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

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

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 1 year ago

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