Chemical Forums
Chemistry Forums for Students => Physical Chemistry Forum => Topic started by: Fr9219 on May 11, 2013, 08:40:30 AM
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Do you determine the steady state rate law for consumption of a reactant in the same way as you determine the rate law for the formation of a product?
Here is the equation:
2NO + H2 ----> N20 + H20
The mechanistic equations are:
2NO ----> N2O2 (k1)
N2O2 ----> 2NO (k2)
N2O2 + H2 ----> N20 + H20 (k3)
The question is: Determine the rate law for the consumption of H2
N2O2 is the intermediate.
Is d[H2]/dt = [N2O2] [H2] correct?
PLEASE HELP ME ?!
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I am not a professional kineticist, but your expression has no rate constants in it. Also, were you told to use the steady-state approximation for this problem?
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1. You need a rate constant
2. Your sign's wrong
3. N2O2 needs to be eliminated
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is it d[H2]/dt = - k3k1 [NO]2[H 2]/(k2 + k3[H]2)?
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sorry d[H2]/dt = - k3k1[NO]2[H2]/(k2 + k3[H2])?