1. Determine ΔGo for the following reaction: 2 Na(s) + 2 H2O(l) --> H2(g) + 2...

1. Determine ΔG^o for the following reaction:

2 Na(s) + 2 H₂O(l) --> H₂(g) + 2 OH^-(aq) + 2 Na⁺(aq)

2. Calculate K for the oxidation of iron by H⁺:

2 Fe(s) + 6 H⁺(aq) --> 2 Fe³⁺(aq) + 3 H₂(g)

Solutions

Expert Solution

2Na(s) ------------------> 2Na^+ (aq) + 2e^- E0 = 2.71v

2H2O(l) +2e^- -------> H2(g) + 2OH^- (aq) E0 = -0.83v

------------------------------------------------------------------------------------

2 Na(s) + 2 H₂O(l) --> H₂(g) + 2 OH^-(aq) + 2 Na⁺(aq) E0cell = 1.88v

n = 2

ΔG^o = -nE0cell*F

= -2*1.88*96500

= -362840J/mole = -362.84KJ/mole

2Fe(s) --------------> 2Fe^3+(aq) + 6e^- E0 = 0.04v

6H^+ (aq) + 6e^- ------> 3H2(g) E0 = 0.00v

------------------------------------------------------------------------------

2 Fe(s) + 6 H⁺(aq) --> 2 Fe³⁺(aq) + 3 H₂(g) E0cell = 0.04v

n = 6

ΔG^o = -nE0cell*F

= -6*0.04*96500

= -23160J/mole

ΔGo = -RTlnK

-23160 = -8.314*298*2.303logK

-23160 = -5705.84logK

logK = -23160/-5705.84

logK = 4.06

K = 10^4.06 = 1.15*10^4 >>>>answer

queen_honey_blossom answered 1 year ago

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