The rate constant for the first-order decomposition of N20 is 3.40 s1. What is the half-life of the decomposition? O 0.424 s O 0.204 s O 0.491 s O 0.236 s O 0.294 s
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![**Determining Half-Life for a First-Order Decomposition Reaction**
The rate constant for the first-order decomposition of N₂O is 3.40 s⁻¹. What is the half-life of the decomposition?
**Multiple Choice Options:**
- O 0.424 s
- O 0.204 s
- O 0.491 s
- O 0.236 s
- O 0.294 s
To solve this, you can use the formula for the half-life of a first-order reaction:
\[ t_{1/2} = \frac{0.693}{k} \]
where \( t_{1/2} \) is the half-life and \( k \) is the rate constant.
By substituting \( k = 3.40 s^{-1} \):
\[ t_{1/2} = \frac{0.693}{3.40} \approx 0.204 s \]
So, the half-life of the decomposition is approximately 0.204 seconds.
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For educational purposes, it's important to understand the calculation of half-life from rate constants, especially in first-order reactions, as this knowledge is widely applicable in fields such as chemistry and pharmacokinetics.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F560885b1-95a6-46a1-8479-9132da42c8bd%2Fc9264626-5492-47d0-b641-76a0cbf18f1b%2Flt7vza_processed.jpeg&w=3840&q=75)
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