Question

Copper has a specific heat of 0.386 J/g°C. How much heat is required to increase 5.00 g of copper from 0.0°C to 10.0°C?

3.86 J
5.00 J
10.0 J
19.3 J

Answer 1

To calculate the heat required to increase the temperature of a substance, you can use the formula:

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

where:
- \( q \) is the heat energy (in joules),
- \( m \) is the mass (in grams),
- \( c \) is the specific heat capacity (in J/g°C),
- \( \Delta T \) is the change in temperature (in °C).

Given:
- \( m = 5.00 \, \text{g} \)
- \( c = 0.386 \, \text{J/g°C} \)
- \( \Delta T = 10.0°C - 0.0°C = 10.0°C \)

Now plug in the values:

\[
q = 5.00 \, \text{g} \cdot 0.386 \, \text{J/g°C} \cdot 10.0 \, \text{°C}
\]

Calculating that:

\[
q = 5.00 \cdot 0.386 \cdot 10.0 = 19.3 \, \text{J}
\]

Therefore, the amount of heat required to increase the temperature of 5.00 g of copper from 0.0°C to 10.0°C is **19.3 J**.