The rate constant for the first-order decomposition at 45 6.2x 10-4 min-1. what is the rate of the reaction when N,05=0.40 M ? of dinitrogen pentoxide, N205, dissolved in chloroform, CHCI3, is 2N,05→4NO,+0, (A 2.5x 10-5 mol/L/min B 2.5x 10-4 mol/L/ min 0.4 mol/L/min (D 6.2x 10-4 mol/L/min

Using the data in the table, calculate the rate constant of this reaction. k= = A + B → C + D Trial 1 2 3 Units [A] (M) [B] (M) 0.340 0.400 0.340 0.920 0.408 0.400 Rate (M/s) 0.0114 0.0603 0.0137

The reaction     2 NO (g)   +   O2 (g)   →   2 NO2 (g)     occurs when automobile exhaust releases NO into the atmosphere.  Use the following data to determine the order with respect to NO for this reaction. Trial [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.012 0.020 1.02 x 10-4 2 0.024 0.020 4.08 x 10-4 3 0.024 0.040 8.16 x 10-4   Enter the answer as a single digit, not the word.

The decomposition of nitrous oxide at 565 °C N,0(g)N2(g) +½ O2(g) is second order in N2O with a rate constant of 1.10x10-3 M's. If the initial concentration of N20 is 2.08 M, the concentration of N,0 will be |M after 3.30x103 seconds have passed.

The decomposition of nitrous oxide at 565 °CN2O(g)N2(g) + ½ O2(g)is second order in N2O with a rate constant of 1.10×10-3 M-1 s-1.If the initial concentration of N2O is 2.22 M, the concentration of N2O will be 0.258 M after seconds have passed.

Can you explain step by step?