Question

1) From the balanced molecular equations, write the complete ionic and net ionic equations for the following. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)

a) SnCO₃(s) + H₂SO₄(aq) → SnSO₄(s) + CO₂(g) + H₂O(l)

b) Sr(NO₃)₂(aq) + H₂SO₄(aq) → SrSO₄(s) + 2 HNO₃(aq)

c) K₂C₂O₄(aq) + Pb(OH)₂(aq) → 2 KOH(aq) + PbC₂O₄(s)

2) Indicate what type, or types, of reaction each of the following represents. (Select all that apply.)

(a) 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

acid-base, combustion, double displacement, neutralization, oxidation-reduction, precipitation, single-displacement

(b) Sn(NO₃)₂(aq) + H₂SO₄(aq) → SnSO₄(s) + 2 HNO₃(aq)

acid-base, combustion, double displacement, neutralization, oxidation-reduction, precipitation, single-displacement

(c) C₄H₈O₂(l) + 5 O₂(g) → 4 CO₂(g) + 4 H₂O(g)

acid-base, combustion, double displacement, neutralization, oxidation-reduction, precipitation, single-displacement

(d) Al(OH)₃(aq) + 3 HBr(aq) → AlBr₃(aq) + 3 H₂O(l)

acid-base, combustion, double displacement, neutralization, oxidation-reduction, precipitation, single-displacement

Answer 1