4. The decomposition of N₂O5 to NO₂ and O₂ is a first-order reaction with the rate constant, k = 1.2 x 10³ s¹ at 374 K. a. Determine the half-life of this reaction. b. At 374 K, how much N₂O5 would remain in a 1.0 L flask 5.0 min after the introduction of 0.05 mol of N₂O5?
4. The decomposition of N₂O5 to NO₂ and O₂ is a first-order reaction with the rate constant, k = 1.2 x 10³ s¹ at 374 K. a. Determine the half-life of this reaction. b. At 374 K, how much N₂O5 would remain in a 1.0 L flask 5.0 min after the introduction of 0.05 mol of N₂O5?
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Chapter1: Chemical Foundations
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![4. The decomposition of N₂O5 to NO2 and O₂ is a first-order reaction with the rate constant, k = 1.2 x 10³ s¹ at 374
K.
a. Determine the half-life of this reaction.
b. At 374 K, how much N₂O5 would remain in a 1.0 L flask 5.0 min after the introduction of 0.05 mol of
N₂O5?
5. The reaction A➜ products is a second-order reaction and takes place at 32°C.
a.
Given that the half-life of this reaction is 4.22 x 104 s when the initial concentration of A is 0.2 M, what is
the rate constant for the reaction? Include units with your answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F50de52e1-7d33-4b3c-a050-8482f7f33c6d%2Fccb6a8ce-fa50-4506-893f-124d0aa44c98%2F37m8px_processed.jpeg&w=3840&q=75)
Transcribed Image Text:4. The decomposition of N₂O5 to NO2 and O₂ is a first-order reaction with the rate constant, k = 1.2 x 10³ s¹ at 374
K.
a. Determine the half-life of this reaction.
b. At 374 K, how much N₂O5 would remain in a 1.0 L flask 5.0 min after the introduction of 0.05 mol of
N₂O5?
5. The reaction A➜ products is a second-order reaction and takes place at 32°C.
a.
Given that the half-life of this reaction is 4.22 x 104 s when the initial concentration of A is 0.2 M, what is
the rate constant for the reaction? Include units with your answer.
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