Please help, none of these make sense

What is the rate for the zero order reaction A Products when [A]= 0.200M?(k=5.01M/min) The reaction A+B2C has the rate law rate =k[A][B]3. By what factor does the rate of reaction increase when [A] remains constant but [B] is doubled? The following reaction 2AB+C is second order, following the rate law Rate =k[A]2. If the starting concentration [A0]=0.250M, and after 245min,[A(t)]=0.0150M, what is the second order rate constant k (in M1min1 ) ? Consider the table of data collected for the reaction A Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. How long will it take for the concentration of A to decrease from 1.25 M to 0.309 for the second order reaction A Products? (k=1.52 M1min1)