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(b)A 36.8 g sample of N2O4 was heated in a closed flask of volume 16.0 dm3. An equilibrium was established at a constant temperature according to the following equation.

N2O4(g) 2NO2(g)

The equilibrium mixture was found to contain 0.180 mol of N2O4

(i)Calculate the number of moles of N2O4 in the 36.8 g sample.

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(ii)Calculate the number of moles of NO2 in the equilibrium mixture.

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(iii)Write an expression for Kc and calculate its value under these conditions.

Expression for Kc .............................................................................................

...........................................................................................................................

Calculation .......................................................................................................

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...........................................................................................................................

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(iv)Another 36.8 g sample of N2O4 was heated to the same temperature as in the original experiment, but in a larger flask. State the effect, if any, of this change on the position of equilibrium and on the value of Kc compared with the original experiment.

Effect on the position of equilibrium .................................................................

Effect on the value of Kc ....................................................................................

(9)

(Total 12 marks)

3

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