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20.19 Indicate whether the following balanced equations involve oxidation-reduction. If...
Identify the species (atoms/ elements) undergoing oxidation and reduction in the following equations, assign oxidation numbers...
Identify the species (atoms/ elements) undergoing oxidation and
reduction in the following equations, assign oxidation numbers to
each, and write balanced net ionic equations.
a) Cu(s)
Cu2+(aq) + 2e-
b) Cl2(aq) + 2e-
Cl-(aq)
c) Cu(s) + Cl2(aq)
Cu2+(aq) + 2Cl-(aq)
d) 4CuO(s) + CH4(g)
4Cu(s) + CO2(g) + 2H2O(l)
e) 2CuSO4(aq) + 4KI(aq)
2CuI (aq) + 2K2SO4(aq) +
I2(aq)
f) Cu2O(s) + Fe(SO4)3 (aq) +
H2SO4(aq)
2CuSO4(aq) + 2FeSO4(aq) +
H2O(l)
any oxidation-reduction reactions can be balanced by i spection. Try to balance the following reactions by...
any oxidation-reduction reactions can be balanced by i spection. Try to balance the following reactions by inspection In each reaction, identify the substance reduced and the sub stance oxidized. a. Al(s) + HCl(aq)→AICI3(aq) 12(g) b. CH4(g) + S(s) → CS2(l) + H2S(g) c. C3H8(g) + O2(g) → CO2(g) + H2O(1) d. Cu(s) + Ag+(aq) → Ag(s) + Cu2+ (aq)
for each reaction- classify as oxidation-reduction,acid-base or precipitation Classify each of the following reactions as oxidation-reduction,...
for each reaction- classify as oxidation-reduction,acid-base
or precipitation
Classify each of the following reactions as oxidation-reduction, acid-base, or Note that in order to be a redox reaction, the oxidation number of an element must be different when it is a reactant than when it is a product. (1 point each) precipitation. Classification Reaction Number 24 Ca (s) +2 H2O ()- Ca(OH)2 (s) + H2 (g) 25 CdCl2 (aq)+ Na2S (aq)CdS (s) +2 NaCl (aq) Zn(OH)2 (s) + H2SO4 (aq)ZnSO4 (aq)...
RODOX EXAMINATION An oxidation-reduction reaction involves the (1) sharing of electrons &n
RODOX EXAMINATION An oxidation-reduction reaction involves the (1) sharing of electrons (3) transfer of electrons (2) sharing of protons (4) transfer of protons In this reaction, CO→ 2 CO + O2 the oxidation number of carbon changes from: (1) 0 to +4 (3) +3 to 0 (2) +2 to +4 (4) +4 to +2 Which balanced equation represents a redox reaction? AgNO3 (aq) +NaCl (aq) →AgCl (s) +NaNO3 (aq) H2CO3 (aq)...
Three parts for each of the balanced equations in a) and b): Part 1. Indicate whether...
Three parts for each of the balanced equations in a) and b): Part 1. Indicate whether the reaction is a precipitation reaction, an acid-base reaction, or an oxidation-reduction reaction. Part 2. If the reaction is a precipitation reaction, identify the precipitate. If the reaction is an acid-base reaction, identify the acid and the base. If the reaction is an oxidation-reduction reaction, indicate which reactant is oxidized and which reactant is reduced. Part 3. Write the total ionic equation for each...
Which of the following reactions is an oxidation-reduction reaction? A) NH4HS(s) → NH3(g) + H2S(g) B)...
Which of the following reactions is an oxidation-reduction reaction? A) NH4HS(s) → NH3(g) + H2S(g) B) 2 NaHCO3(s) → Na2CO3(s) + H2O(g) + CO2(g) C) N2O4(g) → 2 NO2(g) D) 2 SO2(g) + O2(g) → 2 SO3(g) E) 2 HC2H3O2(aq) + Ba(OH)2(aq) → Ba(C2H3O2)2(aq) + 2 H2O(l)
Write balanced equations for the following oxidation-reduction reactions. Show your work. a. The oxidation of Zn...
