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2. (3)For the following reaction: Mg(s) + Ni(NO3)2 (aq) → Mg(NO3)2(aq) + Ni(s) a. Write the...
Consider the following chemical reaction. Mg(s)+Ni(NO3)2(aq)⟶Ni(s)+Mg(NO3)2(aq) Which statement is true for the reaction? The nickel(II) ion...
Consider the following chemical reaction. Mg(s)+Ni(NO3)2(aq)⟶Ni(s)+Mg(NO3)2(aq) Which statement is true for the reaction? The nickel(II) ion is oxidized. The nitrate ion is the reducing agent. The nickel(II) ion is the oxidizing agent. Metallic magnesium is reduced.
Ni(OH)2 + NO3- _______> NiO2 + NO2- + H2O In the above redox reaction, use oxidation numbers to identify the...
Ni(OH)2 + NO3- _______> NiO2 + NO2- + H2O In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent:
Suppose the galvanic cell sketched below is powered by the following reaction: Ni(s)+Pb(NO3),(aq) → Ni(NO3)2(aq)+Pb(s) E1...
Suppose the galvanic cell sketched below is powered by the following reaction: Ni(s)+Pb(NO3),(aq) → Ni(NO3)2(aq)+Pb(s) E1 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?
1. Balance the reaction between Mg and NO3- to form Mg2+ and HNO2 in acidic solution....
1. Balance the reaction between Mg and
NO3- to form
Mg2+ and
HNO2 in acidic solution.
When you have balanced the equation using the smallest integers
possible, enter the coefficients of the species shown. Enter "1" if
the coefficient is "1."
Mg + NO3Mg2+
+ HNO2
Water appears in the balanced equation as a (reactant,
product, neither) with a coefficient of ______. (Enter 0 for
neither.)
How many electrons are transferred in this reaction? _______
.
.
2. Balance the following...
a.) Cu 2 b.) Mg +29) +2e- → Cus) + 2e- → Mg(s) (aq) c.) Mg,...
a.) Cu 2 b.) Mg +29) +2e- → Cus) + 2e- → Mg(s) (aq) c.) Mg, → Mgt? (aq) + 2e- → Cus+ 2e- d.) Cu (aq) the reduction half reaction is a.) Cut2 +2e- → Cus) b.) Mg? (aq) + 2e- → Mgie c.) Mg» → Mg(aq) + 2e- → + 2e- d.) Cu (aq) Cuis) is being oxidized a.) Cu? (aq) b.) Mg(s) c.) Mg (aq) d.) Cu(s) RING 2018 is being reduced a.) Cu 2 (aq) b.)...
2. For the oxidation-reduction reaction 3Mn(s) + 2Fe(NO3)3(aq) → 2Fe(s) + 3Mn(NO3)2 (aq) Hint: HNO3 a)...
2. For the oxidation-reduction reaction 3Mn(s) + 2Fe(NO3)3(aq) → 2Fe(s) + 3Mn(NO3)2 (aq) Hint: HNO3 a) provide equation for the oxidation half-reaction: b) provide equation for the reduction half-reaction: In the given equation above or in your answers to a) and b): c) label the substance which is oxidizing agent, d) label the substance which is reducing agent.
17) Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) +...
17) Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s) A) Ag B) Ni C) CI D) O E) This is not an oxidation-reduction reaction. 18) When an aqueous solution of manganese (II) nitrate is combined with an aqueous solution of ammonium sulfide, what should precipitate out? A) Mns B) Mn(SO3)2 C) Mn(SO4)2 D) Mn 2503 E) Mn 2504 19) If 4.89 g of ZnCl2 is dissolved in enough water to give a total...
3) Given: Sn(NO:)2 (aq) + Ni(s) > Sn (s)+ Ni(NO3)2 (aq) Write the standard electrochemical line...
3) Given: Sn(NO:)2 (aq) + Ni(s) > Sn (s)+ Ni(NO3)2 (aq) Write the standard electrochemical line notation and sketch a complete cell diagram for this electrochemical cell. Calculate the value of E cell.
When answering Parts a-h, consider only the molecules and ions, Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq), and Cr2O7^2-(aq), under standard state conditions. (1 pt each) Use standard reduction...
