A reaction has a rate constant of 0.0396 sec-1; how long will it take (in minutes) until 0.292 mol/L of the compound is left, if there was 0.803 mol/L at the start? (give answer to 3 decimal places)?

t = 0.426 min

Explanation:

assuming order one for the reaction:

∴ K = 0.0396/s

∴ Ca = 0.292 mol/L

∴ Cao = 0.803 mol/L

⇒ K∫δt = - ∫δCa/Ca

⇒ K*t = Ln (Cao/Ca)

⇒ t = [ Ln (Cao/Ca) ] / K

⇒ t = [ Ln (2.75) ] / (0.0396/s)

⇒ t = ( 1.0116)/(0.0396/s)

⇒ t = 25.545 s = 0.426 min

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.