)- → ◊ ♥ ◊ ◊ Mg2+ (aq) + 2Fe²+ (aq) ◊
In the following reaction, Rb is 2 Rb(s) + Cl2(g) 2 RbCI(s) A) the reducing agent. B) reduced. C) the oxidizing agent. D) the electron acceptor
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 chemical formulas. Omit states-of- matter. a. b. CH4 (9) + 302(g) → CO2 (g) + 2H₂O(g) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced 3AgNO3(aq) + Sc(s) → Sc(NO3)3(aq) + 3Ag(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced î
Write balanced, net ionic equations for the reactions shown. Identify the spectator ions. Please solve and explain. Thank you.
Ⓡ D Classify each reaction as a redox reaction or a non-redox reaction. > SO₂ + H₂O H₂SO4 √x #3 F3 E F4 $ 4 R S D F Redox с 2 CO +0,2 CO₂ F5 % 5 T F6 6 ✈ Answer Bank F7 HCI + NaOH →→→→ H₂O + NaCl & 7 Q F8 Y U 4 C V B N * 00 8 G H J 8 F9 1 M 09 ( 9 Zn + CuCl₂ →→→ ZnCl₂ + Cu Non-redox K F10 O 0 F11 L P + F12 11 PrtSc { Ins + 11 [ ? D
www-awn.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-lijkPWvZoZLqKt1FLlq7w SIMPLE REACTIONS Writing net ionic equations The following chemical reaction takes place in aqueous solution: MnBr, (aq)+2 NaOH(aq) → Mn(OH),(s)+2 NaBr(aq) | Write the net ionic equation for this reaction.
Chemistry Consider the following redox reactions assuming they occur in a basic solution. (a) SO, (aq) + Cu(OH), (s) →SO, (aq) + Cu(OH)(s) MnO₂ (s) (b) O₂(g) + Mn(OH)₂ (s) → (c) NO, (aq) + H₂(g) →→→ NO(g) (d) Al(s) + Cro, (aq) AK(OH), (s) + Cr(OH), (aq) Which of the following presents a wrong balanced equation? Show your work on your worksheet. 2Cu(OH), (s) +SO, (aq) →→2 Cu(OH)(s) + SO₂³(aq) + H₂O(l) 2Mn(OH)₂ (s) + O₂(g) →→→ 2MnO₂ (s) + 2H₂O(l) (b) (c) 2NO, (aq) + 2(H* +OH) + 3H₂(g) → 2NO(g) + 4H₂O(l) (d) CO₂ (aq) + Al(s) +H*(aq) + 2H₂O(1)→→ C(OH), (aq) + Al(OH),(s)
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. a. CH4 (9) + H2O(g) → CO(g) + 3H2 (g) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced b. 3 AgN O3 (ag) + Al(s) → Al(NO3), (ag) +3 Ag(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced 2Al(s) + 6 HC1(aq) → 2AIC13 (ag) + 3H2 (g) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d. 4H (aq) + TeO, (aq) → Te O4² (aq) + 2H2O(1) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced (Previous Next
7
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