ch M The decomposition of N₂O5 can be described with the following reaction: 2 N₂O5(g) → 4NO2(g) + O2(g) - The reaction is second order. The rate law for the reaction is: a) rate = K[N₂051² b) rate= k/ [N₂05] c) rate = k ([NO₂]4 x [0₂]) / [N₂05] d) rate = k[N₂05] e) rate = k/ [N₂O5]² o E C п % 5 6 & 7 99+ hp 8 O 9 to 411 O fn 77°F inse
ch M The decomposition of N₂O5 can be described with the following reaction: 2 N₂O5(g) → 4NO2(g) + O2(g) - The reaction is second order. The rate law for the reaction is: a) rate = K[N₂051² b) rate= k/ [N₂05] c) rate = k ([NO₂]4 x [0₂]) / [N₂05] d) rate = k[N₂05] e) rate = k/ [N₂O5]² o E C п % 5 6 & 7 99+ hp 8 O 9 to 411 O fn 77°F inse
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![rch
The
decomposition of N₂O5 can be described with the following reaction:
2 N₂O5(g) → 4NO2(g) + O2(g)
The reaction is second order. The rate law for the reaction is:
E
$
a) rate = K[N₂051²
b) rate = k/ [N₂O5]
c) rate = k ([NO₂] x [0₂]) / [N₂05]
d) rate = k[N₂O5]
e) rate = k/ [N₂O51²
O
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C
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4
&
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8
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Transcribed Image Text:rch
The
decomposition of N₂O5 can be described with the following reaction:
2 N₂O5(g) → 4NO2(g) + O2(g)
The reaction is second order. The rate law for the reaction is:
E
$
a) rate = K[N₂051²
b) rate = k/ [N₂O5]
c) rate = k ([NO₂] x [0₂]) / [N₂05]
d) rate = k[N₂O5]
e) rate = k/ [N₂O51²
O
101
R
DL
D
C
F
%
b
V
T
6
4
&
G H
7
B N
+
00
8
J
1
IAA
M
(
9
K
O
O
W
fn
U
(?)
{
77°F
insert
Expert Solution
Step 1
Given ->
2N2O5(g) --> 4NO2(g) + O2(g)
-> The reaction is of second order .
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