The decomposition of sulfuryl chloride into sulfur dioxide and chlorine SO2Cl2(g) → SO2(g) + Cl2(g) follows first-order kinetics. At 320◦C the rate constant is 2.2 × 10−5 sec−1 . If one started with a sample containing 0.16 moles of sulfuryl chloride per liter at 320◦C, what concentration would be left after 6.00 hours?

The concentration of sulfuryl chloride left is 0.0995 M

Explanation:

For the given chemical equation:

Rate law expression for first order kinetics is given by the equation:

where,

k = rate constant  =

t = time taken for decay process = 6.00 hours = (6 × 3600) = 21600 s    (Conversion factor:  1 hr = 3600 seconds)

= initial amount of the sample = 0.16 moles

[A] = amount left after decay process =  ?

Putting values in above equation, we get:

Molarity is calculated by using the equation:

Moles of sulfuryl chloride left = 0.0995 moles

Volume of solution = 1 L

Hence, the concentration of sulfuryl chloride left is 0.0995 M

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