Problem: The gas-phase decomposition of SO2Cl2, SO2Cl2(g) → SO2 (g) + Cl2 (g), is first order in SO2Cl2. At 600 K the half-life for this process is 2.3 x 105 s.At 320 oC the rate constant is 2.2 x 10 - 5 s- 1. What is the half-life at this temperature?

FREE Expert Solution

We're being asked to determine the half-life of the reaction at 320°C. We’re given the following first-order reaction:

SO2Cl2(g) → SO2 (g) + Cl2 (g)


Recall that half-life is the time needed for the amount of a reactant to decrease by 50% or one-half

The half-life of a first-order reaction is given by:

t12=ln 2k


We're given:

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Problem Details

The gas-phase decomposition of SO2Cl2, SO2Cl2(g) → SO2 (g) + Cl2 (g), is first order in SO2Cl2. At 600 K the half-life for this process is 2.3 x 105 s.

At 320 oC the rate constant is 2.2 x 10 - 5 s- 1. What is the half-life at this temperature?

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Our tutors have indicated that to solve this problem you will need to apply the Integrated Rate Law concept. You can view video lessons to learn Integrated Rate Law Or if you need more Integrated Rate Law practice, you can also practice Integrated Rate Law practice problems .

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Based on our data, we think this problem is relevant for Professor Poler's class at UNC.