CHE112 Problem Set 10 Solutions

2. KMNO4 + NagC204 + H2SO4 K2SO4 + MNSO4 + NagSO4 + CO2+ H20 Balanced equation: Oxidizing agent: Reducing agent: Criteria for each item Solution following the 5-step process Balanced equation Oxidizing agent Reducing agent 10 points 3 points 1 point 1 point Total points or each item: 15points

Consider the following redox reaction: Fe(s)  +  2 HCl(aq)  →  FeCl2(aq)  +  H2(g) Which of the following statements are true?  (Check all correct answers.) Group of answer choices The oxidation state of each Cl atom  in FeCl2 is -2 Chlorine (Cl) is being reduced Fe(s) is being oxidized The oxidation state of iron in FeCl2 is +2 Hydrogen is being reduced The oxidation state of hydrogen in H2(g) is +1

What is the oxidation number for each of the following elements? (e.n.'s: C = 2.5, O = 3.5, H = 2.1) 1. Co in Co (NO:)a а.

Denitrification is an important biologically-mediated process by which nitrate is reduced. This is especially important in environments with excess inputs of nutrients. Denitrification is shown in the following (unbalanced) equation: CH2O + NO3- + H+àH2O + N2 + CO2. What are the oxidation states of each element in the equation? Write the number under the element in the equation. Write the half reactions. Label which half reaction shows oxidation and reduction. Balance each half reaction. Write is the full balanced equation. Calculate the reduction potential DEo’. Calculate the Gibbs free energy DGo’. Will this reaction produce energy for bacterial growth?

4. Consider the following redox equation (balanced) 32 H+ + 4 4 Cr₂0² + 3 S²- → 8 Cr³+ + 3 SO² + 16 H₂O a. b. C. Calculate the Molarity of a solution prepared by dissolving 0.624 g of Na2S in enough water to give 250 mL of solution. How many mL of this solution will be required to react with 0.512 g of Al2(Cr2O7)3? Suppose that 24.86 mL of this Na2S solution was required to react with 0.377 g of a dichromate salt. Which one of the following could be this salt? Fe2(Cr2O7)3 CaCr2O7 PbCr2O7 BaCr2O7 Bi2(Cr2O7)3. d. How many mL of the Na2S solution would be required to react with 50.00 mL of 0.300 M K2Cr2O7 solution?

Consider the two-step process for the formation of tellurous acid described by the following equations:  ???2+ 2??−⟶ ???3 2− + ?2? ???3 2− + 2?+⟶ ?2???3 What mass of H2TeO3 is formed from 74.2 g of TeO2, assuming 100% yield?

50.00 grams of chromium (III) sulfate is dissolved in enough water to prepare 250.0 ml of solution. • What is the chemical formula for chromium (III) sulfate? • What is the molecular weight of chromium (III) sulfate grams per mole? • What is the concentration of chromium (III) sulfate in the solution above in moles per liter? • What is the concentration of Cr+3 ions in the solution above in moles per liter? Answer M • What is the concentration of SO4−2 ions in the solution above in moles per liter? • How many milliliters of the solution above are required to supply 0.100 moles of chromium (III) sulfate? • How many milliliters of the solution above are required to supply 0.275 moles of SO4−2 ions? • How many milliliters of the solution above are required to supply 0.120 moles of Cr+3 ions

When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown?Cl- + NiO2 Ni(OH)2 + Cl2 Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which element is oxidized?

Adding an oxidation state to each element in each reaction and use the change in oxidation state to determine which element is being oxidized and which is being reduced. a) CH4(g) + 2H2S(g) = CS2(g) + 4 H2(g) b) 2 H2S(g) = 2 H2(g) + S2(g) c) C6H12O6(s) + 6 O2(g) = 6 CO2(g) + 6 H2O(g)

Which element in the compounds below has an oxidation number (state) of +2? N in NH4Br Ba in Ba(OH)2 Cr in CrO3 V in VO2+

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 2Na(s) + Cl, (8) 2NACI (s) reducing agent: ? oxidizing agent: redox reaction? yes no C(s) + 0, (g) → co,(g) reducing agent: oxidizing agent: redox reaction? yes no + co, (g) + 2H,0(1) → H,0" (aq) + HCO,(aq) reducing agent: oxidizing agont:

VII. Write the balanced chemical equation for the given reactions. 1. Fe(s) + Cl: –→ FeCl:(s) 2. N:(g) + H:(g) → NH:(g) 3. CeH.COOH(ag) + O:(g) → CO:(g) + H:O(I) 4. AGNO:(ag) + Cu(s) - 5. HCN(ag) + CUSO:(ag) Cu(NO:)-(ag) + Ag(s) H.SO:(ag) + Cu(CN)(ag)

