HI decomposes into its elements according to second-order kinetics. What concentration of HI remains from an initial concentration of 2.30 M after 4.5 hours? The rate constant, k, equals 1.6 x 10-3 M-1 hr-1.

Therefore (2.30-0.03747)= 2.2625 M of HI remains from an initial concentration of 2.30 M after 4.5 hours.

Step-by-step explanation:

second order reaction: The rate of reaction  proportional to the square of the concentration of reactant.

For second order reaction

K is rate constant = 1.6×10⁻³M⁻¹hr⁻¹

a = initial concentration of reactant = 2.30 M

a-x = concentration of reactant after t h

t = time = 4.5 h

Putting the values in the above equation,

Therefore (2.30-0.03747)= 2.2625 M of HI remains from an initial concentration of 2.30 M after 4.5 hours.

dc=6 square root of 3 and ac is 12 square root 3

c and d

step-by-step explanation:

square root of 3/2 = 18/c

cross multiply to get 18*2=√3*c

36/√3 * √3/√3 = c

c= 36*√3/3

c=12√3