The isotope Manganese-56 decays and udergoes `beta-` particle eission to form the stable isotope Iron-56 .The half life for this decay is 2.6 hours .Initially,at time t=0,a sample of Manganese-56 has a mass of `1.4muG` and there is no iron - 56.
Determine the time at which the ratio is equal to 9.0.

The isotope Manganese-56 decays and udergoes beta- particle eission to form the stable isotope Iron-56 .The half life for this decay is 2.6 hours .Initially,at time t=0,a sample of Manganese-56 has a mass of 1.4muG and there is no iron - 56. For the smple of Manganese-56 ,determine the initial activity.

The isotope Manganese-56 decays and udergoes beta- particle eission to form the stable isotope Iron-56 .The half life for this decay is 2.6 hours .Initially,at time t=0,a sample of Manganese-56 has a mass of 1.4muG and there is no iron - 56. For the smple of Manganese-56 ,determine the initial number of Manganese-56 atoms in the sample an d

The isotope Phosphorus-33 undergoes beta - decay to form Sulphur-33, which is stable.The half - life of Phosphorus-33 is 24.8 days. Show that the decay constant of Phosphorus -33 is 3.23 xx 10^(-7) s^(-1) .

The isotope Phosphorus-33 undergoes beta - decay to form Sulphur-33,which is stable.The half - life of Phosphorus-33 is 24.8 days. A pure sample of Phosphorus - 33 has an initial activity of 3.7 xx 10^6 Bq. Calculate the initial number of Phosphorus - 33 nuclei in the sample,

Strontium-90 is a radioactive isotope having a half-life of 28 years.Strontium-90 has a denstiy f 2.5 g cm^(-3) .A smaple of Strontium-90 has an activity of 6.4 xx 10^9 Bq .Calculate the mass of stronitium 90 in the sample

The isotope Phosphorus-33 (_(15)P^(33)) undergoes beta - decay to form "Sulphur"-33(_(16)S^(33)) ,which is stable.The half - life of Phosphorus-33 is 24.8 days. A pure sample of Phosphorus - 33 has an initial activity of 3.7 xx 10^6 Bq.Calculate the number of Phophorus - 33 nuclei remaining in the sample after 30 days.

Strontium-90 is a radioactive isotope having a half-life of 28 years.Strontium-90 has a denstiy f 2.5 g cm^(-3) .A smaple of Strontium-90 has an activity of 6.4 xx 10^9 Bq .Calculate the volume of the sample.

A radioactive nucleus X decays to a nucleus Y with a decay constant lambda_X=0.1s^-1, Y further decays to a stable nucleus Z with a decay constant lambda_Y=1//30s^-1 . Initially, there are only X nuclei and their number is N _0=10^20 . Set up the rate equations for the populations of X, Y and Z. The population of Y nucleus as a function of time is given by N_Y(t)={N _0lambda_X//(lambda_X-lambda_Y)}[exp(-lambda_Yt)-exp(-lambda_Xt)]. Find the time at which N_Y is maximum and determine the population X and Z at that instant.

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 : For a second order reaction, the correct plot of t_(1//2) vs. 1//[A]_0 is

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 rate for the first order reaction is 0.0069 mol L^-1 mi n^-1 and the initial concentration is 0.2 mol L^-1 . The half life period is