Question

In: Chemistry

1. Determine the equilibrium constant for the following reaction at (3.950x10^2) K. 2 A(g) + B2(g)...

1. Determine the equilibrium constant for the following reaction at (3.950x10^2) K.

2 A(g) + B2(g) → 2 AB(s)     ΔH° = -(2.2x10^2) kJ; ΔS° = -(3.988x10^2) J/K

2.

A+ (aq) + BC3- (aq) à A(BC3)(s) ΔH° f = -64.4 kJ/mol

For the above reaction ΔSsys is ________(positive or negative), and ΔG is __________ (positive or negative) and the reaction is _______________ (spontaneous or nonspontaneous) at 600K  

3.

Which of the following pairs of reactants will result in a spontaneous reaction at 25°C. (select all that are spontaneous)

Pb2+(aq) + 2e- → Pb (s)    Eºcell= -0.13V
Cu+(aq) + e- → Cu (s)      Eºcell= +0.52
Ag+(aq)+ e- → Ag (s)       Eºcell= +0.80
Br2 (l)+ 2e- → 2 Br- (aq)   Eºcell= +1.09
Li+(aq) + e- → Li (s)         Eºcell= -3.04
Al 3+(aq)+ 3e- → Al (s)     Eºcell= -1.66
Fe3+(aq) + 3e- → Fe (s)    Eºcell= -0.036
Ni2+(aq) + 2e- → Ni (s)     Eºcell= -0.23

Solutions

Expert Solution

Hope it helps you please thumb's up.

queen_honey_blossom answered 2 years ago
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