Cyclobutane decomposes to ethylene according to the equation: c4h8(g) → 2c2h4(g) determine the value of the rate constant for the reaction based on the following pressures, which were recorded when the reaction was carried out at 430°c in a constant-volume vessel. × 10 s−1 (enter your answer in scientific notation.) time(s) mmhg 0 400 2000 316 4000 248 6000 196 8000 155 10000 122

The value of the rate constant for the reaction based on the given pressures  =  

First step : determine the order of reaction

The reaction is a first-order reaction because the S.I. unit of K = s⁻¹  in the question

next step : Plot the value of  In( p ) vs Time

Where:  P = pressure ( mmHg )

            In ( p ) =  natural Logarithm of P values

Graph is attached below

Final step : calculate the value of the slope of the graph

slope = Δ y / Δ x

         = ( 4.8 - 5.99 ) / ( 10000 - 0 )

         = -1.19 / 10000  

∴ The value of  K ( rate constant )  = 1.19  *  10^{-4} s^{-1}

Hence we can conclude that the The value of the rate constant for the reaction based on the given pressures  =  

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Explanation:

1. Determine the order of reaction

The question gives us a hint: the units of k are s⁻¹. This suggests a first order rate law.

To confirm, we plot ln(p) vs t.  We should get a straight line with slope = -k.

Here are your data with the pressures converted to natural logarithms.

We get the graph shown below.

2. Determine the rate constant

The points fit so well that we can just use the end points to determine the slope.