11.17 Ammonia can react with oxygen to produce nitric oxide and water: 4 NH 3 ( g ) + 5 O 2 ( g ) → 4 NO ( g ) + 6 H 2 O ( g ) If the rate at which ammonia is consumed in a laboratory experiment is 4.23 ×10-4 mol L_ 1 s_l, at what rate is oxygen consumed? At what rate is NO produced? At what rate is water vapor produced?
11.17 Ammonia can react with oxygen to produce nitric oxide and water: 4 NH 3 ( g ) + 5 O 2 ( g ) → 4 NO ( g ) + 6 H 2 O ( g ) If the rate at which ammonia is consumed in a laboratory experiment is 4.23 ×10-4 mol L_ 1 s_l, at what rate is oxygen consumed? At what rate is NO produced? At what rate is water vapor produced?
Solution Summary: The author explains how ammonia reacts with oxygen to produce nitric oxide and water.
11.17 Ammonia can react with oxygen to produce nitric oxide and water:
4
NH
3
(
g
)
+
5
O
2
(
g
)
→
4
NO
(
g
)
+
6
H
2
O
(
g
)
If the rate at which ammonia is consumed in a laboratory experiment is 4.23 ×10-4 mol L_1s_l, at what rate is oxygen consumed? At what rate is NO produced? At what rate is water vapor produced?
The reaction for the Haber process, the industrial production of ammonia, is
N2(g) + 3H2(g) → 2NH3(g)
Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 mol L-1 s-1. At what rate is hydrogen consumed?
One of the least abundant nitrogen oxides in the atmosphere is dinitrogen pentoxide. One reason concentrations of this oxide are low is that the molecule is unstable and rapidly decomposes to N2O4 and O2: 2N2O5(g) → 2N2O4(g) + O2(g) A kinetic study of the decomposition of N2O5 at a particular temperature yielded the data in the following Table. Assume that the decomposition of N2O5 is first order in N2O5.
Test the validity of your assumption.
Determine the value of the rate constant.
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