The isomerization reaction CH3NC (g) <---> CH3CN (g) obeys the first order rate law. At 500K, the concentration of CH3NC is 85% of its original value after 247s. What is the rate constant for this decomposition at 500K? At what time will the concentration of CH3NC be 25℅ of its original value?
for the first order reaction we know that
where Ca = Concentration at any time t
Cao = intial concentration
K = rate constant
t = time
according to the problem Ca = 0.85 Cao at t=247s
therefore putting the values we get,
therefore value of K = sec-1
for the next part..
given that Ca = 0.25 Cao
therefore again using the formula
we get
therefore t= 2110.037 sec
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