Final answer:
The heat released when 192 g of water is cooled from 54 degrees Celsius to 16 degrees Celsius is approximately -30,000 J, factoring in the specific heat of water which is 4.184 J/g°C.
Step-by-step explanation:
To calculate the heat released when 192 g of water is cooled from 54 degrees Celsius to 16 degrees Celsius, we utilize the formula q = mcΔT where q is the heat exchanged, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature.
The specific heat capacity (c) of water, given as 4.184 J/g°C, indicates that to transform 1 g of water by 1 °C releases or absorbs 4.184 J. Therefore:
- Mass (m): 192 g
- Temperature change (ΔT): 54°C - 16°C = 38°C
- Specific heat (c): 4.184 J/g°C
The calculation becomes:
q = (192 g) × (38°C) × (4.184 J/g°C)
q = 30,659.424 J
Since heat is released during cooling, the sign is negative, making q = -30,659.424 J. However, when looking at the provided options, we can round it to nearest thousands, resulting in -30,000 J.