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For the chemical reaction I^(ɵ) + OCl^...

For the chemical reaction
`I^(ɵ) + OCl^(ɵ) rarr Cl^(ɵ) + OI^(ɵ)`
Rate `= (k[OCl^(ɵ)] [I^(ɵ)])/([overset(ɵ)(OH)]`
What is the order and molecularity of the reaction ?

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To determine the order and molecularity of the given chemical reaction: **Step 1: Write down the given reaction and rate expression.** - The reaction is: \[ I^{\circ} + OCl^{\circ} \rightarrow Cl^{\circ} + OI^{\circ} \] - The rate expression is: ...
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For the chemical reaction I^(ɵ) + OCl^(ɵ) rarr Cl^(ɵ) + OI^(ɵ) Rate = (k[OCl^(ɵ)] [I^(ɵ)])/([overset(ɵ)(OH)] a. What is the order and moleculartiy of the reaction ? b. In the above reaction, what are the molecularity and order with respect to [overset(ɵ)(OH)]

For the chemical reaction: 5Br^(ɵ) + BrO_(3)^(ɵ) + 6H^(o+) rarr 3Br_(2) + 3H_(2)O Rate = k[Br^(ɵ)] [BrO_(3)^(ɵ)] [H^(o+)] What is the molecularity and order of reaction with respect to [Br^(ɵ)] ?

The order of reaction is an experimentally determined quanity. It may be zero, poistive, negative, or fractional. The kinetic equation of nth order reaction is k xx t = (1)/((n-1))[(1)/((a-x)^(n-1)) - (1)/(a^(n-1))] …(i) Half life of nth order reaction depends on the initial concentration according to the following relation: t_(1//2) prop (1)/(a^(n-1)) ...(ii) The unit of the rate constant varies with the order but general relation for the unit of nth order reaction is Units of k = [(1)/(Conc)]^(n-1) xx "Time"^(-1) ...(iii) The differential rate law for nth order reaction may be given as: (dx)/(dt) = k[A]^(n) ...(iv) where A denotes the reactant. For a reaction: I^(ɵ) + OCl^(ɵ) rarr IO^(ɵ) + Cl^(ɵ) in an aqueous medium, the rate of the reaction is given by (d[IO^(ɵ)])/(dt) = k([I^(ɵ)][OCl^(ɵ)])/([overset(ɵ)(OH)]) The overall order of the reaction is

The experiment rate law for the reaction S_(2)O_(8)^(2-)(aq) + 2I^(ɵ)(aq) rarr 2SO_(4)^(2-) (aq) + I_(2)(aq) is k[S_(2)O_(8)^(2-)] [I^(ɵ)] . How would the rate change if (a) Concentration of S_(2)O_(8)^(2-) is halved. (b) Concentration of S_(2)O_(8)^(2-) and I^(ɵ) are halved.

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For the reaction, 2NOCl(g) hArr 2NO(g)+Cl_(2)(g) Calculate the standard equilibrium constant at 298 K . Given that the value of DeltaH^(ɵ) and DeltaS^(ɵ) of the reaction at 298 K are 77.2 kJ mol^(-1) and 122 J K^(-1) mol^(-1) .

For the cell reaction: 2Fe^(3+)(aq)+2l^(-)(aq)to2Fe^(2+)(aq)+l_(2)(aq) E_(cell)^(ɵ)=0.24V at 298K . The standard gibbs energy (triangle,G^(ɵ)) of the cell reaction is [Given that faraday constnat F=96500Cmol^(-1)]

The reaction S_(2)O_(8)^(2-) + 3I^(ɵ) rarr 2SO_(4)^(2-) + I_(3)^(ɵ) is of first order both with respect to persulphate and iofide ions. Taking the initial concentration as a and b , respectively, and taking x as the concentration of the triofide at time t , a differential rate equation can be written. Two suggested mechanism for the reaction are: I. S_(2)O_(8)^(2-)+I^(ɵ) hArr SO_(4)I^(ɵ)+SO_(4)^(2-) ("fast") I^(ɵ)+SO_(4)I^(ɵ) overset(k_(1))rarrI_(2) + SO_(4)^(2-) (show) I^(ɵ) + I_(2) overset(k_(2))rarr I_(3)^(ɵ) ("fast") II. S_(2)O_(8)^(2-) + I^(ɵ) overset(k_(1))rarr S_(2)O_(8) I^(2-) (slow) S_(2)O_(8)I^(3-) overset(k_(2))rarr2SO_(4)^(2-)+I^(o+) ("fast") I^(o+) + I^(ɵ) overset(k_(3)) rarr I_(2) ("fast") I_(2) + I^(o+) overset(k_(4))rarr I_(3)^(ɵ) ("fast") The general difference equation for the above reaction is

Why does the chromyl chloride test fail with Br^(ɵ) and I^(ɵ) ?

CENGAGE CHEMISTRY ENGLISH-CHEMICAL KINETICS-Archives Subjective
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