Final answer:
To find the energy required to heat 38.0g of water from 25.0°C to 105.00°C, we calculate using the specific heat capacity formula resulting in 12.7 kJ, which is not among the provided options suggesting a possible typo.
Step-by-step explanation:
The question asks how much energy is required to raise the temperature of 38.0g of water from 25.0°C to 105.00°C. To solve this, we use the formula q = mc∆T, where q is the heat energy, m is the mass of the water, c is the specific heat capacity of water, and ∆T is the change in temperature. Given that the specific heat capacity of water is 4.184 J/g°C, the mass of the water is 38.0 g, and the change in temperature (∆T) is 105.00°C - 25.00°C = 80.00°C, we can calculate the energy required.
Plugging in the values:
q = (38.0 g)(4.184 J/g°C)(80.00°C)
q = 12701.76 J
Since 1 kJ = 1000 J, we have:
q = 12.70176 kJ
Therefore, the closest answer provided in the options is B. 12.7 kJ, which is not listed, indicating there may be a typo in the options provided.