Activation energy questions

Assignment: Questions on Topic 16.2: Activation energy

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At a temperature of 700 K the rate constant for the redox reaction between nitrogen(IV) oxide and carbon monoxide is 1.30 mol−1 dm3 s−1.

NO2(g) + CO(g)→ NO(g) + CO2(g) k = 1.30 mol−1 dm3 s−1 at 700 K

i.   Deduce the overall order of this reaction.

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ii.  The activation energy is 133.8 kJ mol−1.
Determine the temperature when the rate constant for the reaction will be 20.0 mol−1 dm3 s−1.

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In the gas phase methyl isocyanide, H3CNC, rearranges to form ethanenitrile, H3CCN.

The table below shows the experimentally determined values of the rate constant for this rearrangement at different temperatures.

i.   Determine the overall order of the reaction.

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ii.  Write the rate expression for the reaction.

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iii.  Using a graphical method, determine the activation energy for the rearrangement of methyl isocyanide.

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iv.  Determine the value of the rate constant for this reaction at (I) 210 oC and (II) 283 oC.

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