What is the change in enthalpy when 1.50 moles of H₂ are reacted with an excess O2 of according to the following balanced chemical reaction: -381 mol H₂ ADD FACTOR 381 g 0₂ -572 KJ 2 H₂(g) + O₂(g) -429 ΔΗ = -572 1.50 g H₂O 32.0 - kJ 1 2 H₂O(l) ANSWER mol O₂ 429 2 mol H₂O RESET J 2 18.02 2.02 g H₂
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.
![**Title: Calculating the Change in Enthalpy During a Reaction**
**Description:**
The problem asks for the change in enthalpy when 1.50 moles of \( \text{H}_2 \) are reacted with an excess of \( \text{O}_2 \) according to the given balanced chemical reaction:
\[ 2 \, \text{H}_2(g) + \text{O}_2(g) \rightarrow 2 \, \text{H}_2\text{O}(l) \]
The enthalpy change (\( \Delta H \)) for the reaction is given as -572 kJ.
**Interface:**
The user interface is designed to calculate the enthalpy change based on input values:
1. **Input Fields:**
- Two pairs of input boxes allow the user to set up a calculation by determining the correct proportion or conversion factor to use.
2. **Calculation Tools:**
- Users can choose from a selection of numerical values and units to perform their calculations:
- Values: -381, 381, -572, -429, 1.50, 1, 2, 18.02, 2.02.
- Units: mol \( \text{H}_2 \), g \( \text{O}_2 \), kJ, mol \( \text{O}_2 \), mol \( \text{H}_2\text{O} \), J, g \( \text{H}_2 \).
3. **Answer Box:**
- An answer box is provided for the user to input the final calculated enthalpy change.
4. **Reset Button:**
- A reset button is available to clear the inputs and start over.
**Purpose:**
This interface guides students through finding the change in enthalpy for the given reaction using stoichiometry and thermochemical data. Students apply the concept of enthalpy proportionality to determine the heat change for a specific amount of reactant, reinforcing understanding of thermochemical equations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc42f8bf5-c4ea-440d-bf0d-c8a9270c2068%2F375ebc8f-5ee7-4ac3-b5b9-7ef16bfbb22e%2F2ns12ac_processed.jpeg&w=3840&q=75)
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