Use the rules (in order) to assign oxidation numbers to each of the elements in the compounds below.   bismuth hydroxide H Bi O Bi(OH)3         bromine trifluoride Br F   BrF3         periodic acid H I O HIO4

Identify the oxidation numbers to all the elements in each of the compound or ions H2SO3 O a. H2 =+2; S=+2; O3 =-2 O b. H2 =+1; S=+3; 03 =-2 H2 =+2; S=+4; O3 =-2 d. H2 =+1; S=+4; O3 =-2

Given the type of the reaction, complete and balance each of the following reactions: a) b) Na(s) + CuSO4(aq) → - Single replacement. K(s) + N₂(g) → - combination. Edit View Insert Format Tools Table 12pt ✓ Paragraph BIU AT²V

Combustion reactions (burning of fuels) are another example of redox.  Coal is nearly pure carbon and has been burned as a fuel for centuries.  The reaction of coal with oxygen in the air is illustrated by the balanced equation: C + O2 → CO2 What is the change in oxidation state for the carbon in this reaction? Group of answer choices +2 -4 +4

Listen What is the balanced chemical equation that represents the following reaction? 80 goo go 6H + 2N – 2HN3 -> O 2N + 2H3 - 2H3N O 6H + 2N · 2NH3 → -> 6H + 2N – 2N3H 3H2 + N2 - 2NH3 V Saved Question 40 (1 point)

Rank the following according to oxidation number on chlorine.  (#1 lowest) HOCl, Cl2, AlCl3, ClO2

G c3h6 m G no2 mo G nh3 mo O Poelt W Wordle * Ground G co3 - G b Answer G co2 mo O Caffein G molar b Answer Gk Question 11 of 28 Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow. K:SO:(aq) + FeCls(aq) → 12+ 3+ 4+ 1 3 4 6. 7 8 9. 口2 Do 14 (s) (1) (g) (aq) K CI NR Fe •x H2O Delete Reset PgUp PgDn Home F9 End F10 F1 PrtScn

What numbers belong in the blank spaces to fully balance the following reaction? _ Fe (s) + Cl2 (g) → FeCl3 (s)

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) → MgCl₂ (aq) + Ni (s) -> Element Mg Ni CI Oxidizing Agent 1 OM O NiCly Reducing Agent O ME O NiCl₂ b) C₂H (g) + 30₂ (g) 2 CO₂ (g) + 2 H₂O(g) Element Initial OS C H 0 Oxidizing Agent O Cylla O 0₂ Reducing Agent Tab Caps Shift Esc ! 1 Initial OS A @ 2 21 Q x Z F2 W S I # 3 X F3 E D L Q Search » $ 4 Final OS Final OS F4 R C DII TI F F5 % 5 T V * G F6 ^ 6 * Y B

80°F Sunny The oxidation number of an element can vary. O True Search F8 6725 F9 O False - « Οι F10

Some chemical reactants are listed in the table below. Complete the table by filling in the oxidation state of the highlighted atom. oxidation state of highlighted atom 0 0 species FeSO4(s) VO(s) Fe₂O3(s) KMnO4(s) X 0 0

ter 8: EOC t Calculate the number of grams of solute in each of the following solutions. (a) 3.63 L of a 3.23 M HCI solution (b) 36.3 mL of a 14.6 M HNO3 solution (c) 37.3 mL of a 10.4 M AgNO3 solution (d) 1.57 L of a 3.2x10-³ M Na₂SO4 solution Submit Answer Try Another Version [References grams of HCI grams of HNO3 grams of AgNO3 grams of Na2SO4 5 item attempts remaining

When the following skeletal equation is balanced under basic conditions, what are the coefficients of the species shown? NiO2 + Sno,2- → Ni(OH)2 + Sno32- (Enter 0 Water appears in the balanced equation as a for neither.) (reactant, product, neither) with a coefficient of Which species is the reducing agent?

Would you use an oxidizing agent(OA) or reducing agent(RA) in order for the following reactions to occur? NH3 ==> NO2 Choose... As ==> As+3 Choose... MnO2 ==> Mn2O3 Choose... P205 ==> P4H10 Choose...

When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown?Cl- + Br2ClO3- + Br-Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which element is reduced?  Part B: When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown? Cl- +  I2   I- +  Cl2Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which element is oxidized?

MISSED THIS? Read Section Review | Constants Periodic Part A 20.2 (Pages 898 - 901) Watch WE 20.2. Balance each of the following redox reactions occurring in acidic solution. Cr30; (aq) + Cu* (aq)Cr" (aq) + Cu (aq) Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦ DA chemical reaction does not occur for this question. Submit Reauest Answer Part B CIO, (aq) + CI (aq) CIO, (aq) + Cl, (R) Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣφ BA chemical reaction does not occur for this question.