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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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#### 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 ...

#### Solution Summary

The solution provides a step-by-step explanation to answer the question regarding the first order reaction.

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