Question

not sure if im doing it correctly

| (c) Sa (a) Al2(50), 3:9; 2)+3.030 S=+5 1838 5 5 2. Balance each redox reaction. Then, classify each reaction as combination, decomposition or displacement. Identify the oxidizing and reducing agents. +2 2 -2 (a)2NO(g) + O2(g) - N2020) Combination 2(2) + 2(x) = 6 -2(4) + 2(x120 2 th oxidized (#vent up) reducing 4 2 (6) Čr(NO3)3(aq) + Al(s) – A(NO3)3(aq) + cřís Displacement 1(3) + 3x)+91-2)=0 Gr Cro reduced C#went down) oxidizing 3+30%) +18-0 -3 X =5 ti 3 Follow up question: How do you know if this reaction actually occurs? If Fe(s) is used in place of Al(s) in the above reaction, does it still occur? Explain. The reaction will not accur because it is below Cr in the activity series. ill not car becoin, does it still occur Bescolars? If Fe(s) is

Answer 1

oxidized +4 -2 2. a 2 Noigt on N2O4(e) reduced It is a combination reaction A + B C Either A or B or both A and B must be in the elemental form for such a reaction to be redox rekn. oxidired +3 + 52 b) 3 Cr(NO) +2Al(s) - 2A1(NO3)3 (as)' +2 + 52 2Y + 7 reduced It is a displacement reaction x + y2 – x2 + y In this reaction one metal in the combined state may be displaced by another metal in the uncombined state.

The above reaction is possible because Al is located above Cr in the activity series. Thus Al can displace. cx from its combined state It fe(s) is used in place of Al this reaction will not occur because fe is located below cr in the activity series. Thus fe cannot displace Gr from its combined state.