The table below gives concentrations of reactants and products as a function of

Question

The table below gives concentrations of reactants and products as a function of time for the following reaction at 55 degree C: 2N_2O5 (g) rightarrow 4 NO_2 (g) + O_2 (g) Plot [N_2O_5] vs. Time (s) on a separate graph. Label the axes and give title as "Zero Order Test." Fit a straight line through the points and display the equation on the graph. Display the RSQ value on the graph as well. Plot In [N_2O5] vs. Time (s) on a separate graph. Label the axes and give title as "First Order Test." Fit a straight line through the points and display the equation and the RSQ value on the graph. Plot 1 / [N_2O_5] vs. Time (s) on a separate graph. Label the axes and give title as "Second Order Test." Fit a straight line through the points and display the equation and the RSQ value on the graph. Determine the order of reaction with respect to N_2O_5 and the rate constant with appropriate units. Write this information on the appropriate graph.

Explanation / Answer

We Know that :

      The given reaction is :

              2 N2O5 (g) 4 NO2 (g) +O2 (g)

     Rate of the reaction = -1 / 2 d [ N2 O5 ] / dt   = + 1 / 4 d [ NO2 ] / dt = + d [ O2] / dt

           Average Rate of Formation of O2 is :

              [0.0064 - 0.0040 ] / 600 - 300

        = 0.000008 M/ s

             Average rate of decompopsition of N2O5 is :

               [ 0.0072 - 0.0120 ] M /   600 - 300s

         =    - 0.000016 M / s

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