Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

8. Thermochemistry

Thermochemical Equations

General Chemistry

8. Thermochemistry

Thermochemical Equations

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Multiple Choice

When iron metal is mixed with hydrochloric acid, the following reaction occurs: 2Fe(s) + 6HCl(aq) → 2FeCl3(aq) + 3H2(g). When 1.104 g of iron is mixed with 26.023 g of HCl in a coffee cup calorimeter, the temperature rises from 25.2°C to a final temperature of 32.5°C. What is the enthalpy change (ΔH) for the reaction per mole of iron, assuming the specific heat capacity of the solution is 4.18 J/g°C and the total mass of the solution is 100.0 g?

-125 kJ/mol

-100 kJ/mol

-200 kJ/mol

-165 kJ/mol

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Verified step by step guidance

Identify the limiting reactant by calculating the moles of iron and HCl. Use the molar mass of iron (55.85 g/mol) and HCl (36.46 g/mol) to convert grams to moles.

Determine the heat absorbed by the solution using the formula q = mcΔT, where m is the total mass of the solution (100.0 g), c is the specific heat capacity (4.18 J/g°C), and ΔT is the change in temperature (32.5°C - 25.2°C).

Convert the heat absorbed (q) from joules to kilojoules by dividing by 1000, since 1 kJ = 1000 J.

Calculate the enthalpy change (ΔH) per mole of iron by dividing the heat absorbed (in kJ) by the moles of iron reacted. This will give you ΔH in kJ/mol.

Compare the calculated ΔH value with the given options to determine the correct answer, which is -165 kJ/mol.