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Why in the redox titration of KMnOX4 vs oxalic acid, we heat oxalic acid solution before starting the titration? - Chemistry

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प्रश्न

Why in the redox titration of \[\ce{KMnO4}\] vs oxalic acid, we heat oxalic acid solution before starting the titration?

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उत्तर

The reaction between \[\ce{KMnO4}\] and oxalic acid is very slow. By raising the temperature we can increase the rate of reaction.

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अध्याय 4: Chemical Kinetics - Exercises [पृष्ठ ५६]

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एनसीईआरटी एक्झांप्लर Chemistry [English] Class 12
अध्याय 4 Chemical Kinetics
Exercises | Q III. 49. | पृष्ठ ५६

संबंधित प्रश्न

Explain a graphical method to determine activation energy of a reaction.


The rate constant for the first-order decomposition of H2O2 is given by the following equation:

`logk=14.2-(1.0xx10^4)/TK`

Calculate Ea for this reaction and rate constant k if its half-life period be 200 minutes.

(Given: R = 8.314 JK–1 mol–1)


The rate constant for the decomposition of N2O5 at various temperatures is given below:

T/°C 0 20 40 60 80
105 × k/s−1 0.0787 1.70 25.7 178 2140

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The rate constant for the decomposition of hydrocarbons is 2.418 × 10−5 s−1 at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor?


The decomposition of hydrocarbon follows the equation k = `(4.5 xx 10^11 s^-1) e^(-28000 K//T)`

Calculate Ea.


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Half life period of a reaction (t1/2)

 

 

Consider figure and mark the correct option.


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(i) energy is always released

(ii) energy is always absorbed

(iii) energy does not change

(iv) reactants may be formed


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