Download 1. Identify the reactants and products in each of the following

1. Identify the reactants and products in each of the following reactions:
a) BaO2(s) + H2SO4(l) → BaSO4(s) + H2O2
b) 2H2O2(aq) → 2H2O(l) + O2(g)
c) methane + water → carbon monoxide + hydrogen
d) copper(II) oxide + hydrogen → copper + water
a) Reactants = BaO2 and H2SO4
Products = BaSO4 and H2O2
b) Reactants = H2O2
Products = H2O and O2
c) Reactants = methane and water
Products = carbon monoxide and hydrogen
d) Reactants = copper(II) oxide and hydrogen
Products = copper and water
2. Identify which of the following are consistent with the law of conservation of
matter. For those that are not, explain why they are not.
a) 4Al(s) + 3O2(g) → 2Al2O3(s) b) 3.20 g O2 + 3.21 g S → 6.41 g SO2
c) P4(s) + O2(g) → P4O10(s) d) CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
a) Consistent
b) Consistent
c) Not consistent, number of oxygen atoms does not balance
d) Consistent
3. Determine the number of atoms of each element on each side of the
following equations and decide which equations are balanced:
a) H2S(aq) + I2(aq) → 2HI(aq) + S(s)
b) KClO3(s) → KCl(s) + O2(g)
c) SO2(g) + H2O(l) → H2SO4(aq)
d) Ba(ClO3)2(aq) + H2SO4(aq) → 2HClO3(aq) + BaSO4(s)
a) Reactants: 2H, 1S, 2I
Products: 2H, 1S, 2I
Balanced
b) Reactants: 1K, 1Cl, 3O
Products: 1K, 1Cl, 2O
Not balanced
c) Reactants: 1S, 3O, 2H
Products: 1S, 4O, 2H
Not balanced
d) Reactants: 1Ba, 2Cl, 10O, 2H, 1S
Products: 1Ba, 2Cl, 10O, 2H, 1S
Balanced
4. For each of the following equations, indicate whether the underlined
element has been oxidized, reduced, or neither oxidized or reduced.
a) 2Mg(s) + O2(g) → 2MgO(s)
b) CuO(s) + H2(g) → Cu(s) + H2O(g)
c) Ag+(aq) + Cl-(aq) → AgCl(s)
d) BaCl2(aq) + H2SO4(aq) → BaSO4(s) + 2HCl(aq)
e) Zn(s) + 2H+(aq) → Zn2+(aq) +H2(g)
a) Oxidized
b) Reduced
c) Neither
d) Neither
e) Oxidized
5. Assign oxidation numbers to each element in the following equations and
identify the oxidizing and reducing agents:
a) H2(g) + Cl2(g) → 2HCl(g)
b) H2O(g) + CH4(g) → CO(g) + 3H2(g)
c) CuO(s) + H2(g) → Cu(s) + H2O(g)
d) B2O3(s) + 3Mg(s) → 2B(s) + 3MgO(s)
e) Fe2O3(s) + CO(g) → 2FeO(s) + CO2(g)
f) Cr2O72-(aq) + 2H+(aq) + 3Mn2+(aq) → 2Cr3+(aq) + 3MnO2(s) + H2O(l)
a) Reactants: H 0, Cl 0
Products: H +1, Cl -1
Oxidizing agent is Cl2 and reducing agent is H2
b) Reactants: H +1, O -2, C -4
Products: H 0, O -2, C +2
Oxidizing agent is H2O and reducing agent is CH4
c) Reactants: Cu +2, O -2, H 0
Products: Cu 0, O -2, H +1
Oxidizing agent is CuO and reducing agent is H2
d) Reactants: B +3, O -2, Mg 0
Products: B 0, O -2, Mg +2
Oxidizing agent is B2O3 and reducing agent is Mg
e) Reactants: Fe +3, O -2, C +2
Products: Fe +2, O -2, C +4,
Oxidizing agent is Fe2O3 and reducing agent is CO
f) Reactants: Cr +6, O -2, H +1, Mn +2
Products: Cr +3, O -2, Mn +4, H +1
Oxidizing agent is Cr2O72- and reducing agent is Mn2+
6. Classify each of the reactions represented by the following equations first
as a redox or nonredox reaction. Then further classify each redox reaction as
a decomposition, single-replacement, or combination reaction; and each
nonredox reaction as a decomposition, double-replacement, or combination
reaction.
a) N2O5(g) + H2O(l) → 2HNO3(aq)
b) Cr2O3(s) + 2Al(s) → 2Cr(s) + Al2O3(s)
c) CaO(s) + SiO2(s) → CaSiO3(s)
d) H2CO3(aq) → CO2(g) + H2O(l)
e) PbCO3(s) → PbO(s) +CO2(g)
f) Zn(s) + Cl2(g) → ZnCl2(s)
a) Reactants: N +5, O -2, H +1
Products: N +5, O -2, H +1
Non-redox, combination
b) Reactants: Cr +6, O -2, Al 0
Products: Cr 0, Al +3, O -2
Redox, single replacement
c) Reactants: Ca +2, O -2, Si +4
Products: Ca +2, Si +4, O -2
Non-redox, combination
d) Reactants: H +1, C +4, O -2
Products: H +1, C +4, O -2
Non-redox, decomposition
e) Reactants: Pb +2, C +4, O -2
Products: Pb +2, C +4, O -2
Non-redox, decomposition
f) Reactants: Zn 0, Cl 0
Products: Zn +2, Cl -1
Redox, combination