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The conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °C is first order in CH3NC . In one experiment, when the initial concentration of CH3NC was 0.115 M, the concentration of CH3NC dropped to 2.09x10^-3 after 430 seconds had passed. Based on these data, the rate constant for the reaction is .



Answer :

subhamjrp

Explanation:

The rate constant (k) for a first-order reaction can be calculated using the formula:

k = -ln(A/A₀) / t

where:

A₀ = initial concentration = 0.115 M

A = final concentration = 2.09 × 10^-3 M

t = time = 430 s

Plugging in the values, we get:

k = -ln(2.09 × 10^-3 / 0.115) / 430

= -ln(1.82 × 10^-2) / 430

= 0.0255 s^-1

Therefore, the rate constant for the reaction is 0.0255 s^-1.

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