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bSulfuryl chloride undergoes first-order decomposition at 320.°C with a half-life of 8.75 h (k = 2.20 x 10-5 s-1). So,Cl2(g) SO2(g) + Cl2(g) If the initial pressure of SO2CI2 is 791 torr and the decomposition occurs in a 1.25-L container, how many molecules of So,Cl, remain after 11.7 h? molecules SO2CI2

bSulfuryl chloride undergoes first-order decomposition at 320.°C with a half-life of 8.75 h (k = 2.20 x 10-5 s-1). So,Cl2(g) SO2(g) + Cl2(g) If the initial pressure of SO2CI2 is 791 torr and the decomposition occurs in a 1.25-L container, how many molecules of So,Cl, remain after 11.7 h? molecules SO2CI2

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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b Sulfuryl chloride undergoes first-order decomposition at 320.°C with a half-life of 8.75 h (k = 2.20 x 10-5 s1). So,Cl2(g) → SO2(g) + Cl2(g) If the initial pressure of S02CI2 is 791 torr and the decomposition occurs in a 1.25-L container, how many molecules of SO2CI, remain after 11.7 h? molecules SO2CI2
Transcribed Image Text:b Sulfuryl chloride undergoes first-order decomposition at 320.°C with a half-life of 8.75 h (k = 2.20 x 10-5 s1). So,Cl2(g) → SO2(g) + Cl2(g) If the initial pressure of S02CI2 is 791 torr and the decomposition occurs in a 1.25-L container, how many molecules of SO2CI, remain after 11.7 h? molecules SO2CI2
Expert Solution
Step 1

The given data is as follows:

The half life of the reaction = 8.75 h

The rate constant of the first order reaction (K) = 2.20×10-5  s-1

The initial pressure of SOCl2 = 791 torr

Temperature = 320 °C=320+273=593 K

The volume of the container = 1.25 L

The number of molecules after time 11.7 h = ?     

 

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