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    First Order Reaction

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    The following first order reaction is conducted in an inert liquid at 45 Celsius:

    N2O5 N2O4 + 1/2 O2

    THE RATE CONSTANT IS K=6.2*10 XY TO -4 SXY -1
    AN 80.0g SAMPLE OF N2O5 IS DISSOLVED IN THE INERT LIQUID AND ALLOWED TO DECOMPOSE AT 45 CELSIUS.

    1- HOW LONG WILL IT TAKE FOR THE QUANTITY OF N2O5 TO BE REDUCED TO 2.5g?

    2- WHAT VOLUME OF O2 (AT 1 ATM PRESSURE AND 25 CELSIUS) IS PRODUCED UP TO THIS POINT?

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    https://brainmass.com/chemistry/chemical-kinetics/first-order-reaction-39910

    Solution Preview

    The half life (t 1/2) for a first order reaction is related to the rate constant by the equation:

    t1/2 x k = ln(2) = 0.693

    It will take five half-lives to get from 80 to 2.5 g (2.5 = 80 * 0.5 * 0.5 * 0.5 * 0.5 * 0.5)

    At 1 atm pressure and 25 Celsius, 1 mole of an ideal ...

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