can you plot the graphs mentioned in the image using the following data

Table 5. Summary of the sample calculations before equilibrium.

Run	CA (gmol / L)	XA	K(L.gmol/min)	-ra (gmol/Lmin)
1st	0.008	0.84	1.180604357	0.002951511
2nd	0.00755	0.849	1.509333333	0.003773333
3rd	0.00745	0.851	2.387096774	0.005967742

Table 6. Summary of sample calculations after 2 hours (at equilibrium).

Run	CA (gmol / L)	XA	K(L.gmol/min)	-ra (gmol/Lmin)
1st	0.078	0.56	0.787069571	0.001967674
2nd	0.073	0.46	0.817777778	0.002044444
3rd	0.07	0.4	1.122019635	0.002805049

For a second order reaction: A+BC+D With CAO=CBo and negligible change in density of reaction mixture The reaction rate (rate of disappearance of A ) =rA=kCA2 Hence, =VoVR=rACA0XA=kCA2CA0CArA Degree of conversion, XA=(CA0CA)/CA0 and rate of reaction, rA=CA0XA/,gmol/in the rate constant, k=(CAOCA)/(CA2),1/ gmol-min for nth order reaction, rA=kCAn log(rA)=logk+nlogCA The order of the reaction, n, can be obtained from a plot of log(rA) vs logCA, that yields a straight line with slope =n, and intercept ( at CA=1 or at logCA=0) shall give the value of log(k). Also, a plot of vs XA/(1XA)2 shall yield a straight line for an assumed second order reaction with slope =1/(kCA0). From this slope rate constant, k can be obtained