The tabulated data show the concentration of N2O5 versus time for this reaction: N2O5(g) → NO3(g) + NO2(g). Time (s) [N2O5] (M): 0 - 1.000, 25 - 0.822, 50 - 0.677, 75 - 0.557, 100 - 0.458, 125 - 0.377, 150 - 0.310, 175 - 0.255, 200 - 0.210. Determine the order of the reaction and the value of the rate constant. Predict the concentration of N2O5 at 250 s.

Verified step by step guidance

1. insert step 1: Determine the order of the reaction by analyzing the concentration data. Test for zero, first, and second order reactions by plotting [N2O5] vs. time, ln[N2O5] vs. time, and 1/[N2O5] vs. time, respectively. The plot that yields a straight line indicates the order of the reaction.
2. insert step 2: Once the order is determined, use the appropriate integrated rate law to calculate the rate constant (k). For a first-order reaction, use ln[N2O5] = -kt + ln[N2O5]_0. For a second-order reaction, use 1/[N2O5] = kt + 1/[N2O5]_0.
3. insert step 3: Calculate the slope of the straight line from the plot that determined the order of the reaction. This slope is equal to the rate constant (k) for the reaction.
4. insert step 4: Use the integrated rate law with the calculated rate constant to predict the concentration of N2O5 at 250 s. Substitute the time (t = 250 s) into the equation and solve for [N2O5].
5. insert step 5: Verify the calculated concentration by checking if it aligns with the trend observed in the data. This ensures the accuracy of the determined reaction order and rate constant.