The following data were obtained during the first order thermal decomposition of {\SO}_2 {\Cl}_2 at a constant volume: {\SO}_2 {\Cl}_2( {\g}) \to {\SO}_2( {\g})+ {\Cl}_2( {\g}) Experiment Time / {s}^{-1} Total pressure/atm 1 0 0.4 2 100 0.7 Calculate the rate constant. (Given: \log 4=0.6021, \log 2=0.3010)

CBSE Class 12 Chemistry 2014 Outside Delhi Set 1 Solved Paper

Question : 20 of 30

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The following data were obtained during the first order thermal decomposition of

{\SO}_2 {\Cl}_2

at a constant volume:

{\SO}_2 {\Cl}_2( {\g}) → {\SO}_2( {\g})+ {\Cl}_2( {\g})

Experiment	Time $/ {s}^{-1}$	Total pressure/atm
1	0	0.4
2	100	0.7

Calculate the rate constant. (Given:

\log 4=0.6021

\log 2=0.3010)

Solution:

{\SO}_2 {\Cl}_2( {\g}) → {\SO}_2( {\g})+ {\Cl}_2( {\g})

\table \At t=0, {\P}^0, {\0}, {\0} ;\At t=100 {\sec} ,{\P}^0- {\P}, {\P},{\P}

{\P}^0\;=0.4 {\atm}

{\P}^0- {\P}+ {\P}+ {\P}\;=0.7 {\atm}

{\P}^0+ {\P}\;=0.7 {\atm}

{\P}\;=0.3 {\atm}

It's a first order reaction.

\; {\K}=\;{2.303}/{t} \log \;{P^0}/{P^0-P}

\; {\K}=\;{2.303}/{t} \log \;{0.4}/{0.1}

So, the rate constant,

{\K}=1.39 × 10^{-2} {\ sec}^{-1}

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