Podcast
Questions and Answers
What formula represents the relationship between the enthalpy changes during a combustion reaction?
What formula represents the relationship between the enthalpy changes during a combustion reaction?
- ΔH1 = ΔHf + ΔH2 (correct)
- ΔHf = ΔH1 - ΔH2
- ΔHf + ΔH2 = ΔH1
- ΔH1 = ΔHf - ΔH2
If ΔHf for NaHCO3(s) is -950.8 kJ/mol, what is the overall enthalpy change, ΔHr, for the reaction involving Na2CO3(s), CO2(g), and H2O(l)?
If ΔHf for NaHCO3(s) is -950.8 kJ/mol, what is the overall enthalpy change, ΔHr, for the reaction involving Na2CO3(s), CO2(g), and H2O(l)?
- -104.2 kJ/mol
- 84.6 kJ/mol
- 91.6 kJ/mol (correct)
- 100.3 kJ/mol
What does Hess's Law state regarding enthalpy changes in a chemical reaction?
What does Hess's Law state regarding enthalpy changes in a chemical reaction?
- The total enthalpy change is always zero.
- The enthalpy change can differ based on the path taken.
- The enthalpy change is dependent solely on the products formed.
- The total enthalpy change is the same regardless of the route taken. (correct)
What is the first step in applying Hess's Law for enthalpy change calculations?
What is the first step in applying Hess's Law for enthalpy change calculations?
Which of the following statements about standard enthalpy of formation is correct?
Which of the following statements about standard enthalpy of formation is correct?
How can one indirectly determine the standard enthalpy of formation from combustion products?
How can one indirectly determine the standard enthalpy of formation from combustion products?
What does ΔH2 represent in the equation ΔH1 = ΔHf + ΔH2?
What does ΔH2 represent in the equation ΔH1 = ΔHf + ΔH2?
When performing enthalpy change calculations, what must be considered about the elements involved?
When performing enthalpy change calculations, what must be considered about the elements involved?
Which statement best describes Hess’s Law?
Which statement best describes Hess’s Law?
What is a typical application of Hess's Law?
What is a typical application of Hess's Law?
In an energy cycle using Hess's Law, how are ΔHr and ΔHf related?
In an energy cycle using Hess's Law, how are ΔHr and ΔHf related?
What does the symbol ΔHf indicate?
What does the symbol ΔHf indicate?
Which of the following statements is true regarding combustion enthalpy?
Which of the following statements is true regarding combustion enthalpy?
Which reaction pathway does Hess's Law allow you to compare?
Which reaction pathway does Hess's Law allow you to compare?
In a given reaction represented by 3C (s) + 4H2 (g) → C3H8(g), why can ΔHf (propane) not be found experimentally?
In a given reaction represented by 3C (s) + 4H2 (g) → C3H8(g), why can ΔHf (propane) not be found experimentally?
What is the significance of the initial and final conditions in Hess's Law?
What is the significance of the initial and final conditions in Hess's Law?
What is the enthalpy change of combustion for carbon (graphite) when reacting with oxygen?
What is the enthalpy change of combustion for carbon (graphite) when reacting with oxygen?
Using Hess's Law, how is the enthalpy of formation (ΔHf) for ethane calculated?
Using Hess's Law, how is the enthalpy of formation (ΔHf) for ethane calculated?
What is the enthalpy of formation of ethane (C2H6), calculated from the provided values?
What is the enthalpy of formation of ethane (C2H6), calculated from the provided values?
What is the definition of the enthalpy change of atomisation (ΔHθat)?
What is the definition of the enthalpy change of atomisation (ΔHθat)?
When calculating average bond energies using Hess's cycles, what is essential?
When calculating average bond energies using Hess's cycles, what is essential?
In which reaction is water produced as a product?
In which reaction is water produced as a product?
What do the values of ΔH1, ΔH2, and ΔH3 represent in the enthalpy formation calculation using Hess's Law?
What do the values of ΔH1, ΔH2, and ΔH3 represent in the enthalpy formation calculation using Hess's Law?
What is the overall process used for calculating the enthalpy change of formation of a compound?
What is the overall process used for calculating the enthalpy change of formation of a compound?
Study Notes
Enthalpy of Formation and Hess's Law
- Standard enthalpy of formation (ΔHf) refers to the change in enthalpy when one mole of a compound is formed from its elements in their standard states.
- Hess’s Law states that the total enthalpy change for a reaction is the same, regardless of the paths taken, as long as the initial and final conditions are identical.
Applying Hess's Law
- Formula to apply Hess's Law: ΔHr = ΔH2 – ΔH1
- Example calculation for sodium carbonate:
- ΔHr = (ΔHf [Na2CO3 (s)] + ΔHf [CO2 (g)] + ΔHf [H2O (l)]) – 2ΔHf [NaHCO3 (s)]
- Result: ΔHr = +91.6 kJ mol⁻¹
Calculating ΔHf from ΔHc
- Combustion products can be derived directly from elements (ΔH1) or indirectly through intermediates (ΔHf + ΔH2).
- Relationship: ΔHf = ΔH1 – ΔH2
- Example for ethane (C2H6):
- Combustion reactions with associated ΔHc values are needed.
- Calculation yields ΔHf = –84.7 kJ mol⁻¹ for ethane.
Average Bond Energies
- Average bond energies are determined using Hess’s law and cannot be measured directly.
- Enthalpy changes of atomisation and combustion or formation are used to calculate average bond energies.
Summary of Hess's Law Applications
- Hess's Law allows for the calculation of enthalpy changes that are difficult to obtain experimentally.
- The method helps predict the enthalpy change in reactions where direct measurement is not feasible, such as the reaction of hydrogen and carbon under standard conditions.
Key Points
- Direct routes for reactions yield the same enthalpy change as indirect routes.
- Understanding and applying Hess's Law is crucial for thermodynamic calculations in chemistry.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
Test your knowledge on the standard enthalpy of formation and Hess's Law. This quiz includes questions that will help you understand how to apply thermodynamic principles effectively. Whether you're preparing for an exam or brushing up on your chemistry knowledge, this quiz is for you.
