The isomerization reaction of cyclopropane to propene at 500 degree C follows fi

Question

The isomerization reaction of cyclopropane to propene at 500 degree C follows first-order kinetics with a ra constant of 6.70 x 10^-4 s^-1. Starting with pure cyclopropane, about how long will it take for 99.0% to convert to propene? The reaction NO2(g)+ CO(g) right arrow NO(g) + CO2(g) appears to be second order in NO and zero order in CO, with a rate constant at 488 K of 0.749 M^-1s^-1. Suppose the initial partial pressure of NO2, in a reaction vessel containing air at STP (1atm, 273 K) is 0.0278 am. How many moles of NO2 are pres per liter after 2.50 minutes?

Explanation / Answer

Hi,

The equation for first order kinetics is

ln([A]t/[A]o) = -K X t

Now, [A]t/[A]o = 1/100 (since 99% has to converted to propene)

K = 6.70 X 10^-4 s-1

substituting in the equation we get

t= ln (0.01)/ - 6.70 X 10^-4

t = -4.605/ - 6.70 X 10^-4

t = 6.8734 X 10^3 s or 114.5 min or 1.91 hour

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