Answer:
option A.
Explanation:
given,
rate constant. k = 0.241/min
[A_0] = 0.859 M
[A_t] = ?
t = 10 minutes.
using first order reaction formula
[tex]k=\dfrac{2.303}{t}log(\dfrac{[A_0]}{[A_t]})[/tex]
[tex]0.241=\dfrac{2.303}{10}log(\dfrac{[0.859]}{[A_t]})[/tex]
[tex]log(\dfrac{[0.859]}{[A_t]}) = 1.0464[/tex]
[tex]\dfrac{[0.859]}{[A_t]} = 11.129[/tex]
[tex][A_t]=\dfrac{0.859}{11.129}[/tex]
[tex][A_t]=0.0772\ M[/tex]
the concentration of A after 10 minutes is equal to 0.0772 M.
Hence, the correct answer is option A.
