Consider the reaction of a to form b: 2a< —> b. kc=1.8x10^-5(at 298k). a reaction mixture at 298k initially contains [a]=0.50m. what is the concentration of b when the reaction reaches equilibrium? the answer is 4.5x10^-6m but how do i get that answer?

For the reaction, 4 a(g) + 3 b(g) => 2 c(g), the following data were obtained at constant temperature. experiment initial[a],mol/l initial [b],mol/l initial rate, m/min 1 0.200 0.150 5.00 2 0.400 0.150 10.0 3 0.200 0.300 10.0 4 0.400 0.300 20.0 which of the following is the correct rate law for the reaction? 1. rate = k[a]2[b]2 2. rate = k[a][b] 3. rate = k[a]2[b] 4. rate = k[a][b]2