Which energy is needed to change 35.0 g of lead at 22.0˚C to 400.0˚C?

To calculate the energy required to heat a substance, we use the formula:

\[
Q = m \cdot c \cdot \Delta T
\]

where:
- \( Q \) is the heat energy required (in joules, J),
- \( m \) is the mass of the substance (in grams, g),
- \( c \) is the specific heat capacity of the substance (in joules per gram per degree Celsius, J/g°C),
- \( \Delta T \) is the change in temperature (in degrees Celsius, °C).

For lead:
- Specific heat capacity (\( c \)) = 0.128 J/g°C,
- Mass (\( m \)) = 35.0 g,
- Temperature change (\( \Delta T \)) = \( 400.0^\circ C - 22.0^\circ C = 378.0^\circ C \).

Now, plug in the values:

\[
Q = 35.0 \, \text{g} \times 0.128 \, \text{J/g°C} \times 378.0 \, \text{°C}
\]

Let's calculate this.The energy required to heat 35.0 g of lead from 22.0°C to 400.0°C is approximately 1693.44 joules.

Would you like more details on this calculation or have any other questions?

Here are five related questions you might find interesting:
1. How do you calculate the energy needed for phase changes in addition to temperature changes?
2. What is the specific heat capacity, and why does it vary between substances?
3. How does the mass of a substance affect the energy required to heat it?
4. How does the energy required change if you use a different material, such as water or copper?
5. What is the role of specific heat capacity in thermal energy storage?

**Tip:** When dealing with temperature changes, always ensure you're using consistent units, especially for specific heat capacity and temperature.

Discover how to calculate the energy needed to change 35.0 g of lead from 22.0°C to 400.0°C using the formula Q = m * c * ΔT. Explore the specific heat capacity of lead and the temperature change involved in this problem.

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