`|{:([A],[B],"Initial Rate"),(0.05,0.05,0.045),(0.10,0.05,0.09),(0.20,0.10,0.72):}|` for `2A+BtoC`. Find the rate law

For the reaction 2A+BrarrC , the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is : {:([A]("mol"L^(-1)),[B]("mol"L^(-1)),{:("Initial Rate"),("mol"^(-1)s^(-1)):}),(0.05,0.05,0.045),(0.10,0.05,0.090),(0.20,0.10,0.72):}

The data for the reaction: A + B overset(k)rarr C . |{:("Experiment",[A]_(0),[B]_(0),"Initial rate"),(1,0.012,0.035,0.10),(2,0.024,0.070,0.80),(3,0.024,0.035,0.10),(4,0.012,0.070,0.80):}| The rate law corresponding to the above data is (a) Rate = k[B]^(3) , (b) Rate = k[B]^(4) ( c) Rate = k[A][B]^(3) , (d) Rate = k[A]^(2)[B]^(2)

Evaluate: 0.05 xx 505.050

Select the rate law that corresponds to the datashown for the reaction A+BtoC {:(,Exp.,[A],[B],Rate),(,1,0.012,0.035,0.10),(,2,0.024,0.070,0.80),(,3,0.024,0.035,0.10),(,4,0.012,0.070,0.80):}

For the hypothetical reaction 2A + B rarr Products following data obtained: |{:("Experiment number","Initial conc of (A)" (mol L^(-1)),"Initial conc of (B)" (mol L^(-1)),"Initial rate mol" L^(-1) s^(-1),),(1,0.10,0.20,3 xx 10^(2),),(2,0.30,0.40,3.6 xx 10^(10^(3)),),(3,0.30,0.80,1.44 xx 10^(4),),(4,0.10,0.40,...,),(5,0.20,0.60,...,),(6,0.30,1.20,...,):}| Find out how the rate of the reaction depends upon the concentration of A and B and fill in the blanks given in the table.

For the reaction A + B to products, the following initial rates were obtained at various given initial concentration {:("S.No.",,"[A]mol/L",,"[B] mol/L",,"Initial rate M/s"),(1.,," "0.1,," "0.1,," "0.05),(2.,," "0.2,," "0.1,," "0.10),(3.,," 0.1",," 0.2",," 0.05"):} Determine the half-life period.

For the given reaction , A+Brarr Products Following data are given : {:("initial conc."(m//L),"initial conc."(m//L),"initial conc."(mL^(-1)S^(-1))),([A]_0,[B]_0,),(0.1,0.1,0.05),(0.2,0.1,0.1),(0.1,0.2,0.05):} calculate the Rate constant

The kinetic date for the given reaction A(g)+2B(g)overset(K)toC(g) is provided in the following table for three experiments at 300 K {:("Ex. No.","[A/M]","[B/M]","Initial rate" (M sec^(-1))),(1.,0.01,0.01,6.930xx10^(-6)),(2.,0.02,0.01,1.386xx10^(-5)),(3.,0.2,0.02,1.386xx10^(-5)):} In another experiment starting swith initial concentration of 0.5 and 1 M respectively for A and B at 300 K, find the rate of reaction after 50 minutes from the starting of edperiment (inM // sec).

(0.3x+0.5)/(0.4x-0.5)=6

The reaction of A_(2) and B_(2) follows the equation A_(2)(g)+B_(2)(g)to2AB(g) The following data were observed {:(,[A_(2)]_(0),[B_(2)]_(0),"Initial rate of appearance of AB(g)(in" Ms^(-1)),(,0.10,0.10,2.5xx10^(-4)),(,0.20,0.10,5xx10^(-4)),(,0.20,0.20,10xx10^(-4)):} The value of rate constatnt for the above reaction is :