The irreversible, elementary gas phase reaction shown below is carried out in an

Question

The irreversible, elementary gas phase reaction shown below is carried out in an isothermal, isobaric CSTR reactor. Calculate the volume of the reactor that reaches conversion equal to 60%. A rightarrow B + C, -r_A = k C_A Data: y_A degree - 1, k = 0.1 L mol^-1 s^-1, F_A degree = 2 mol/s, C_A degree = 1 mol/liter A plot of ln C_A (M) vs t (s) gives a slope = -0.03 and an intercept = 0 with R^2 = 0.6. A plot of 1/C_A (M) vs t (s) gives a slope = 0.02 and an intercept = 1 with R^2 = 0.6. A plot of C_A (M) vs t (s) gives a slope = -0.01 and an intercept = 1 with R^2 = 0.95. Calculate the order of reaction and the k value. Justify using the integral method.

Explanation / Answer

Given:

1. Ca vs t, Slope = -0.03 intercept = 0 R2 = 0.6

2. 1/Ca vs t, slope = 0.02 intercept = 1 R2 = 0.6

3. Ca vs t, Slop = 0.01 intercept = 1 R2 = 0.95

We can assume the first data set as Zero order as it has negative slope but the data for linearity of the graph is not provided and the intercept is zero which cannot be possible.

similarly the second data set suggest the reaction can be second order but again the linearity of the graph is not given

Coming to third option, the graph is plotted as Ca vs t with positive slope which is also not possible.

so the given reaction should be second order. The K value of the reaction is 0.02.

Kindly refer the reference link given below.

Reference:

https://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Kinetics/Reaction_Rates/Using_Graphs_to_Determine_Rate_Laws

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