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?© BrainMass Inc. brainmass.com March 4, 2021, 6:19 pm ad1c9bdddf
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 ...
The solution provides a step-by-step explanation to answer the question regarding the first order reaction.