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Which of the following expressions is co...

Which of the following expressions is correct for the rate of reaction given below?
`5Br^(-)(aq)+BrO_(3)^(-)(aq)+6H^(+)(aq) to 3Br_(2)(aq)+3H_(2)O(l)`

A

`(Delta[Br^(-)])/(Deltat)=5(Delta[H^(+)])/(Deltat)`

B

`(Delta[Br^(-)])/(Deltat)=(6)/(5)(Delta[H^(+)])/(Deltat)`

C

`(Delta[Br^(-)])/(Deltat)=(5)/(6)(Delta[H^(+)])/(Deltat)`

D

`(Delta[Br^(-)])/(Deltat)=6(Delta[H^(+)])/(Deltat)`

Text Solution

Verified by Experts

The correct Answer is:
C
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Which of the following expression is correct for the rate of reaction given below ? 5Br^(-)(aq) + BrO_(3)^(-)(aq) + 6H^(+) (aq) to 3Br_(2) (aq) + 3H_(2) O(l) .

Consider the following reaction in aqueous solution 5Br^(-) (aq) + BrO_(3)^(-) (aq) + 6H^(+)(aq) to 3Br_(2)(aq) + 3H_(2)O(l) If the rate of appearance of Br_(2) at a particular time during the reaction is 0.025 M"sec"^(-1) , what is the rate of disappearance (in "Msec"^(-1) ) of Br^(-) at that time?

Determining the order of reaction from the rate law: Bromide ion is oxidized by bromate ion in acidic solution. 5Br^(-)(aq.)+BrO_(3)^(-)(aq.)+6H^(+)(aq.)rarrBr_(2)(aq.)+3H_(2)O(l) The expermentally determined rate law is "Rate" = k[Br^(-)][BrO_(3)^(-)][H^(+)]^(2) What is the order of reaction with respect to each of the reactants and what is teh overall reaction order ? Strategy : To find the reaction order with respect to each reactant, look at the exponents in the rate law, not the coefficients in the balanced chemical equation, and then sum the exponents to obtain the overall reaction order.

5Br^(-)(aq)+BrO_(3)^(-)(aq)+6H^(+)(aq) rarr 3 Br_2(aq) + 3 H_2O(l) which of the following is incorrect regarding the rate of the reaction? (A) Rate= - d[Br^(-)] /dt (B) Rate =- d[BrO_(3)^(-)] /dt (C) - d[Br^(-)] /dt =(5)/(3) d[Br_(2)] /dt (D) - d[BrO_(3)^(-)] /dt = (1)/(3) d[Br_(2)] /dt

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