Question

Part B of the equation says, "If the rate constant for this reaction at 1000 K is 6.0×104M−2s−1, what is the reaction rate when [NO]= 3.60×10⁻²M and [H2]= 1.80×10⁻²M?"

Part C says, "What is the reaction rate at 1000 K when the concentration of NO is increased to 0.12 M while the concentration of H2 is 1.80×10⁻²M?" I'm confused about the units.

Answer 1

B) Rate law: Rate = k[NO] [H] Rate constant, k = 6.0x10* m*s-1 Concentration of NO, [NO]= 3.60x10-2M Concentration of H, (H)=1.80x102 M Rate of the reaction = ke[NO[H,] = (6.0x10* m*s-1)(3.60x10-2 M) (1.80x10-2 M) = 1.4 M/s C) Rate law: Rate = k [NO] [Hz] Rate constant, k = 6.0x10* M--1 Concentration of NO, [NO]= 3.60x10-2 M Concentration of Hz, [H] = 1.80x102 M Rate of the reaction = {[NO][H,] =(6.0x10* Mºs")(0.12 M) (1.80x10 PM) = 15.6 M's