Consider the chemical reaction 2A + B->2D + E. The reaction has a rate law of the form Rate=k[A]^x[B]^y. The following data was collected for the rate of the reaction at a constant temperature with different concentrations of reactants 'A' and 'B'.

Expt #1 [A]=0.375Mol/L [B]=0.600Mol/L Rate:Mol/(L*s)=19.583

Expt #2 [A]=0.375Mol/L [B]=0.500Mol/L Rate:Mol/(L*s)=28.200

Expt #3 [A]=0.250Mol/L [B]=0.500Mol/L Rate:Mol/(L*s)=18.800

Expt #4 [A]=0.100Mol/L [B]=0.750Mol/L Rate:Mol/(L*s)=3.342.

Important: Exponents that have integer values should be entered as integers (2, 1, -1, 0, etc.). Non-integer exponents should be entered as fractions (1/3, -1/2, 3/2, 5/2, etc.).

Determine the exponential dependence of the rate law on the [A]. "x"=

Determine the exponential dependence of the rate law on the [B]. "y"=

What is the value of the rate constant for the reaction? k=