SO2Cl2- SO2-Cl2 is a first order gas reaction with k-2-2- 10-5-1 at 320o C- The percentage of SO2Cl2 decomposed on heating for 90 minutes is-

Time required to decompose $S O_{2} C L_{2}$ to half of its
initial amount is 60 minutes . If the decompose is a first order reaction,
calculate the rate constant of the
reaction.

Time required to decompose SO₂Cl₂ to half of its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.

Q. The reaction,

S O_{2} (g) + C l_{2} (g) ⇋ S O_{2} C l_{2} (l)

is exothermic. A mixture of

S O_{2}, C l_{2}

and

S O_{2} C l_{2}

is at equilibrium in a closed container. Now, a certain amount of

S O_{2}

is added to the mixture, the volume remaining the same. Which of the following statement is true?

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SO2Cl2→SO2+Cl2 is a first order gas reaction with k=2.2×10−5sec−1 at 320oC. The percentage of SO2Cl2 decomposed on heating for 90 minutes is:

The correct option is D 11.18For a first order reaction,k=ln[RoR]tln[RoR]=2.2×10−5×90×60lnRoR=0.1188RoR=1.126R=0.8879RoPercentage of decomposition = R0−R ⇒Ro−0.8879 Ro⇒11.18 Ro % Hence, option D is correct.

$S O_{2} C l_{2} \to S O_{2} + C l_{2}$ is a first order gas reaction with $k = 2.2 \times 10^{- 5} {sec}^{- 1}$ at $320^{o} C$ . The percentage of $S O_{2} C l_{2}$ decomposed on heating for 90 minutes is: