А00000155 1.2.1 Formal kinetics of chemical reactions.

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1.2.1 Formal kinetics of chemical reactions. Arrhenius equation

1.2.1.1 Plot the concentration C of the starting material versus time t for reaction B given in Table 1.3 in the coordinates lnC = f(t) and 1/C = f(t). Determine the order of the reaction from the graph.
Option 6.
Reaction B: С2Н5Br = C2H4 + HBr
T = 677 K
t, s c∙103 mol/l
0 1.0000
30 0.9712
60 0.9432
120 0.8897
240 0.7916
300 0.7465
1.2.1.2 Calculate the rate constant of reaction B.
1.2.1.3 Calculate the concentration of the starting material and reaction products B after 200 s from the beginning of the reaction.
1.2.1.4 Calculate the time it takes for 10% of the starting material to react.
1.2.1.5 Determine the half-life of reaction B.
1.2.1.6 Determine the activation energy of chemical reaction B (Table 1.3) using the reaction rate constants k1 and k2 at two temperatures T1 and T2 (Table 1.4).
1.2.1.7 Write down the Arrhenius equation. Determine the pre-exponential factor in the Arrhenius equation.
1.2.1.8 Determine the rate constant of chemical reaction B at temperature T3 (Table 1.4).
1.2.1.9 Determine the van´t Hoff temperature coefficient for the reaction rate B in the temperature range T1 and T2.
1.2.1.10 Using the temperature coefficient, determine how many times the reaction rate will change if the temperature T1 is increased by T (Table 1.4).