if one percent of the reactant decomposes in first minute in a first order reaction calculate how much reactant would remain undecomposed after one hour
Dear student
We can use the equation for the first order kinetics as:
Lets say the initial concentration is A0 .
Now the percentage decomposition in first minute is 1% i.e, now the concentration of A that is left is
A0 - (A0/100) = 0.99Ao.
so the equation becomes,
0.99 Ao = Ao e-k1min
So 0.99 = e-k1min
ln 0.99 = -k *1 min
so k = - ln 0.99
So In 1 hour or 60 minutes thus the
new concentration of the reactant will be,
A = Ao(e-(-ln 0.99)*60 min)
So A = 0.5471 Ao
so after the given time, 54.71% of the initial reactant will be remaining.
Regards
We can use the equation for the first order kinetics as:
Lets say the initial concentration is A0 .
Now the percentage decomposition in first minute is 1% i.e, now the concentration of A that is left is
A0 - (A0/100) = 0.99Ao.
so the equation becomes,
0.99 Ao = Ao e-k1min
So 0.99 = e-k1min
ln 0.99 = -k *1 min
so k = - ln 0.99
So In 1 hour or 60 minutes thus the
new concentration of the reactant will be,
A = Ao(e-(-ln 0.99)*60 min)
So A = 0.5471 Ao
so after the given time, 54.71% of the initial reactant will be remaining.
Regards