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Chemistry
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12 Nov 2019

From the following data for the first-order gas-phase isomerization of CH3NC at 215 ?C, calculate the first-order rate constant and half-life for the reaction:

Time (s) Pressure CH3NC(torr)
0 502
2000 335
5000 180
8000 95.5
12000 41.7
15000 22.4




k = ?

t1/2 = ?

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Tod Thiel
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21 Aug 2019

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Related questions

From the following data for the first-order gas-phase isomerization of CH3NC at 215 °C, calculate the first-order rate constant and half-life for the reaction:

The isomerization of methyl isonitrile (CH3NC) to acetonitrile (CH3CN) was studied in the gas phase at 215 °C, and the following data were obtained:

(a) Calculate the average rate of reaction, in M/s, for the time interval between each measurement. (b) Calculate the average rate of reaction over the entire time of the data from t = 0 to t = 15,000 s. (c) Which is greater, the average rate between t = 2000 and t = 12,000 s, or between t = 8000 and t = 15,000 s? (d) Graph [CH3NC] versus time and determine the instantaneous rates in M/s at t = 5000 s and t = 8000 s.

The following data were collected for the conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °C.

CH3NC(g)--------->CH3CN(g)

[CH3NC], M 4.20×10-2 2.10×10-2 1.05×10-2 5.25×10-3
time, s 0 160.00 320.00 480.00




(a) What is the half-life for the reaction when [CH3NC] = 4.20×10-2 M?

_______s

(b) What is the half-life for the reaction when [CH3NC] = 2.10×10-2 M? ______s

(c) Is the reaction first order? yes or no?

If so, what is the rate constant for the reaction? (If not first order leave blank).__________________ s-1

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