Answer to Question #144575 in Chemistry for OTHER

Question

The data in the table are for the reaction of NO and O2 at 660 K.
NO (g) + ½ O2 (g) → NO2 (g)
[NO] [O2] Rate of disappearance of NO
(mol/L.s)
0.010 0.010 2.5 x 10-5
0.020 0.010 1.0 x 10-4
0.010 0.020 5.0 x 10-5
a) Determine the order of the reaction for each reactant.
b) Write the rate equation for the reaction.
c) Calculate the rate constant.
d) Calculate the rate (in mol/L.s) at the instant when when [NO] = 0.015 mol/L and [O2] =
0.0050 mol/L.
e) At the instant when NO is reacting at the rate of 1.0 x10-4 mol/L.s, what is the rate at which
O2 is reacting and NO2 forming?

Answer 1

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