Use the following data to calculate the reaction rate law and the rate law constant for the system. NO(g) + H₂(g) → HNO2(g) Initial Rate Trial Run [NO] (mol/L) [H₂] (mol/L) (mol/L.s) 1 0.001 0.004 0.002 2 0.002 0.004 0.008 3 0.003 0.004 0.018 4 0.004 0.001 0.008 5 0.004 0.002 0.016 6 0.004 0.003 0.024 a) rate = k[NO] [H₂]², where k = 7 L²/mol².s b) rate = k[NO]²[H₂], where k = 5.0x105 L²/mol²-s c) rate = k[NO] [H₂], where k = 5.0x105 L²/mol.s d) rate = k[NO]²[H₂]³, where k = 3.0x10-7 L/mol².s
Use the following data to calculate the reaction rate law and the rate law constant for the system. ??(?)+?2(?)→???2(?)
Trial Run [NO] (mol/L) [H2] (mol/L) Initial Rate (mol/L∙s)
1 0.001 0.004 0.002
2 0.002 0.004 0.008
3 . 0.003 0.004 0.018
4 0.004 0.001 0.008
5 0.004 0.002 0.016
6 . 0.004 0.003 0.024
a) rate = k[NO][H2]2, where k = 7 L2/mol2∙s
b) rate = k[NO]2[H2], where k = 5.0x105 L2/mol2∙s
c) rate = k[NO][H2], where k = 5.0x105 L2/mol∙s
d) rate = k[NO]2[H2]3, where k = 3.0x10-7 L/mol2∙s
![Use the following data to calculate the reaction rate law and the rate law
constant for the system.
NO(g) + H₂(g) → HNO2(g)
Initial Rate
Trial Run
[NO] (mol/L)
[H₂] (mol/L)
(mol/L.s)
1
0.001
0.004
0.002
2
0.002
0.004
0.008
3
0.003
0.004
0.018
4
0.004
0.001
0.008
5
0.004
0.002
0.016
6
0.004
0.003
0.024
a) rate = k[NO][H₂]², where k = 7 L²/mol².s
b) rate = k[NO]²[H₂], where k = 5.0x105 L²/mol².s
c) rate = k[NO] [H₂], where k = 5.0x105 L²/mol.s
d) rate = k[NO]²[H₂]³, where k = 3.0x10-7 L/mol²-s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc6dad125-de4a-4574-8357-3a1a28519f72%2Fcecc1d5c-033c-4484-a98d-6972c1d21c20%2Fq7443x_processed.png&w=3840&q=75)
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