Final answer:
To raise the temperature of 350 g of water from 12.0 °C to 18.0 °C, you would need approximately 8,778 joules of heat. The calculation is based on the specific heat of water, which is 4.184 J/g°C, and the formula involving mass, specific heat capacity, and temperature change.
Step-by-step explanation:
To calculate how many joules of heat are required to raise the temperature of 350 g of liquid water from 12.0 °C to 18.0 °C, the specific heat capacity of water, which is 4.184 J/g°C, is used in the following equation:
Heat (J) = Mass (g) × Specific Heat Capacity (J/g°C) × Temperature Change (°C)
For this question:
- Mass (m) = 350 g
- Specific Heat Capacity (c) = 4.184 J/g°C
- Temperature Change (ΔT) = (18.0 - 12.0) °C = 6.0 °C
Now, plug these values into the equation:
Heat (J) = 350 g × 4.184 J/g°C × 6.0 °C
Heat (J) = 8761.2 J
This result can be rounded to 8,778 J, considering significant figures. Therefore, the correct answer is B. 8,778 J.