When answering Parts a-h, consider only the molecules and ions,
Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq),
and Cr2O7^2-(aq), under standard state conditions. (1 pt each)
Use standard reduction table.
a) Which of these molecules and ions are oxidizing agents?
b) Which of these molecules and ions are reducing agents?
c) List the oxidizing agents from part a in DECREASING order of
oxidizing agent strength. (strongest OA to weakest OA)
d) List the reducing agents from part b in DECREASING order of...
PLL35 W 13. For the following redox reaction, 2CBn 2CsBr a) write the two half reactions...
PLL35 W 13. For the following redox reaction, 2CBn 2CsBr a) write the two half reactions b) identify what is oxidized and what is reduced c) identify the oxidizing agent and the reducing reagent 20s + Br2 -> 2 Cs Br 20s → 205* Poxidized) 2e + Brz- Br" creduced). Reducing feagent: oxidizing agent. 14. Write the Molecular. Ionic and Net Ionic equations for the reaction between Mg(NO3)2 (aq) and LisPO4 (aq). Mg(NO3)2 + Liz PO4 - MADO4 + Liz...
Suppose the galvanic cell sketched below is powered by the following reaction: Ni(s)+Pb(NO3),(aq) → Ni(NO3)2(aq)+Pb(s) E1 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?
1. Balance the reaction between Mg and
NO3- to form
Mg2+ and
HNO2 in acidic solution.
When you have balanced the equation using the smallest integers
possible, enter the coefficients of the species shown. Enter "1" if
the coefficient is "1."
Mg + NO3Mg2+
+ HNO2
Water appears in the balanced equation as a (reactant,
product, neither) with a coefficient of ______. (Enter 0 for
neither.)
How many electrons are transferred in this reaction? _______
.
.
2. Balance the following...
a.) Cu 2 b.) Mg +29) +2e- → Cus) + 2e- → Mg(s) (aq) c.) Mg, → Mgt? (aq) + 2e- → Cus+ 2e- d.) Cu (aq) the reduction half reaction is a.) Cut2 +2e- → Cus) b.) Mg? (aq) + 2e- → Mgie c.) Mg» → Mg(aq) + 2e- → + 2e- d.) Cu (aq) Cuis) is being oxidized a.) Cu? (aq) b.) Mg(s) c.) Mg (aq) d.) Cu(s) RING 2018 is being reduced a.) Cu 2 (aq) b.)...
2. For the oxidation-reduction reaction 3Mn(s) + 2Fe(NO3)3(aq) → 2Fe(s) + 3Mn(NO3)2 (aq) Hint: HNO3 a) provide equation for the oxidation half-reaction: b) provide equation for the reduction half-reaction: In the given equation above or in your answers to a) and b): c) label the substance which is oxidizing agent, d) label the substance which is reducing agent.
17) Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s) A) Ag B) Ni C) CI D) O E) This is not an oxidation-reduction reaction. 18) When an aqueous solution of manganese (II) nitrate is combined with an aqueous solution of ammonium sulfide, what should precipitate out? A) Mns B) Mn(SO3)2 C) Mn(SO4)2 D) Mn 2503 E) Mn 2504 19) If 4.89 g of ZnCl2 is dissolved in enough water to give a total...
3) Given: Sn(NO:)2 (aq) + Ni(s) > Sn (s)+ Ni(NO3)2 (aq) Write the standard electrochemical line notation and sketch a complete cell diagram for this electrochemical cell. Calculate the value of E cell.
When answering Parts a-h, consider only the molecules and ions,
Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq),
and Cr2O7^2-(aq), under standard state conditions. (1 pt each)
Use standard reduction table.
a) Which of these molecules and ions are oxidizing agents?
b) Which of these molecules and ions are reducing agents?
c) List the oxidizing agents from part a in DECREASING order of
oxidizing agent strength. (strongest OA to weakest OA)
d) List the reducing agents from part b in DECREASING order of...
PLL35 W 13. For the following redox reaction, 2CBn 2CsBr a) write the two half reactions b) identify what is oxidized and what is reduced c) identify the oxidizing agent and the reducing reagent 20s + Br2 -> 2 Cs Br 20s → 205* Poxidized) 2e + Brz- Br" creduced). Reducing feagent: oxidizing agent. 14. Write the Molecular. Ionic and Net Ionic equations for the reaction between Mg(NO3)2 (aq) and LisPO4 (aq). Mg(NO3)2 + Liz PO4 - MADO4 + Liz...
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