Problem: 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 was heated to 600. K in a 5.00 x 10 -1-L container.Defining the rate as - Δ [SO2Cl2] / Δt,a. determine the value of the rate constant for the decomposition of sulfuryl chloride at 600. K.

🤓 Based on our data, we think this question is relevant for Professor Davidson's class at WEBER.

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FREE Expert Solution

We're being asked to calculate for the rate constant for the decomposition of sulfuryl chloride at 600 K.


 We don't know the order of the reaction. We will assume that the reaction is an elementary reaction which means that the given reaction is the slow step.

▪ the coefficients of the reactants in the slow step are the order of the reaction with respect to that reactant


Given reaction: Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2) by a reaction in the gas phase

SO2Cl2(g) → SO2(g) + Cl2(g)

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Problem Details

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 was heated to 600. K in a 5.00 x 10 -1-L container.

Defining the rate as - Δ [SO2Cl2] / Δt,
a. determine the value of the rate constant for the decomposition of sulfuryl chloride at 600. K.

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

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.