11:11 AM Sun Oct 22 Question 16 of If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.0 mol of NO₂ were collected, then what is the percent yield for the reaction? 2 NO (g) + O₂(g) → 2 NO₂ (g)
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.
![**Question 16 of 34**
If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.0 mol of NO₂ were collected, then what is the percent yield for the reaction?
\[ 2 \, \text{NO (g)} + \text{O}_2 \, (\text{g}) \rightarrow 2 \, \text{NO}_2 \, (\text{g}) \]
**Explanation:**
To calculate the percent yield, you need to compare the actual yield (the amount of product collected) to the theoretical yield (the amount of product expected based on stoichiometry).
1. **Theoretical Yield Calculation:**
According to the balanced equation, 1 mole of O₂ reacts with 2 moles of NO to produce 2 moles of NO₂. Therefore, if you start with 10 moles of O₂, you would expect to produce:
\[
10 \, \text{moles O}_2 \times \frac{2 \, \text{moles NO}_2}{1 \, \text{mole O}_2} = 20 \, \text{moles NO}_2
\]
2. **Actual Yield:**
The problem states that 5.0 moles of NO₂ were collected.
3. **Percent Yield Calculation:**
\[
\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% = \left( \frac{5.0}{20} \right) \times 100\% = 25\%
\]
Thus, the percent yield for the reaction is 25%.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F65936c84-20b2-4046-a438-4a3445f2d7a5%2Fc98d95be-5a9c-4de9-a02e-424a2fd78e9c%2Fiqzk1i9_processed.jpeg&w=3840&q=75)
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