To calculate the heat energy used, 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), and
- \( \Delta T \) is the change in temperature (in °C).
Given:
- \( m = 33 , \text{g} \)
- \( c = 0.385 , \text{J/g°C} \)
- Initial temperature = 240 °C
- Final temperature = 393 °C
First, calculate the change in temperature:
\[ \Delta T = \text{Final Temperature} - \text{Initial Temperature} = 393 , °C - 240 , °C = 153 , °C \]
Now, substitute the values into the equation:
\[ Q = 33 , \text{g} \cdot 0.385 , \text{J/g°C} \cdot 153 , °C \]
Calculating this:
\[ Q = 33 \cdot 0.385 \cdot 153 \] \[ Q = 33 \cdot 0.385 = 12.705 , \text{J/}°C \] \[ Q = 12.705 \cdot 153 = 1942.065 , \text{J} \]
So, the total heat energy used is approximately:
\[ Q \approx 1944 , \text{J} \]
Thus, the answer is 1944 J.