The rate of a reaction is given as, rate =k[X]^(3//2)[Y]^(-1//2) . What is the order of the reaction ? If Y is taken large in excess, write the rate equation.

The rate of a reaction is given as , rate = k[X]^(3//2) [Y]^(-1//2) What is the order of the reaction ? If Y is taken large in excess , write the rate equation.

For a reaction, A +B to Product : the rate law is given by r =k [A]^(1//2)[B]^(2) What is the order of the reaction ?

The rate equation for the reaction 2A+BtoC is found to be : rate =K[A][B]. The correct statement in relation to this reaction is

If the rate for the chemical reaction is expresssed at Rate =K[A][B]" then

For a reaction, A +B to Product : the rate law is given by r =k [A]^(1//2)[B]^(2) What is the order of the reaction ?

The instantaneous rate of an elementary chamical reactkon aA+bBhArr cC+dD can be given by rate =K_(f)[A]^(a)[B]^(b)-K_(b)[C]^(c)[D]^(d) where K_(f) and K_(b) are rate constants for forward and backward reactions respectively for the reversible reaction. If the reaction is an irreversible one, the rate is expressed as, rate =K[A]^(a)[B]^(b) where K is rate contant for the given irreversible rate of disappearance of A is a/b times the rate of disappearance of B. The variation of rate constant K with temperature is expressed in terms of Arrhenius equation: K=Ae^(-E_(a)//RT) whereas the ratio (K_(f))/(K_(b)) is expressed in terms of van't Hoff isochore: (K_(f))/(K_(b))=Ae^(-DeltaH//RT) , where E_(a) and DeltaH are energy of activation and heat of reaction respectively. For a gaseous phase -I order reaction A(g)toB(g)+2C(g) (rate constant K=10^(-2)"time"^(-1) ) in a closed vesel of 2 litre containing 5 mole of A(g) at 27^(@)C which of the following is correct?