Dinitrogen pentoxide, N2O5, decomposes when heated in carbon tetrachloride solvent.N2O5 →2NO2 + 1/2 O2(g) If the rate constant for the decomposition of N2O5 is 6.2 x10-4/min, what is the half-life? (The rate law is first order in N2O5.)(a) How long would it take for the concentration of N2O5 to decrease to 25% of its initial value? (b) To 12.5% of its initial value?
Dinitrogen pentoxide, N2O5, decomposes when heated in carbon tetrachloride solvent.N2O5 →2NO2 + 1/2 O2(g)
If the rate constant for the decomposition of N2O5 is 6.2 x10-4/min, what is the half-life? (The rate law is first order in N2O5.)(a) How long would it take for the concentration of N2O5 to decrease to 25% of its initial value? (b) To 12.5% of its initial value?
Given reaction is
N2O5 → 2NO2 + 1/2 O2(g)
rate law
rate [N2O5]1
rate =K [N2O5]1
where
K = rate constant = 6.2 x10-4/min
first order rate constant :
K = (2.303/t) log a /(a-x)
k = rate constant, t = time taken,
a = initial concentration of N2O5 =100 , x = percentage completed , (a-x) = remaining percentage
t1/2 and K relation :
t1/2 = 0.693/K
= 0.693 / 6.2 x10-4 min-1
= 0.11177 x 104 min
= 1117.7 min
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