SO2CL2 decomposes by first-order kinetics, and k=2.91x10^-3 min^-1 at a particular temperature. Determine the half life for the reaction.

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Nelly StrackeLv2

17 Dec 2019

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SO2Cl2 decomposes in a first-order process with a half-life of 4.88 Ã 103 s. If the original concentration of SO2Cl2 is 0.062 M, how many seconds will it take for the SO2Cl2 to reach 0.0064 M?

When 2.00 mol of SO₂Cl₂ is placed in a 2.00-L flask at 303 K, 56% of the SO₂Cl₂ decomposes to SO₂ and Cl₂:

SO₂Cl₂(g) SO₂(g) + Cl₂(g)

(a) Calculate K_c for this reaction at this temperature. (b) Calculate K_p for this reaction at 303 K. (c) According to Le Châtelier’s principle, would the percent of SO₂Cl₂ that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel? (d) Use the equilibrium constant you calculated above to determine the percentage of SO₂Cl₂ that decomposes when 2.00 mol of SO₂Cl₂ is placed in a 15.00-L vessel at 303 K.

redant521

SO₂Cl₂ decomposes by a first order reaction with a rate constant of 7.92x10^-2 hr^-1 at 320⁰C. How long will it take for 90% of the SO₂Cl₂ intially present in a sample to decompose at this temperature? Answer is 29.1 hr please show your work.

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SO2CL2 decomposes by first-order kinetics, and k=2.91x10^-3 min^-1 at a particular temperature. Determine the half life for the reaction.

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