Math Problem Statement
Solution
The image contains a problem regarding the enthalpy change () for a reaction involving combustion. Here's the transcription of the problem for clarity:
Problem Statement:
Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for:
- : ,
- : ,
- : ,
calculate for the reaction:
Solution:
The enthalpy change () for the reaction is calculated using the formula:
Step 1: Write down the enthalpies for the given compounds:
- : (reactant)
- : (reactant; 2 moles, so multiply by 2)
- : (product)
Step 2: Substitute into the formula:
[ \Delta H = \left[ \Delta H(C_4H_8) \right] - \left[ \Delta H(C_4H_4) + 2 \cdot \Delta H(H_2) \right] ]
Substitute the values: [ \Delta H = \left[ -2755 \right] - \left[ -2341 + 2 \cdot (-286) \right] ]
Step 3: Simplify:
Final Answer:
Do you want further details or additional examples?
Related Questions:
- What is the significance of negative and positive values of ?
- How would the calculation change if one of the substances was in a different phase?
- How are enthalpy changes measured experimentally?
- What is the role of stoichiometry in enthalpy calculations?
- Can this reaction be considered endothermic or exothermic? Why?
Tip:
Always ensure the phases of reactants and products match the provided enthalpy values, as phase changes can affect the enthalpy significantly.
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Math Problem Analysis
Mathematical Concepts
Thermodynamics
Chemical Reactions
Enthalpy Change
Formulas
ΔH = Σ(enthalpies of products) - Σ(enthalpies of reactants)
Theorems
Hess's Law
Suitable Grade Level
Grades 10-12 (High School Chemistry)
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