The equations for each step and the corresponding enthalpy changes are: a. c (graphite) + o2(g) > co2 (g) ah = - 393.5 kj b. h2(g) + 1/2o2 (g) > h: 0 () ah = -285.8 kj c. 2ch3(g) + 50(g) > 4co2 (g) + 2h20 (1) ah = -2598.8 kj

There are main groups in the modern periodic table of elements

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

If anyone would be able to me out with these three questions it would be these are from the chem 2202 course.