Radium decomposes at a rate proportional to the quantity of radium present. It is found that in 25 years, aproximately 1.1% of a certain quantity of radium has decomposed. Determine approximately how long will it take for half of the original amount to decompose?
(given `log_e(.989)=-0.01106` and `log_e 2=0.6931)`

Experiments show that radium decomposes at a rate proportioanl to the amount of radium present at the moment. If its half life is 1570 years, what percentage will disappear in one years?

The reaction cis-Xcis-X underset(k_(b))overset(k_(f))ltimplies trans-X is first order in both direction At 25^(@)C, the equilibrium constant is 0.10 and the rate constant k_(f)=3xx10^(-4)s^(-1) In an experiment starting with the pure cis- from , how long would it take for half of the equilibrium amount of the trans-iomer to be fromed?

A country has a food deficit of 10%. Its population grows continuously at the rate of 3% per year. Its annual food production every year is 4% more than that of the last year Assuming that the average food requirement per person remains constant, prove that the country will become self-sufficient in food after n years, where n is the smallest integer bigger than or equal to (log_e 10-log_e 9)/((log_e 1.04)-0.03)

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 gaseous decomposition reaction, A(g)rarr2B(g)+C(g) is observed to first order over the excess of liquid water at 25^(@)C . It is found that after 10 minutes the total pressure of system is 188 torr and after very long time it is 388 torr. The rate constant of the reaction (in hr^(-1)) is : [Given : vapour pressure of H_(2)O at 25^(@) is 28 torr (ln 2=0.7 , ln 3=1.1, ln10=2.3) ] a) 0.02 b) 1.2 c) 0.2 d) none of these

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, rate at a particular time is x. if the initial concentration is tripled, the rate will become

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 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

Radioactive disintegration is a first order reaction and its rate depends only upon the nature of nucleus and does not depend upon external factors like temperature and pressure. The rate of radioactive disintegration (Activity) is represented as -(dN)/(dt)=lambdaN Where lambda= decay constant, N= number of nuclei at time t, N_(0) =initial no. of nuclei. The above equation after integration can be represented as lambda=(2.303)/(t)log((N_(0))/(N)) Half-life period of U is 2.5xx10^(5) years. In how much time will the amount of U^(237) remaining be only 25% of the original amount ? a) 2.5xx10^(5) year b) 1.25xx10^(5) years c) 5xx10^(5) years d) none of these

Radioactive disintegration is a first order reaction and its rate depends only upon the nature of nucleus and does not depend upon external factors like temperature and pressure. The rate of radioactive disintegration (Activity) is represented as -(dN)/(dt)=lambdaN Where lambda= decay constant, N= number of nuclei at time t, N_(0) =intial no. of nuclei. The above equation after integration can be represented as lambda=(2.303)/(t)log((N_(0))/(N)) Calculate the half-life period of a radioactive element which remains only 1//16 of its original amount in 4740 years: a) 1185 years b) 2370 years c) 52.5 years d) none of these