Homework Help: Chemistry

Posted by Kyo on Thursday, November 11, 2010 at 4:53am.

The given reaction,
2N2O5 4NO2 + O2,
follows first-order kinetics and has an activation energy of 103 kJ mol-1. At 298 K, k = 0.0000354 s-1. What is the half-life (min) for this reaction at 338 K ? Round your answer to 3 significant figures.

Chemistry - DrBob222, Thursday, November 11, 2010 at 3:47pm
k = 0.693/t_1/2
Substitute for k and calculate t_1/2.
Chemistry - Kyo, Thursday, November 11, 2010 at 8:11pm
?? and then what do you do?
.0000354 = 0.693/t(1/2)
t(1/2) = 19576.27119
Chemistry - Kyo, Thursday, November 11, 2010 at 10:34pm
the answer is suppose to be 2.38 min

Answer this Question

Related Questions

CHEM- KINETICS - Dinitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, ...
chemistry - The given reaction, cyclopropane propene (isomerization), follows ...
chemistry - follows first-order kinetics and has an activation energy of 244 kJ ...
Chemistry - The standard free energy of activation of a reaction A is 88.6 kJ ...
Chem - Variation of the rate constant with temperature for the first-order ...
chemistry - The standard free energy of activation of a reaction A is 78.2 kJ ...
chemistry - The activation energy for the reaction in which CO2 decomposes to CO...
chemistry - calculate the lattice energy of sodium oxide (Na2O) from the ...
Chemistry - 1. The reaction, CO(CH2COOH)2 CO(CH3)2 + 2CO2, follows first-order ...
chemistry - I have two questions that I really don't understand. The first ...

For Further Reading

First Name:
School Subject:
Answer: