Dinitrogen pentoxide decomposes via a first order reaction. Rate = k[N,Os], k = 6.93 × 10*3 s-1 The concentration of N,O5 is initially 0.200 mol/L. After 100 s it has dropped to 0.100 mol/L and after 200 s it has dropped to 0.0500 mol/L. What is the concentration after 150 s?

In a study to determine the rate of the following reaction: 2NO(g) + O₂(g) - 2NO₂(g) the concentration of NO was 0.0550 Mat t= 5.0 s and 0.0225 Mat t= 650.0 s. What is the average rate of the reaction during this time period? M/S

The initial concentration of reactant in a first order reaction is 0.27 M.  The rate constant for the reaction is 0.75 s-1.  What is the concentration (in mol/L) of reactant after 1.5 seconds? 3.8 1.7 0.088 0.020

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: O [A] = 6.0 and [B] = 0.6 O [A] = 3.0 and [B] = 0.6 O [A] = 4.5 and [B] = 0.6 [A] = 1.5 and [B] = 1.2 O [A] = 3.0 and [B] = 1.8 [A] = 1.5 and [B] = 1.8 O [A] = 3.0 and [B] = 1.2 O [A] = 7.5 and [B] = 0.6 Rate = K[A][B][C] Rate = K[A][C] Experiment [A] (M) [B] (M) Rate (M/s) (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A]* [B]Y? Choose all correct possibilities. k[A]² [C] O Rate = K[A][C]² Rate = k[A]²[C]² Rate = k[A]³ [C] O Rate = K[A][C]³ 1 2 Rate = 1.5 3.0 (b) For a reaction of the form, A + B + C --> Products, the following observations are made: tripling the concentration of A increases the rate by a factor of 9, doubling the concentration of B has no effect on the rate, and doubling the concentration of C…