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Nitrogen pentoxide decomposes according to equation : 2N_(2)O_(5)(g) rarr 4NO_(2)(g) + O_(2)(g). This first order reaction was allowed to proceed at 40^(@)C and the data below were collected : (a) Calculate the rate constant. Include units with your answer. (b) What will be the concentration of N_(2)O_(5) after 100 minutes ? (c ) Calculate the initial rate of reaction ? |
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Answer» Solution :(a) `K = (2.303)/(t)log.(A_(0))/([A])` `k = (2.303)/(20 min)log.(0.400)/(0.289)` `k = 0.0163 min^(-1)` (b) `k = (2.303)/(t)log.(A_(0))/([A])` `=0.0163 - (2.303)/(100)log.(0.400)/([A])` `[A] = 0.078 M` (C ) Initial rate R `= k[N_(2)O_(5)]` `= 0.0163 min^(-1) xx (0.400 M)` `=0.00652 M min^(-1)` |
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