At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.118 M^-1* s^-1:
ClCH2CH2Cl (g) > CH2CHCI(g) + HCl (g)
a) Suppose a vessel contains ClCH2CH2Cl at a concentration of 1.41 M. Calculate how long it takes for the concentration of CICH2CH2Cl to decrease to 10.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.

Hello there,it will only be somewhat eroded (25%)hope this : ))~top

Answer:             1.0  × 10⁻⁵ msolution:                     as we know ph is given as,                                    ph  = -log [h⁺]and,                                    [h⁺]  =  10^-ph    (1)putting value of ph in eq. 1,                                    [h⁺]  =  10⁻⁵                                    [h⁺]  =  1.0  × 10⁻⁵ m