For 2N2O5(g) = 4NO2(g) + O2(g) 1. Determine, by making the appropriate graphs, whether this decomposition reaction...

For 2N₂O₅(g) = 4NO₂(g) + O₂(g)

1. Determine, by making the appropriate graphs, whether this decomposition reaction is zero, first, or second order with respect to N2O5

I found by makin the graph in excel that it was a first order reaction

Now here are my questions

2. The stoichiometric coefficient for N205 in the reaction equation is 2. Depending on your answer to Problem 1, explain why the reaction order you obtained in Problem 1 is also 2, or explain why it can be different than 2?

3.Using the "Trendline" feature in the chart and the appropriate integrated rate equation, determine the rate constant for the reaction. (I have no idea how to even begin this in excel or on paper)

4. Sketch a graph showing the relative concentrations of N205, N02, and 02 as a function of time as the reaction proceeds. Your graph should show these concentrations on the same scale, and should show the final concentrations relative to each other after equilibrium has been reached. Note that the concentrations can be obtained just by considering the stoichiometry of the reaction. (Im not given the concentration of NO2 and O2)

Time (sec)

Conc N2O5 (M)

Conc NO2 (M)

Conc O2 (M)

0
1000
2000
8000
9000
15000
16000
20000
21000

0.75
0.65
0.57
0.24
0.21
0.092
0.080
0.046
0.040

Solutions

Expert Solution

2. The order of the reaction may not agree with stoichiometric coefficient in every reaction. As the decomposition of N2O5 is not a single step mechanism the the above is considered as non-elementary reaction. Which is why the order of the reaction is not equal to the stoichiometric coefficient of N2O5.

The above graph is rate constant (K) versus Time (T)

By taking linear series for trendline K value ranges from 13.95 x 10^-3 to 14.1 x 10^-3 (sec^-1)

The above graph if concentration of individual components versus time

Amanda K answered 1 year ago

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