Butadiene reacts to form its dimmer according to the equation 2C_4H_6(g) rightar

Question

Butadiene reacts to form its dimmer according to the equation 2C_4H_6(g) rightarrow C_8H_12(g) The following data were collected for this reaction at a given temperature. a. Is this reaction first order or second order? b. What is die value of the rate constant for the reaction? c. What is the half-life for the reaction under the conditions of this experience. The balanced equation for the reaction of the gases nitrogen dioxide 2NO_2(g) + F_2(g) rightarrow 2NO_2F(g) The experimentally determined rate law is Rate = k[NO_2][F_2] A suggested mechanism for this reaction is NO_2 + F_2 rightarrow NO_2F + F F + NO_2 rightarrow NO_2F

Explanation / Answer

On plotting a garph between Ln(concentration) v/s time if a straight line is obtained then the rate of reaction is of first order

So not first order

Now we will plot graph between time and 1/ [conc]

A straight line is obtained so the order = 2

The rate constant

The rate constant = slope

Equation is y = 0.061x + 99.36

Slope = rate constant = 0.061

c) t1/2 = 1/ K[A0] = 1 / 0.061 X 0.01 = 1639.34 seconds

concentration time Ln concentration 0.01 0 -4.60517 0.00625 1000 -5.07517 0.00476 1800 -5.34751 0.0037 2800 -5.59942 0.00313 3600 -5.76672 0.0027 4400 -5.9145 0.00241 5200 -6.02813 0.00208 6200 -6.17539

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