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) + C1O3(aq) + S(s) + Cl(aq) +

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) ◊

For the following reaction, determine the number of electrons transferred. If the reaction is not a redox reaction, please enter "0" for your answer. 3CuS(x) + SHNO, (aq) -CuSO (aq) +8NO(g) + 4H₂O(/) electrons

Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. The following molecular equation represents the reaction that occurs when aqueous solutions of silver(1) nitrate and sodium iodide are combined. AgNO3(aq) + Nal (aq) →→→Agl (s) + NaNO3(aq) Write the balanced net ionic equation for the reaction. + + + +

Balance the following reaction. If a reactant or product is not present, put a zero (0) in the blank. H+(aq) + H2O(l) + ClO-13(aq) + e-1 <--> Cl-1(g) + H+(aq) + H2O(l)

Determine net ionic equations, if any, occuring when aqueous solutions of the following reactants are mixed. Nickel(II) chloride and lead(II) nitrate; Pb2+(aq) + 2Cl-(aq) -> PbCl2(s) Ammonium sulfate and barium nitrate; Ba2+(aq) + SO42-(aq) -> BaSO4(s) Copper(II) sulfate and ammonium carbonate; No reaction occurs. Sodium bromide and hydrochloric acid; Na+(aq) + Cl-(aq) -> NaCl(s) Calcium acetate and sodium carbonate; Ca2+(aq) + CO32-(aq)  CaCO3(s)

Use the References to access important values if needed for this question. Write the net ionic equation for the following molecular equation. ZnCl2 (aq) +NazCO3(aq)→ ZnCO3(s) + 2NaCl(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.) + tps://als-asp.cengage.info/als-asp/take a e Type here to search

Write the net ionic equation for the following molecular equation.   (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)

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