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 number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

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