q11 a 500 g iron block (c = 0.449 j g^{-1} °c^{-1}) and a 500 g block of water both absorb 10,000 j of heat energy.
(a) calculate the temperature change (\delta t) for the iron block.
(b) calculate the temperature change (\delta t) for the water.
(b) a different liquid requires only 2,600 j to achieve the same temperature change for the same mass. calculate the specific heat capacity of this liquid.
(c) would the other liquid in (b) be a better or worse thermal buffer than water? explain.
q12 the specific heat capacity of water is much higher than most other liquids. explain this at the molecular level, with reference to hydrogen bonding.
(c) what does this comparison tell you about why water is used as a coolant in car engines and industrial processes?

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{ "quality": "clear", "question_count": 5, "skills_matched": [ "step_cot", "explain_then_answer", "quick" ], "needs_drawing": false, "concepts_used": [ "Specific Heat Capacity", "Heat Energy Calculations", "Hydrogen Bonding in Water" ], "new_concepts": [ "Thermal Buffering Capacity" ], "current_concepts": [ "Specific Heat Capacity", "Heat Energy Calculations", "Hydrogen Bonding in Water", "Thermal Buffering Capacity" ] } ## Calculate temperature change for the iron block $$ \begin{aligned} &q = m \cdot c \cdot \Delta T \ &\Delta T_{\text{iron}} = \frac{q}{m \cdot c} = \frac{10000\text{ J}}{500\text{ g} \cdot 0.449\text{ J g}^{-1}\text{ }^{\circ}\text{C}^{-1}} \approx 44.54\text{ }^{\circ}\text{C} \end{aligned} $$ ## Calculate temperature change for the water block $$ \begin{aligned} &c_{\text{water}} = 4.18\text{ J g}^{-1}\text{ }^{\circ}\text{C}^{-1} \ &\Delta T_{\text{water}} = \frac{q}{m \cdot c} = \frac{10000\text{ J}}{500\text{ g} \cdot 4.18\text{ J g}^{-1}\text{ }^{\circ}\text{C}^{-1}} \approx 4.78\text{ }^{\circ}\text{C} \end{aligned} $$ ## Explain water as a coolant and its high specific heat capacity $$ \begin{aligned} &\text{Water absorbs large amounts of heat with minimal temperature change, making it an excellent coolant.} \ &\text{Extensive hydrogen bonding requires significant energy to break before kinetic energy (temperature) increases.} \end{aligned} $$ ## Question 11 (a) The temperature change ($\Delta T$) for the iron block is: $$\Delta T_{\text{iron}} = \frac{10000\text{ J}}{500\text{ g} \times 0.449\text{ J g}^{-1}\text{ }^{\circ}\text{C}^{-1}} \approx 44.5\text{ }^{\circ}\text{C}$$ (b) The temperature change ($\Delta T$) for the water is: $$\Delta T_{\text{water}} = \frac{10000\text{ J}}{500\text{ g} \times 4.18\text{ J g}^{-1}\text{ }^{\circ}\text{C}^{-1}} \approx 4.78\text{ }^{\circ}\text{C}$$ (c) This comparison shows that water can absorb much more heat energy than iron for the same temperature rise, explaining why water is highly effective as a coolant to prevent overheating in car engines and industrial processes. ## Question 12 At the molecular level, water molecules form extensive networks of hydrogen bonds. A large amount of heat energy must first be absorbed to disrupt and break these strong intermolecular hydrogen bonds before the kinetic energy of the water molecules can increase, resulting in an exceptionally high specific heat capacity. { "subject": "Natural Science", "question_type": "Multi-part", "knowledge_point": [ "Natural Science", "Chemistry", "Specific Heat Capacity" ] }

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Calculate temperature change for the iron block

Calculate temperature change for the water block

Explain water as a coolant and its high specific heat capacity

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Question 11

Question 12