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17 Nov 2019

Write balanced net ionic equations for each oberserved reaction along with the relative half reactions: oxidation and reduction. (All with phase labels)

1. Cu(s)+AgNO3(aq)

2.Zn(s)+AgNO3(aq)

3.Zn(s)+HCl(aq)

4.Fe(s)+Cu(NO3)2(aq)

5.Fe(s)+HCl(aq)

6.Mg(s)+Cu(NO3)2(s)

7.Mg(s)+Zn(NO3)2(aq)

8.Mg(s)+AgNO3(aq)

9.Mg(s)+HCl(aq)

*Below i completed 1. And 2.**

P Reaction 1 Relevant Half-Reactions: oxidation: Cu us) Reduction: 2 Ag (aa) Net Ionic Equation cu s) 2Agua Reaction 2 Relevant Half-Reactions: Ag(aq) Reduction: znts) y Zn" 2C Net Ionic Equation: 2 Agua? Zn (s) Zi lagos Reaction 3 Relevant Half-Reactions: oxidation: Reduction: Net Ionic Equation: Zn(s) tt (a qb) Reaction 4 Relevant Half Reactions: Oxidation Reduction: Net Ionic Equation: Fc (3 Cu (a -a Reaction 5 Relevant Half. Reactions: oxidation: Reduction: Net Ionic Equation: 11-5 Laboratory 11 The Activity Series: On Chemistry of Metals 121 the

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A. Write a net ionic equation for all chemical reactions below.(Hint: it is possible for the net ionic equation to be the same asthe molecular equation. A complex ion that is in solution ismolecular in nature because units are coordinate covalently bondedtogether.)

1. Cu (s) + 4HNO3 (aq) --> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O(l)

2. Cu(NO3)2 (aq) + 2NaOH (aq) --> Cu(OH)2 (s) + 2NaNo3(aq)

3. Cu(OH)2 (s) --> CuO (s) + H2O (l)

4. CuO (s) + H2SO4 (aq) --> CuSO4 (aq) + H2O (l)

5. CuSO4 (aq) + Zn (s) --> Cu (s) + ZnSO4 (aq)

6. Zn (s) + H2SO4 (aq) --> ZnSO4 (aq) + H2 (g)

7. Zn (s) + 2HCl (aq) --> ZnCl2 (aq) + H2 (g)

B. Balance the following equations. Write each in both themolecular and net ionic form. Idenfity each reaction as anacid-base reaction, a precipitation reaction, anoxidation-reduction reaction, or as a combination of more than oneof these types.

1. ___Pb(NO3)2 (aq) + ____ NaCl (aq) --> _____PbCl2 (s) +_____NaNO3 (aq)

a) Molecular Equation:

b) Net Ionic Equation:

c) Reaction Type:

2. ___HNO3 (aq) + _____Zn(OH)2 (s) --> ____Zn(NO3)2 (aq) +____H2O (l)

a) Molecular Equation:

b) Net Ionic Equation:

c) Reaction Type:

THANK YOU!

blushswan904

1. Cu (s) + 4HNO3 (aq) --> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O(l)

2. Cu(NO3)2 (aq) + 2NaOH (aq) --> Cu(OH)2 (s) + 2NaNo3(aq)

3. Cu(OH)2 (s) --> CuO (s) + H2O (l)

4. CuO (s) + H2SO4 (aq) --> CuSO4 (aq) + H2O (l)

5. CuSO4 (aq) + Zn (s) --> Cu (s) + ZnSO4 (aq)

6. Zn (s) + H2SO4 (aq) --> ZnSO4 (aq) + H2 (g)

7. Zn (s) + 2HCl (aq) --> ZnCl2 (aq) + H2 (g)

1. ___Pb(NO3)2 (aq) + ____ NaCl (aq) --> _____PbCl2 (s) +_____NaNO3 (aq)

a) Molecular Equation:

b) Net Ionic Equation:

c) Reaction Type:

2. ___HNO3 (aq) + _____Zn(OH)2 (s) --> ____Zn(NO3)2 (aq) +____H2O (l)

a) Molecular Equation:

b) Net Ionic Equation:

c) Reaction Type:

THANK YOU!

9. Based on the equations below, which metal is the most active? Pb(NO3)2 (aq) + Ni (s) â Ni(NOJ2 (aq) +pb (s) Pb(NO3)2 (aq) + Ag (s)--No reaction Cu(NO): (aq) + Ni (s) â Ni(NO3)2 (aq) + Cu (s) [a] Ni [b] Ag [c] Cu [d] Pb [e] N 10. The net ionic equation for the reaction between sulfuric acid and sodium hydroxide is [a] H+(aq) + HS04 (aq)-20H-(aq) 2 H20 (l) + S -(aq) [b] H+ (aq) + HSo; (aq) + 2 Na+(aq) + 2 OH-(aq) â 2 H20 () + 2 Na+(aq) + S [c] S04-(aq) 2 Na+(aq) â 2 Na+(aq) + Sof-(aq) [d] H+ (aq) + OH-(aq) â H2O (/) [e] 2 H + (aq) + S04-(aq)-2Na+(aq) + 2 0H-(aq) 2 H 20 () +2 Na+(aq) + S -(ag) -(aq) 11. In which reaction does the oxidation number of oxygen increase? [a] Ba(NO3)2 (aq) + K2SO4 (aq) â BaSO4(s) +2 KNO3 (aq) [b] HCl (aq)-NaOH (aq) â NaCl (aq) + H20 (!) [c] MgO (s) + H20 (l) â Mg(OH)2 (s) [d] 2 SO2 (g) + 02(g) 2 SO3 (g) [e] 2 H20 (1) â 2 H2(g) + 02(g) 12. Based on the activity series, which one of the reactions below will occur? Corrected typo [a] Zn (s) + Mn12 (aq) â Zn12 (aq) + Mn (s) [b] SnCl2 (aq) + Cu (s) â Sn (s) + CuCl2 (aq) [c] 2 AgNO3 (a)Pb (s)-2 Ag (s) + Pb(NO3)2 (aq) [d] 3 Hig (l) 2 Cr(N03)3 (aq) â 3 AgN03 (aq) + 2 Cr(s) [c] 3 FeBr2 (aq) + 2 Au (s) â 3 Fe (s) + 2 AuBr3 (aq) 13. Which of the following is an oxidation-reduction reaction? [a] Cu (s) + 2 AgNO3 (aq) â 2 Ag (s)-Cu(NOJ2 (aq) [b] HCl (aq)-NaOH (aq) â H20 (1)-NaCl (aq) [c] AgNO3 (aq) + HCl (aq) â AgCl (s) + HNO3 (aq) [d] Ba(C2H302)2 (aq)-Na,so, (aq) â BaS04 (s) t. 2 NaC2H,02 (aq) [e] H2C03 (aq) + Ca(NO3)2 (aq) â 2 HNO3 (aq)-CaCO3 (s) 14. A 0.355 M K-SO4 solution can be prepared by- [a] dissolving 46.7 g of K SO4 in water and diluting to a total volume of 250.0 mL [b] dissolving 46.7 g of K2SO, in water and diluting to 500.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL [c] dilution of 1.00 mL of 0.355 M K,SO, to 1.00 L [d] diluting 46.7 mL of 1.90 M K SO, solution to 250.0 mL

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