A first order reaction gets completed to75% in 32 minutes.how much tim

1.	A first order reaction gets completed to75% in 32 minutes.how much time would have been requird for 50% completion
Answer» Answer: Let INITIAL amount = A after 32 minutes = 75% of A COMPLETED = 0.75A we know , formula for 1st order reaction , K = 2.303/t log[ initial ]/[final] = 2.303/32 log{ A/(A - 0.75A)} ={2.303/32}× LOG4 --------(1) for half LIFE , formula is T½ = 2.303/K log2 put K ={2.303/32} × log4 T½ = 2.303/[{2.303/32} × log4 ] × log2 = 32 log2/log4 = 32log2/2log2 = 16 min hence, half life of given reaction is 16 minutes . hope..it..helps.. don't forget to make me brainlist...

A first order reaction gets completed to75% in 32 minutes.how much time would have been requird for 50% completion

Answer»

Answer:

Let INITIAL amount = A

after 32 minutes = 75% of A COMPLETED = 0.75A

we know , formula for 1st order reaction ,

K = 2.303/t log[ initial ]/[final]

= 2.303/32 log{ A/(A - 0.75A)}

={2.303/32}× LOG4 --------(1)

for half LIFE , formula is

T½ = 2.303/K log2

put K ={2.303/32} × log4

T½ = 2.303/[{2.303/32} × log4 ] × log2

= 32 log2/log4

= 32log2/2log2

= 16 min

hence, half life of given reaction is 16 minutes .

hope..it..helps..

don't forget to make me brainlist...