To calculate the amount of heat required to raise the temperature of water, you can use the formula:
\[ Q = m \cdot c \cdot \Delta T \]
where:
- \( Q \) is the heat added (in joules),
- \( m \) is the mass of the water (in grams),
- \( c \) is the specific heat capacity (in J/g°C),
- \( \Delta T \) is the change in temperature (in °C).
For this problem:
- Mass \( m = 20 \) grams,
- Specific heat \( c = 4.18 \) J/g°C,
- Initial temperature = 10°C,
- Final temperature = 30°C,
- Change in temperature \( \Delta T = 30°C - 10°C = 20°C \).
Now, plug in the values:
\[ Q = 20 , \text{g} \cdot 4.18 , \text{J/g°C} \cdot 20 , \text{°C} \]
\[ Q = 20 \cdot 4.18 \cdot 20 \]
\[ Q = 20 \cdot 83.6 \]
\[ Q = 1672 , \text{J} \]
Rounding to the nearest hundred joules gives us 1700 joules.
Thus, the answer is \( \text{C. } 1700 , \text{joules} \).
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