For the decomposition of azoisopropane to hexane and nitrogen at 543 K, the following data are obtained. At o sec P (mm of Hg) is 35 at 360 sec P is 54 at 720 sec P is 63 Calculate the rate constant.

For the decomposition of azoisopropane to hexane and nitrogen at 543 K, the following data is obtained. Calculate the rate constant.

The decomposition of N_2O_5 according to the equation, 2N_2O_5(g) harr 4NO_2(g) + O_2(g) is a first order reaction. After 30 min from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 mm of Hg and on complete decomposition, the total pressure is 584.5 mm of Hg. Calculate the rate constant of the reaction.

The following results were obtained for the decomposition of nitrogen peroxide in an inert solvent : Show that the reaction is of first order and also calculate the rate constant.

The decomposition of phosphine, PH_3 , proceeds according to the following equation : 4PH_3 (g) rarr P_4 (g) + 6H_2 (g) It is found that the reaction follows the following rate equation : Rate = k[PH_3] . The half-life of PH_3 is 37.9 s at 120^@ C. How much time is required for 3/4th of PH_3 to decompose?

The integrated rate equations can be fitted with kinetic data to determine the order of a reaction. The integrated rate equations for zero, first and second order reactions are : Zero order : [Al =-kt+ [A]_0 First order : log [A] = -(kt)/2.303 + log [A]_0 Second order : 1/([A])=kt+1/[A]_0 These equations can also be used to calculate the halt life periods of different reactions, which give the time during which the concentration of a reactant is reduced to half of its initial concentration, i.e, at time t_(1//2), [A] = [A]_0//2 Answer the following (1 to 5) question : The decomposition of nitrogen pentoxide : 2N_2O_5(g) rarr 4NO_2(g) + O_2(g) is a first order reaction. The plot of log [N_2O_5] vs time (min) has slope = - 0.01389. The rate constant k is

The decomposition of dimethyl ether leads to the formation of CH_4, H_2 and CO and the reaction rate is given by Rate = k [CH_3OCH_3]^(3/2) . The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e., Rate= k (P_(CH_3OCH_3 )^(3/2) If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?

The rate constant for the first order decomposition of H_2O_2 is given by the following equation: log k = 14.34 - 1.25 × 10^4K/T Calculate E_a for this reaction and at what temperature will its half-period be 256 minutes?

The following data were obtained during the first order thermal decomposition of SO_2Cl_2 at a constant volume : SO_2Cl_2 (g) rarr SO_2(g)+ Cl_2(g) Calculate the rate constant. (Given : log 4 = 0.6021, log 2 = 0.3010)