The following reaction has an activation energy of 262 kJ/mol. C_4H_8(g) rightar
ID: 484952 • Letter: T
Question
The following reaction has an activation energy of 262 kJ/mol. C_4H_8(g) rightarrow 2C_2H_4(g) 600.0 K the rate constant is 6.1 times 10^-5s^-1. What is the value of the rate constant at 815.0K? Use the Arrhenius equation to solve for k_2 ln k_2/k_1-E_R/R 1/T_1 -1/T_1 Watch out for units! If you use R=8.3145 J/(mol middot K), you'll need to convert the activation energy to J/mol. Recall that to "undo" the natural log function, you need to raise the expression as a power of e. For example, if-5 =ln(x), then x = e^-5. On this calculator, e^-5 would be entered as: 5/- INVLNExplanation / Answer
log(k2 / k1) = (Ea /2.303R) * ( T2-T1)/T1*T2
= 262000/19.147 * (215/815*600)
k2/k1 = antilog (6.016)
=1037528
k2 = 6.1 * 10^-5 * 1037528 = 63.28 s-1
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