Question

Messages Due in 8 hours, 54 minutes. Due Mon 11/11/2019 1:59p 0.689 M, the reaction is 36.3 % complete at 90.7 min. Calculate the The reaction A B+C is second order with respect to A. When [A]o half-life for this reaction. Show your work:

Answer 1

for second order reaction

first calculate rateconstant

1 / [A] = 1/ [A₀] + Kt

[A₀] = 0.689 M

[A] = assume X

% = (X / 0.689) x 100

36.3 = (X / 0.689) x 100

X / 0.689 = 0.363

X = 0.250

[A] = 0.689 - 0.250 = 0.439 M

1 / [0.439] = 1 / [0.689] + K x 90.7

2.28 = 1.45 + 90.7 K

90.7 K = 0.83

K = 0.009 M^-1s^-1

now

t_1/2 = 1 / K[A₀]

t_1/2 = 1 / 0.009 [0.689]

t_1/2 = 1 / 0.0062

t_1/2 = 161 min