The following question refer to the reaction shown below: A + 2B ---> 2C Experiment 1: Initial [A] (mol/L) 0.20; Initial [B] (mol/L) 0.30; Initial Rate of Disappearance of A (mol/L*s) 0.04.....Experiment 2: Initial [A] (mol/L) 0.20; Initial [B] (mol/L) 0.60; Initial Rate of Disappearance of A (mol/L*s) 0.16.....Experiment 3: Initial [A] (mol/L) 0.10; Initial [B] (mol/L) 0.60; Initial Rate of Disappearance of A (mol/L*s) 0.08..... Question 1: Write the rate law for this reaction. Q2: Calculate the reaction order of this reaction for A and B? Q3: Calculate the rate constant (k) for the reaction (don't forget the unit). If you can somehow help me and maybe upload the worked out problem I would greatly appreciate it and thank you in advance