Question

The following chemical reaction: A → products shows second order kinetics with respect to A; rate k[A2 Assume k = 11.88 x 10-5 mol-1 L s-1 If the initial concentration of A is 0.28 mol L-1, what is the concentration of A in mol L-1) after 3.03 hours? You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 101" should be entered as "4.32E4"

help please

Answer 1

for second order

1/ [A] = Kt + 1/[A₀]

K = 11.88 x 10^-5 mol^-1 L s^-1

t = 3.03 h = 10908 s

[A₀] = 0.28 mol L^-1

[A] = ?

1 / [A] = 11.88 x 10^-5 x 10908 + 1/ [0.28]

1 / [A ] = 1.296 + 3.57

1 /[A] = 4.866

[A] = 0.20 mol L^-1