Home
Class 12
CHEMISTRY
From the rate laws for the reactions giv...

From the rate laws for the reactions given below, determine order with order to each species and the overall order:
(a) `2HCrO_(4)^(ɵ) + 6l^(ɵ) + 14H^(o+) rarr 2Cr^(3+) + 3I_(2) + 8H_(2)O`
Rate `= k[HCrO_(4)^(ɵ) ][I^(ɵ) ]^(2) [H^(o+)]^(2)`
(b) `H_(2)O_(2) + 2I^(ɵ) +2H^(o+) rarr I_(2)+2H_(2)O`
Rate `= k[H_(2)O_(2)] [I^(ɵ) ]`

Text Solution

Verified by Experts

1. The order of the reaction with respect to `[HCrO_(4)^(–)]` is 1, with respect to `[I^(-)]` is 2 and with respect to `[H^(+)]` is 2. The overall order of the reaction is 1 + 2 + 2 = 5
2. The order of the reaction with respect to `[H_(2)O_(2)]` is 1 and with respect to `[I^(–)]` is 1. The overall order of the reaction is 1 + 1= 2.
Promotional Banner

Topper's Solved these Questions

  • Chemical Kinetics

    MOTION|Exercise SOLVED EXAMPLE (OBJECTIVE)|10 Videos

  • Chemical Kinetics

    MOTION|Exercise SOLVED EXAMPLE (SUBJECTIVE)|24 Videos

  • CHEMICAL EQUILIBRIUM

    MOTION|Exercise Exercise - 4|20 Videos

  • CLASSROOM PROBLEMS

    MOTION|Exercise Electrochemistry|22 Videos

Similar Questions

Explore conceptually related problems

From the rate laws for the reactions given below, determine the order with respect to each species and the overall order: underset("Rate ="k[H_2O_2][I^(-)])(H_2O_2 + 2I^(-)+ 2H^(+) to I_2+ 2H_2O)

From the rate laws for the reactions given below, determine the order with respect to each species and the overall order: underset("Rate = "k[HCrO_4^(-)][I^(-)]^2[H^(+)]^2)(2HCrO_4^(-) + 6I^(-) + 14 H^(+) to 2Cr^(3+) + 3I_2 + 8H_2O)

The reaction 2H_(2)O_(2) rarr 2H_(2)O+O_(2) is r=k[H_(2)O_(2)]

In the reaction: Cr_(2)O_(7)^(2-) + 14H^(o+) + 6I^(Ө) rarr2Cr^(3+) + 3H_(2)O + 3I_(2) Which element is reduced?

From the rate expression for the following reactions determines the order of reaction and the dimensions of the rate constant. a) 3NO(g) to N_(2)O(g) + NO_(2)(g) , Rate =k[NO]^(2) b) H_(2)O_(2)(aq) + 3I^(-)(aq) + 2H^(+)(aq) to 2H_(2)O(l) + I_(3)^(-) , Rate = [H_(2)O_(2)][I^(-)] c) CH_(3)CHO(g) to CH_(4)(g) + CO(g) : Rate = k[CH_(3)CHO]^(3//2) d) CHCl_(3)(g) to Cl_(4)(g) + HCl(g) : Rate = k[CHCl_(3)][Cl_(2)]^(1//2) e) C_(2)H_(5)Cl(g) to C_(2)H_(4)(g) + HCl(g) , Rate = k[C_(2)H_(5)Cl]

For each of the following reactions, express the given rate of change of concentration of the reactants or Products in that reaction: a. H_(2)O_(2) + 2H^(o+) + 3l^(ɵ) rarr I_(3)^(ɵ) + 2H_(2)O , (-d[I^(ɵ)])/(d t) = ? , (-d[H^(o+)])/(d t) ? (b) 16H^(o+) + 2Mn_(4)^(ɵ) + 101^(ɵ) rarr 2Mn^(2+) + 8H_(2)O + 5I_(2) , (-d[MNO_(4)^(ɵ)])/(d t) = ? ( c) 4NH_(3) + 5O_(2) rarr 4NO_(2) + 6H_(2)O , (-d[NH_(3)])/(d t) = ?

Which is the correct order of size ? (O^(ɵ), O^(2-), F^(ɵ) and F )

From the rater expression for the following reactions, determine their order of reaction and dimensions of the rate constants. a. 3NO(g) rarr N_(2)O(g), Rate =k[NO]^(2) b. H_(2)O_(2)(aq)+3I^(c-)(aq)+2H^(o+) rarr 2H_(2)O(l)+I_(3)^(c-), Rate =k[H_(2)O_(2)][I^(c-)] c. CH_(3)CHO(g)rarr CH_(4)(g)+CO(g), Rate =k[CH_(3)CHO]^(3//2) d. C_(2)H_(5)Cl(g) rarr C_(2)H_(4)(g)+HCl(g), Rate k[C_(2)H_(5)Cl]