Acompare substance with a relatively high specific heat capacity to a substance with a relatively low specific heat capacity what is the relationship between the amount of heat required and resolution temperature change for these two

To compare a substance with a **relatively high specific heat capacity** to a substance with a **relatively low specific heat capacity**, we need to understand the relationship between **specific heat capacity** and the **amount of heat required** to cause a **temperature change**.

### Definition of Specific Heat Capacity:
- The **specific heat capacity** of a substance, usually denoted as \( c \), is the amount of heat \( Q \) required to raise the temperature of 1 kg of the substance by 1 degree Celsius (or 1 Kelvin).
  
The relationship between heat, mass, specific heat capacity, and temperature change is given by the formula:
\[
Q = mc\Delta T
\]
Where:
- \( Q \) is the heat added (in joules),
- \( m \) is the mass of the substance (in kg),
- \( c \) is the specific heat capacity (in J/kg·°C or J/kg·K),
- \( \Delta T \) is the change in temperature (in °C or K).

### Comparison:

1. **Substance with High Specific Heat Capacity**:
   - It requires **more heat** to cause the **same temperature change** compared to a substance with a lower specific heat capacity.
   - For example, **water** has a high specific heat capacity (\( c \approx 4184 \, \text{J/kg·°C} \)). This means it takes a lot of heat to increase the temperature of water by a small amount.

2. **Substance with Low Specific Heat Capacity**:
   - It requires **less heat** to cause the same temperature change compared to a substance with a higher specific heat capacity.
   - For example, **metals** like **iron** have a low specific heat capacity (\( c \approx 450 \, \text{J/kg·°C} \)), so they heat up quickly with a relatively small amount of heat.

### Relationship:
- For the same **mass** and **heat input** (\( Q \)), a substance with a **high specific heat capacity** will experience a **smaller temperature change** (\( \Delta T \)) compared to a substance with a **low specific heat capacity**.
- Conversely, to achieve the **same temperature change** (\( \Delta T \)) for both substances, the substance with a **higher specific heat capacity** will require **more heat** than the substance with a **lower specific heat capacity**.

### Conclusion:
- A substance with a high specific heat capacity absorbs and stores **more heat** before showing a significant temperature rise.
- A substance with a low specific heat capacity heats up (or cools down) **faster** with the same amount of heat.

Would you like a more detailed explanation on any specific part of this comparison?

### Follow-up Questions:
1. What are practical examples of substances with high and low specific heat capacities in everyday life?
2. How does specific heat capacity affect the choice of materials for cooking utensils?
3. Why does water have such a high specific heat capacity compared to most other substances?
4. Can specific heat capacity vary with temperature or phase changes?
5. How would the formula \( Q = mc\Delta T \) apply to mixing substances with different heat capacities?

### Tip:
Always consider specific heat capacity when designing systems that need to regulate temperature, like cooling systems or thermal insulation materials!

Compare a substance with a relatively high specific heat capacity to a substance with a relatively low specific heat capacity. What is the relationship between the amount of heat required and the resulting temperature change for these two?

Understand how to compare the amount of heat required to cause a temperature change between substances with different specific heat capacities. Explore thermodynamics concepts, including the formula Q = mcΔT, and see how substances like water and metals behave under heat. Suitable for Grades 10-12.

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