The rate of the reaction , `ArarrB` , is expressed by `-(d[A])/(dt)` . What does the (-) sign imply ?

ArarrB , Rate of this reaction is expressed by -(d[A])/(dt) " or "+(d[B])/(dt) . What is the significance of (-) sign and (+) sign in this case ?

In the reaction ArarrB , if the change in concentration of A in the time interval Deltat " is " Delta[A] , then the rate of reaction is -(Delta[A])/(Deltat) . What is the significance of the 'negative ' sign in the expression -(Delta[A])/(Deltat) ?

The reaction -rate of the reaction AB_(3)rarr(1)/(2)A_(2)+(3)/(2)B2 can be expressed by any one of the following equations : (-d[AB_(3)])/(dt)=k_(1)[AB_(3)], (d[A_(2)])/(dt)=k_(2)[AB_(3)] " or, " (d[B_(2)])/(dt)=k_(3)[AB_(3)] The ratio between k_(1) , k_(2)and k_(3) is -

The decomposition of H_(2)O_(2) is a first order reaction . The rate constant of the reaction can be expressed as logk=14.34-(1.25xx10^(4))/(T) . Calculate the activation energy of the reaction . At what temperature does the half-life of the reaction become 265min?

In the reaction 3A to 2B , rate of reaction +('d(B)')/(dt) is equal to

The rate of change of concentration of (A) for reaction: A rarr B is given by (-d[A])/dt=k[A]^1/3 The half-life period of the reaction will be:

The order of a reaction is 3/2. If concentration is expressed in mol... and time in "mol.L"^(-1) and in 's' , then the unit of rate constant of the reaction would be ………….

Rate law for the reaction A + B to product is rate= k[A]^2{B] . What is the rate constant, if rate of reaction at a given temperature is 0.22 Ms^-1, when [A] =1M and (B]= 0.25 M?

The rate constant of the reaction ArarrB is 6.932xx10^(-3)"min"^(-1) . If initial concentration of A is 1(M) , then , the rate of the reaction ( in mol.L^(-1)."min"^(-1)) after 100 min will be -

The half -life of a first order reaction ArarrB is 10 min . What fraction of the reactant will be left behind after 1 h ?