+ 5 Br (aq) 0.00200M 1. Consider this reaction and the experimental quantities given in the...

     

Transcribed Image Text:

+ 5 Br (aq) 0.00200M 1. Consider this reaction and the experimental quantities given in the table. BrO3 (aq) + 6 H+ (aq) 3 Br, 2 (aq) + 3 H₂O (1) Run 0.00200M 0.0200M H₂O Total KBr No. KBrO, (mL) HCl (mL) (mL) volume (mL) Initial Rate= A[Br₂] At (M/s) (mL) 1 10.0 10.0 10.0 70.0 100.0 1.44 X 10-12 2 20.0 10.0 10.0 60.0 100.0 2.88 X 10-12 3 10.0 20.0 10.0 60.0 100.0 2.88 X 10-12 to hol 4 10.0 10.0 20.0 60.0 100.0 5.76 X 10-12 a. Calculate the molarities in each of the reaction mixtures. Run No. KBr KBrO3 M HCl 1 0.0002 0.0002 0.002 2 0.0004 0.0002 0.0002 3 0.0002 0.0004 .002 0.0004.002 4 .0002 .0002 .004 b. Determine the order of each reactant. (Show work below.) order of [Br] order of [BrO3] order of [H+] C. Determine the value of the rate constant (including units) for the formation of Br₂. d. Write the complete rate law expression for the formation of Br.. e. What would be the initial rate of formation of Br, (in units of M/s) when the following initial concentrations were used? [Br] =3.00 x 10-2 M; [BrO,] = 8.00 x 10-2 M; [H+] = 2.00 x 10-2 M f. Under the conditions specified in part "e" (directly above), what would be the initial rate of disappearance of hydrogen ion (in units of M/s) for this reaction? + 5 Br (aq) 0.00200M 1. Consider this reaction and the experimental quantities given in the table. BrO3 (aq) + 6 H+ (aq) 3 Br, 2 (aq) + 3 H₂O (1) Run 0.00200M 0.0200M H₂O Total KBr No. KBrO, (mL) HCl (mL) (mL) volume (mL) Initial Rate= A[Br₂] At (M/s) (mL) 1 10.0 10.0 10.0 70.0 100.0 1.44 X 10-12 2 20.0 10.0 10.0 60.0 100.0 2.88 X 10-12 3 10.0 20.0 10.0 60.0 100.0 2.88 X 10-12 to hol 4 10.0 10.0 20.0 60.0 100.0 5.76 X 10-12 a. Calculate the molarities in each of the reaction mixtures. Run No. KBr KBrO3 M HCl 1 0.0002 0.0002 0.002 2 0.0004 0.0002 0.0002 3 0.0002 0.0004 .002 0.0004.002 4 .0002 .0002 .004 b. Determine the order of each reactant. (Show work below.) order of [Br] order of [BrO3] order of [H+] C. Determine the value of the rate constant (including units) for the formation of Br₂. d. Write the complete rate law expression for the formation of Br.. e. What would be the initial rate of formation of Br, (in units of M/s) when the following initial concentrations were used? [Br] =3.00 x 10-2 M; [BrO,] = 8.00 x 10-2 M; [H+] = 2.00 x 10-2 M f. Under the conditions specified in part "e" (directly above), what would be the initial rate of disappearance of hydrogen ion (in units of M/s) for this reaction?

Answer rating: 100% (QA)

b To determine the order of each reactant we can use the method of initial rates By comparing the in... View the full answer