Which of the following equations represents an oxidation- reduction reaction? A B с D Ca(OH)₂ (s) + H₂SO4 (aq) → 2 H₂O(l) + CaSO4(s CaO (s) + H₂O(1) → Ca(OH)₂ (s) Zn(s) + Cu(NO3)₂(aq) → Zn(NO3)2 (aq) + Cu(s) AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

What is the correct net ionic equation for the following double displacement reaction? Mg(NO3)2 (ag) +2 KF (ag) MgF (s) + 2 KNO, (ag) → a. Mg+2 (ag) + F (ag) M9F2 (s) b. Mg*2 (aq) +2 NO, (ag) + F (aq) → MgF, (s) +2 NO, (aq) c. Mg*2 (ag) + 2F (ag) - MgF2 (s) d. Mg*2 (ag) + (aq) - MgF, (s) c. K* (ag) + NO, (ag) KNO, (aq)

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 2 Ag NO, (aq) + Cu Cl, (aq) → 2 Ag CI (s) + Cu (N 0,), (aq) reducing agent: ? oxidizing O agent: redox reaction? O yes O no 2N, (2) + 50, &) – 2N,0, 4) reducing n agent: oxidizing agent: redox reaction? O yes no Fe (s) + Cu S O, (aq) → FeSo, (aq) + Cu (s) reducing agent: oxidizing agent:

To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.3600M silver nitrate AgNO3 solution to a 24.00g sample of the fluid and collects the solid silver chloride AgCl product. When no more  AgCl is produced, he filters, washes and weighs it, and finds that 1.28g has been produced. The balanced chemical equation for the reaction is: Cl−(aq) + AgNO3(aq) -> AgCl(s) + NO−3(aq) What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Cl in the sample. Be sure your answer has the correct number of significant digits.

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

Complete and balance the following redox equations using the smallest whole-number coefficients. The reaction takes place in a BASIC solution. Fe(OH)2 (s) + MnO4−(aq)  →  MnO2 (s) + Fe(OH)2 (s)     In the balanced equation, 3 OH- are present on the product side.     In the balanced equation, 5 molecules of water are present on the reagent side.     In the balanced equation, 4 molecules of water are present on the product side.     In the balanced equation, 5 molecules of water are present on the product side.     In the balanced equation, 3 OH- are present on the reagent side.     In the balanced equation, 4 molecules of water are present on the reagent side.

When the following oxidation–reduction reaction in acidic solution is balanced, what is the lowest whole-number coefficient for Na +(aq) ion? Na(s) + Ca2+(aq) → Na+(aq) + Ca(s)

What type of reaction is the following reaction: M(s) + 2 LX(aq) → 2 L(s) + M(aq) O Combustion ● Redox Precipitation Surprised Acid-Base

Balance the following reaction in basic solution. Fill in the coefficients for the balanced overall equation. H₂O + Al(s) + CrO2 (aq) → Al(OH)3(s) + Cr(OH)2 (aq) - -- Al + -- V Cro₂² → -- V Al(OH)3 + Cr(OH)4 + OH

The following chemical reaction takes place in aqueous solution: AGNO3(aq)+KBr(aq) →AGB1(s)+KNO3(aq) Write the net ionic equation for this reaction.