Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2)

Question

Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2) by reaction in the gas phase. The following pressure data were obtained when a sample containing 5.00 x 10^-2 mol sulfuryl chloride were heated to 600 K a 5.00 x 10^-1 L container Defining the rate as Delta[SO2Cl2]/deltat a) Determine the value of the rate constant in the decomposition of sulfuryl chloride at 600 K b) What is the half-life of the reaction? c) What fraction of the sulfuryl chloride remains after 20.0 h?

Explanation / Answer

Plotting the graph with ln[SO2Cl2] with respect to temperature, we get a straight line.so, this is a first order reaction.

(a) so, the rate equation is

lnA = ln Ao - kt

ln4.24 = ln4.93 - k (1 x 60 min x 60 sec)

k = 4.18E-5sec-1

(b) Half life t1/2 = 0.693/k = 0.693/4.18E-5 = 16546sec = 4.6 hours

(c) 20 hours = 20 x 60 x 60 = 72000sec

ln A = ln 4.93 - (4.18E-5)(72000) = -1.414

A = 0.243atm

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