Write balanced equations for the following oxidation-reduction reactions. Show your work. a. The oxidation of Zn by MnO4- in an acidic solution to form Zn^2+ and MnO2 b. The oxidation of NO2 by Au^3+ in basic solution to form Au and NO3-
1. Write balanced net ionic equations for the following oxidation-reduction reac- tions: a. Hydrogen sulfide is...
1. Write balanced net ionic equations for the following oxidation-reduction reac- tions: a. Hydrogen sulfide is added to a solution of Fe(NO3)3. b. Hydrogen peroxide is added to an acidic solution of an iron(II) salt c. The Mn2+ ion is oxidized to MnO2 by KCIO3 in acidic solution (assuming reduction of ClOs to CI-), e Cr20,2 complex ion is reduced to Cr3+ by H2S in acidic solution. e. The compound Co(OH)2 is oxidized to Co(OH)s upon standing in contact with...
Complete and balance the following half-reactions. In each case, indicate whether oxidation or reduction occurs. H2O2...
Complete and balance the following half-reactions. In each case, indicate whether oxidation or reduction occurs. H2O2 (aq) → H2O (aq) acidic solution Cl2 (g) → ClO3- (aq) acidic solution
Part III: Oxidation and Reduction of H2O2 1. Reduction of H2O2: H2O2(aq) + Cr(OH)3(S) (BASIC) •...
Part III: Oxidation and Reduction of H2O2 1. Reduction of H2O2: H2O2(aq) + Cr(OH)3(S) (BASIC) • Observations · Evidence of the oxidation of Cr3+ • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction · Explain occurrence or non-occurrence of reaction by calculating cell. 2. Oxidation of H2O2: H2O2(aq) + FeCl3(aq) • Observations • Evidence of the oxidation of H2O2 • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction • Explain occurrence or...
Identify the species (atoms/ elements) undergoing oxidation and
reduction in the following equations, assign oxidation numbers to
each, and write balanced net ionic equations.
a) Cu(s)
Cu2+(aq) + 2e-
b) Cl2(aq) + 2e-
Cl-(aq)
c) Cu(s) + Cl2(aq)
Cu2+(aq) + 2Cl-(aq)
d) 4CuO(s) + CH4(g)
4Cu(s) + CO2(g) + 2H2O(l)
e) 2CuSO4(aq) + 4KI(aq)
2CuI (aq) + 2K2SO4(aq) +
I2(aq)
f) Cu2O(s) + Fe(SO4)3 (aq) +
H2SO4(aq)
2CuSO4(aq) + 2FeSO4(aq) +
H2O(l)
any oxidation-reduction reactions can be balanced by i spection. Try to balance the following reactions by inspection In each reaction, identify the substance reduced and the sub stance oxidized. a. Al(s) + HCl(aq)→AICI3(aq) 12(g) b. CH4(g) + S(s) → CS2(l) + H2S(g) c. C3H8(g) + O2(g) → CO2(g) + H2O(1) d. Cu(s) + Ag+(aq) → Ag(s) + Cu2+ (aq)
for each reaction- classify as oxidation-reduction,acid-base
or precipitation
Classify each of the following reactions as oxidation-reduction, acid-base, or Note that in order to be a redox reaction, the oxidation number of an element must be different when it is a reactant than when it is a product. (1 point each) precipitation. Classification Reaction Number 24 Ca (s) +2 H2O ()- Ca(OH)2 (s) + H2 (g) 25 CdCl2 (aq)+ Na2S (aq)CdS (s) +2 NaCl (aq) Zn(OH)2 (s) + H2SO4 (aq)ZnSO4 (aq)...
1. Write balanced net ionic equations for the following oxidation-reduction reac- tions: a. Hydrogen sulfide is added to a solution of Fe(NO3)3. b. Hydrogen peroxide is added to an acidic solution of an iron(II) salt c. The Mn2+ ion is oxidized to MnO2 by KCIO3 in acidic solution (assuming reduction of ClOs to CI-), e Cr20,2 complex ion is reduced to Cr3+ by H2S in acidic solution. e. The compound Co(OH)2 is oxidized to Co(OH)s upon standing in contact with...
Part III: Oxidation and Reduction of H2O2 1. Reduction of H2O2: H2O2(aq) + Cr(OH)3(S) (BASIC) • Observations · Evidence of the oxidation of Cr3+ • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction · Explain occurrence or non-occurrence of reaction by calculating cell. 2. Oxidation of H2O2: H2O2(aq) + FeCl3(aq) • Observations • Evidence of the oxidation of H2O2 • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction • Explain occurrence or...
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