please help a stressed out high schooler assignment due tomorrow Question A The following reactions are oxidation-reduction reactions. Identify the oxidative and reductive half reactions. Identify the oxidizing and reducing agents. Hg22+(aq) + Sn2+(aq) >>> 2 Hg(l) + Sn4+(aq) Which is the correct answer? Oxidizing agent - Hg22+ Reducing agent - Sn2+ Oxidizing agent - Hg22+ and Sn2+ Reducing agent - Hg22+ and Sn2+ Reducing agent - Hg22+ Oxidizing agent - Sn2+ Question b The following reactions are oxidation-reduction reactions. Identify the oxidative and reductive half reactions. Identify the oxidizing and reducing agents. Hg22+(aq) + H2S(aq) >>> Hg(l) + HgS(s) + 2 H+(aq) which is the correct answer? Oxidizing agent and reducing agent - Hg22+ Oxidizing agent and reducing agent - H2S Oxidizing agent - Hg22+ Reducing agent - H2S Oxidizing agent - H2S Reducing agent - Hg22+

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please help a stressed out high schooler assignment due tomorrow
Question A

The following reactions are oxidation-reduction reactions. Identify the oxidative and reductive half reactions. Identify the oxidizing and reducing agents.

Hg₂²⁺(aq) + Sn²⁺(aq) >>> 2 Hg(l) + Sn⁴⁺(aq)

Which is the correct answer?

Oxidizing agent - Hg₂²⁺

^{Reducing agent - Sn²⁺}

Oxidizing agent - Hg₂²⁺ and Sn²⁺

^{Reducing agent -} Hg₂²⁺ and Sn²⁺

Reducing agent - Hg₂²⁺

^{Oxidizing agent - Sn²⁺}

Question b

The following reactions are oxidation-reduction reactions. Identify the oxidative and reductive half reactions. Identify the oxidizing and reducing agents.

Hg₂²⁺(aq) + H₂S(aq) >>> Hg(l) + HgS(s) + 2 H⁺(aq)

which is the correct answer?

Oxidizing agent and reducing agent - Hg₂²⁺

Oxidizing agent and reducing agent - H₂S

Oxidizing agent - Hg₂²⁺

^{Reducing agent - H}₂S

Oxidizing agent - H₂S

Reducing agent - Hg2²⁺

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The amount of l3- in a solution can be determined by titration with a solution containing a known concentration of s2o32-(aq) (thiosulfate ion). The determination is based on the net ionic equation Given that it requires 38.2 mL of 0.450 M Na2s2o3(aq) to titrate a 25.0-ml sample of l0-(aq), calculate the molarity of l0-(aq) in the solution. The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 7.99-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCI(aq) and passed over a reducing agent so that all the antimony is in the form Sb3+(ag). The Sb3+(aq) is completely oxidized by 39.4 mL of a 0.115 M aqueous solution of KBr03(aq). The unbalanced equation for the reaction is calculate the amount of antimony in the sample and its percentage in the ore. Write a balanced overall reaction from these unbalanced half-reactions. Cu rightarrow cu2+ Ag rightarrow Ag balanced overall reaction: An experiment was performed to test the relative activities of four metals, A, B, C, and D. Each solid metal was mixed with solutions of each of the other cations as shown in this chart. The results were indicated as follows y=yes a reaction occurred N=no a reaction did not occur For example, when A+ (aq) was mixed with B (s), a reaction occurred. Use this data to rank the neutral metals according to their activity. Rank these species by their ability to act as an oxidizing agent. Best oxidizing agent Best reducing agent. Best reducing agent Mg2+ Cu2t Ct2* Ag+ For the following reaction kcio3 rightarrow kci+3/2o2 assign oxidation states to each element on each side of the equation Write the balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional. H2SO4 + 2KOH rightarrow 2H2O+K2SO4 0.950 L of 0.450 M H2SO4 is mixed with 0.900 L of 0.290 M KOH. What concentration of sulfuric acid remains after neutralization? Enter the net ionic equation, including phases, for the reaction of AgNo3(aq) with BaO(aq). Write the net ionic equation (including phases) that corresponds to Fe(No3)2(aq)+Na2S(aq) rightarrow FeS(s) + 2NaNO3 (aq) If a solution containing 126.27 g of mercury(ll) chlorate is allowed to react completely with a solution containing 17.796 g of sodium sulfide, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction? Write the balanced equation for the reaction of aqueous Pb(CI03)2 with aqueous Nal. Include phases. What mass of precipitate will form if 1.50 L of concentrated Pb(CI03)2 is mixed with 0.850 L of 0.220 M Nal? Assume the reaction goes to completion. Predict whether the following compounds are soluble or insoluble in water: CuC03 KN03 Pb(N03)2 BaS04 PbCI2 CuCI2

