The first-order reaction, SO_2Cl_2 rightarrow SO_2 + Cl_2, has a rate constant e

Question

The first-order reaction, SO_2Cl_2 rightarrow SO_2 + Cl_2, has a rate constant equal to 2.20 times 10^-5 s^-1 at 593 K. What percentage of the initial amount of SO_2Cl_2, will remain after 4.50 hours? 1.00% 99.9% 49.0% 85.4% The isomerization reaction, CH_3NC rightarrow CH_3CN, is first order and the rate constant is equal to 0.46 s^-1 at 600 K. What is the concentration of CH_3NC after 0.20 minutes if the initial concentration is 0.30 M? 1.1 times 10^-3 M 2.4 times 10^-3 M 1.1 times 10^-1 M 1.5 times 10^2 M

Explanation / Answer

For 1st order reaction in gas phase

-ln(1-XA)= Kt where XA= conversion

-ln(1-XA)= 2.2*10-5*4.5*60*60 = 0.3564

1-XA= 0.7, XA=0.3,

CA= CAO*(1-XA)/ 1+eXA) e= fractional change in volume for gas phase reaction = 2-1 =1

CA/CAO= (1-0.3)/1.3 = 0.7/1.3 =0.54

For 1st order liquids phase reaction,   CA/CAO= e(-Kt), K= rate constant and t is time in seconds ( since K is given in seconds), CA/CAO= concentration at any time and CAO= initial concentration

CA/CAO= exp(-4.5*60*60* 2.2*10-5) =0.7

CA= 70% of Initial concentration ( No answer is available)

2. CA= 0.3* exp(-0.46*0.2*60) = 0.001202 =1.202*10-3 M (A is correct)

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