Question

For the following reactions, write a balanced equation using half-reactions and calculate the voltage to be expected.

Answer 1

a) $2Na(s) +2H_2O(I)$→ $2Na^+(aq) + OH^-(aq)+ H_2(g)$

b) $2Ag (s) +2H^(aq)$ → $2 Ag^+ (aq) +H_2(g)$

What are half-reactions?

The half-reaction method is a way to balance redox reactions. It involves breaking the overall equation down into an oxidation part and a reduction part.

a)

$2Na(s) +2H_2O(I)$→ $2Na^+(aq) + OH^-(aq)+ H_2(g)$

$E^0 cell = E^0 (reduction) - E^0 (oxidation)$

= $E^0(\frac{H_2O}{H_2}, OH^-) -E^0(Na^+/Na)$

= -0.83 - (-2.71) =1.88V

b)

$2Ag (s) +2H^(aq)$ → $2 Ag^+ (aq) +H_2(g)$

$E^0cell$= $E^0(H^+/H_2) -E^0(Ag^+/Ag)$

$E^0cell$=-0. - (0.8) =-0.8V

Learn more about the half-reactions here:

https://brainly.in/question/18053421

#SPJ1