In a reaction, 2 N _2 O _ 5(g) 4\, NO _ 2(g) + O _ 2(g) N _2 O _5 disappears at a rate of 0.06 mol dm^ -3 s^ -1 Calculate rate of formation of O _ 2(g) ?

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Correct answer: B. 0.03 mol dm^ -3 s^ -1

For the given reaction 2 N _2 O _ 5(g) 4 NO _ 2(g) + O _ 2(g) The rate of reaction is given by: Rate = - 1 2 d[ N _2 O _5] dt = 1 4 d[ NO _2] dt = d[ O _2] dt Given the rate of disappearance of N _2 O _5 is - d[ N _2 O _5] dt = 0.06 mol dm ^ -3 s ^ -1 The rate of formation of O _2 is: d[ O _2] dt = 1 2 (- d[ N _2 O _5] dt ) d[ O _2] dt = 1 2 0.06 = 0.03 mol dm ^ -3 s ^ -1

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