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

13. Liquids, Solids & Intermolecular Forces

Heating and Cooling Curves

General Chemistry

13. Liquids, Solids & Intermolecular Forces

Heating and Cooling Curves

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Multiple Choice

If 53.2kJ of heat are added to a 15.5g ice cube at - 5.00 ^oC, what will be the resulting state and temperature of the substance?

322.5°C, gas

-3.70ºC, solid

98.82 ºC, liquid

222.5 ºC, gas

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Verified step by step guidance

Step 1: Calculate the heat required to warm the ice from -5.00°C to 0°C using the formula q = m * c * ΔT, where m is the mass of the ice (15.5 g), c is the specific heat of ice (2.09 J/g·°C), and ΔT is the temperature change (0°C - (-5.00°C)).

Step 2: Determine the heat required to melt the ice at 0°C into liquid water using the formula q = m * ΔH_fusion, where m is the mass of the ice (15.5 g) and ΔH_fusion is the heat of fusion of ice (334 J/g).

Step 3: Calculate the heat required to warm the liquid water from 0°C to 100°C using the formula q = m * c * ΔT, where m is the mass of the water (15.5 g), c is the specific heat of water (4.184 J/g·°C), and ΔT is the temperature change (100°C - 0°C).

Step 4: If there is still heat remaining after the previous steps, calculate the heat required to vaporize the water at 100°C into steam using the formula q = m * ΔH_vaporization, where m is the mass of the water (15.5 g) and ΔH_vaporization is the heat of vaporization of water (2260 J/g).

Step 5: If there is still heat remaining after vaporization, calculate the temperature increase of the steam using the formula q = m * c * ΔT, where m is the mass of the steam (15.5 g), c is the specific heat of steam (assumed to be similar to water, 2.09 J/g·°C), and q is the remaining heat. Compare the total heat added (53.2 kJ) to the sum of all these steps to determine the final state and temperature.