3. Write the product formed in the following reactions in the space provided. If the reaction does not take place write NO RXN. Indicate physical states by (s), (l), (g), (aq). Make sure the reaction is balanced! Please write the net ionic equation below.

a. Pb(CH₃CO₂)_2(aq) + Na₂SO₄_(aq) Ã

b. AgNO_3(aq) + NH₄Br_(aq) Ã

4. Balance the following reactions and answer the questions below.

a. Al_(s) + HCl _(aq) Ã AlCl₃ + H₂

What is the element that is oxidized _______________________

What is the element that is reduced _______________________

Which compound is the oxidizing agent ____________________

Which compound is the reducing agent ____________________

b. Na_(s) + FeCl₂ Ã NaCl + Fe

What is the element that is oxidized _______________________

What is the element that is reduced _______________________

Which compound is the oxidizing agent ____________________

Which compound is the reducing agent ____________________

8. Using the unbalanced equation how many grams of lithium nitrate will be needed to make 250g of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction.

Pb(SO₄)_2(aq) + LiNO_3(aq) Ã Pb(NO₃)_4(s) + Li₂SO_4(aq)

9. Using the following equation determine how many grams of sodium fluoride can react with 184.4 grams of magnesium.

Mg + NaF₂ Ã MgF₂ + Na

10. Determine how many Oxygen atoms are present in 46.7g of Zr(SO₄)₂

10. Given the following unbalanced equation:

Al₂O_3(aq) + Fe_(s) Ã Fe₂O_3(aq) + Al_(s)

Determine how many grams of Iron (III) Oxide can be formed if 224 grams of aluminum oxide is reacted with iron.

Multiple choice:

10b. Which of the following statement is true about 1 mole of Ca(NO₃)₂?

a. It contains the 6.02 x 10²³ NO₃^- ions.

b. It weighs 146 grams

c. It will most likely dissolve in a bucket of water.

d. It will produce equal number of Ca⁺² and NO₃^- ion in a solution.

10. How many molecules are present in 48.0 grams of oxygen gas? (O₂)

a. 6.02 x10²³ b. 1.81 x10²⁴ c. 9.03 x10²³ d. 1.03x10²⁴

12. If there are 12 moles of carbon in 1 mole of sucrose, C₁₂H₂₂O_11.How many atoms of carbon are there in 1 mole of sucrose?

a. 1 x6.03 x 10²³ b. 12x 6.03 x 10²³ c. 22 x 6.03 x 10²³

13. Determine the oxidation state of oxygen in the compound Cr₂O₃ in the following equation:

Cr₂O_3(s) + 2Al_(s) Ã Cr_(s) + Al₂O_3(s)

-2 b. -6 c. 6 d. 2

16. Determine the oxidation state of Al in the following equation:

Al_(s) + HCl Ã AlCl_3(aq) + H₂

+2 b. 0 c. +3 d. -5

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		Oxidizing agent - Hg₂²⁺ ^{Reducing agent - Sn²⁺}
		Oxidizing agent - Hg₂²⁺ and Sn²⁺
		^{Reducing agent -} Hg₂²⁺ and Sn²⁺
		Reducing agent - Hg₂²⁺ ^{Oxidizing agent - Sn²⁺}

		Oxidizing agent and reducing agent - Hg₂²⁺
		Oxidizing agent and reducing agent - H₂S
		Oxidizing agent - Hg₂²⁺ ^{Reducing agent - H}₂S
		Oxidizing agent - H₂S Reducing agent - Hg2²⁺