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The decomposition reaction 2N2O5g→Δ2N2O4g+O2g is started in a closed cylinder under isothermal isochoric condition at an initial pressure of 1 atm..After Y×103s the pressure inside the cylinder is found to be 1.45 atm. If the rate constant of the reaction is 5×10−4s−1 , assuming ideal gas behavior, the value of Y is __

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answer is 2.30.

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Detailed Solution

2N2O5 g→Δ2N2O4 g+O2 gGiven rate constant of the reaction = 5×10−4sec−1 12dPN2O5dt=Koverall PN2O5⇒dpN2O5dt=2KoverallPN2O5 2N2O5(g) →2N2O4(g) + O2 (g) 1-x x x/2 1+x2=1.45x=0.90 atmy×10−3=2.3032×5×10−4log10.1y=23.0310=2.30

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