To calculate the energy required to raise 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 of the substance (in grams),
- \( c \) is the specific heat capacity (in J/g°C),
- \( \Delta T \) is the change in temperature (in °C).
Given:
- \( m = 20 \) g
- \( c = 0.215 \) J/g°C
- Initial temperature \( T_i = 72 \) °C
- Final temperature \( T_f = 88 \) °C
First, calculate the change in temperature (\( \Delta T \)):
\[ \Delta T = T_f - T_i = 88 , °C - 72 , °C = 16 , °C \]
Now, plug in the values into the formula:
\[ Q = 20 , g \cdot 0.215 , \text{J/g°C} \cdot 16 , °C \]
Calculating this step by step:
- Calculate \( 20 \cdot 0.215 = 4.3 , J/°C \)
- Now multiply by \( 16 , °C \):
\[ Q = 4.3 , J/°C \cdot 16 , °C = 68.8 , J \]
Therefore, the energy required to raise the temperature of the substance is 68.8 J.
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