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(9) + NH3(g) → NH4B1(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes v GeCl4 (1) + 2H2O(1) → 4HC1(aq) + GeO2(s) C. 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(ОH), (аg) GaOz (ag) + 2H,0() е. Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Previous Next

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

Balance the following redox equation, for a reaction which takes place in basic solution. HS (aq) + ClO3(aq) → S(s) + Cl(aq) (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) - HS (aq) + ClO3(aq) + S(s) Cl(aq) +

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

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

Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction.   NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g)  Balance the reaction.

Use the relative strengths of nonmetals and metals as oxidizing and reducing agents, as indicated in the following unbalanced equations, to construct a table of half‐reactions. Ag (s) + Br2 (l) → AgBr (s) Ag (s) + I2 (s) → no evidence of reaction Cu2+ (aq) + I‐ (aq) → no redox reaction Br2 (l) + Cl‐ (aq) → no evidence of reaction

Balance the following redox reaction in the gas phase. Note that this reaction cannot be balanced with the half-reaction method and must be done by inspection. In the gas phase, H2 O (1) is used to balance oxygen atoms and H3 O+ and OH are not available for balancing purposes. ONLY integers should be used in your answer. NH3 (aq) + O2 (g) –→ NO2 (g) Enter your chemical notation here

Step by step please. also have to answer A-D

Is the reaction a redox reaction; "yes" or "no".