The Reaction `SO_2Cl_2 to SO_2 + Cl_2`, is a first order reaction with `k = 2.2 xx10^-5s^-1` at `320^@C`. Calculate the percentage of `SO_2Cl_2` that is decomposed on heating this gas for 30 minutes.

Write the reactions of F_(2) and Cl_(2) with water.

A first order reaction takes 30 minutes for 50% completion. Calculate the time required for 90% completion of this reaction . (log2=0.3010)

Calculate the amount of Cl_(2) produced by reaction between 1 g of each of MnO_(2) and HCl .

The following data were obtained during the first thermal decomposition of SO_2Cl_2 at a constant volume, SO_2Cl_2(g) to SO_2 (g)+Cl_2 (g) Experiment Time/s Total pressure/ atm 1 0 0.5 2 100 0.6 Calculate the rate of the reaction when total pressure is 0.65 atm.

The decomposition of gaseous Cl_(2)O_(7) to gaseous Cl_(2) and O_(2) at 400K is a first order reaction . After 55 s , the pressure of Cl_(2)O_(7) falls from 0.062 to 0.044 atm . Calculate the pressure of Cl_(2)O_(7) after 100s.

The initial rate of a first order reaction is 5.2 xx 10^(-6)" mol.lit"^(-1).s^(-1) at 298 K. When the initial concentration of reactant is 2.6xx10^(-3)" mol.lit"^(-1) , calculate the first order rate constant of the reaction at the same temperature.

Give the reactions of Cl_2 and CH_4 in presence of diffused sunlight.

For the reaction, SO_2(g) + 1/2 O_2(g) iff SO_3(g) , the value of K_c is 1.7 xx 10^(12) at 300K. Calculate the equilibrium constants for the following reactions at 300K : 2SO_2(g) + O_2(g) iff 2SO_3(g) and SO_3(g) iff SO_2(g) + 1/2O_2(g)

Time required to decompose SO_(2)Cl_(2) to half of its initial amount is 60minutes . If decomposition is a first order reaction, calculate rate constant of the reaction.

The decomposition of gaseous Cl_(2)O_(7) to gaseous Cl_(2) and O_(2) at 400K is a first order reaction . After 55 s , the pressure of Cl_(2)O_(7) falls from 0.062 to 0.044 atm . Calculate the rate constant