A reaction produces carbon monoxide and hydrogen. The reaction runs between 750

Question

A reaction produces carbon monoxide and hydrogen. The reaction runs between 750 degrees C and 1100 degrees C. When the reaction is run in large excess of water, it displays first order kinetics with respect to the concentration of methane and zeo order kinetics with respect to water. At 750 degree C, the half life of this reaction under these conditions is 67.5 minutes. If the activcation energy for this reaction is 96.2 kj/ mol: What is the rate constant k at both 750 degree C and 1100 degree C?

Explanation / Answer

at 750 c   rate constant k1 = 0.693/(t1/2)

k1 = (0.693/67.5) = 0.0103 min-1.

so that,

ln(k2/k1) = (eA/R)(1/T1-1/T2)

ln(K2/0.0103) = (96.2*10^3/8.314)((1/1023.15)-(1/1373.15))

K2 = 0.1834 min-1.

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