Question

urgent

7) Small amounts of the metal barium (Ba, MW = 137.33 g/mol) can be produced by electrolysis. The half-reaction for the production of barium metal is Ba²+ + 2 e → Ba Electrolysis is carried out using a current i = 15.0 amp (1 amp = 1 C/s). How long (in minutes) will it take to produce 16.0 g of barium metal? (12 points)

Answer 1

Answer:- t= 25.0 min Solution:- since we know that Ba2+ + 2e Ba since we know that from faraday's law m*n*f/Z*i=t ............ -(1) m = mass Z= molecular weight i= current in A n = no of electrons f=faraday's constant t=time in sec It is given that Z= molecular weight = 137.33 g i= current in A = 15.0 A = 15.0 C/sec n=no of electrons = 2 f=faraday's constant = 96500 C m = 16.0 g Now from eqn 1 m*n*f/Z*i=t t=(16.0*2*96500)/(137.33*15.0) t=1,499.0655112988179 sec t=24.98 min t=25.0 min Answer Please give me thumbs up

Note:- answer may vary because in some places people uses 96500 or 96485.33

so use whatever is in your textbook

hope it helps