Question

If 190.8 g of water at 35°C absorbs 12.30 kJ, what is the final temperature of the water? The specific heat of water is 4.184 J/g.°C.

A. 15°C
B. 20°C
C. 35°C
D. 50°C
E. 312°C

Answer 1

The final temperature of water after absorbing 12.30 kJ is calculated using the specific heat capacity formula, resulting in approximately 51.53°C. Thus, the closest answer is Option D, 50°C.

Step-by-step explanation:

The student's question requires us to calculate the final temperature of water after it has absorbed a known amount of heat energy. To find this, we use the specific heat capacity of water which is a measure of how much energy is needed to raise the temperature of a certain amount of water by one degree Celsius.

The formula to calculate the heat absorbed or released is:
q = mcδT

where q is the heat absorbed, m is the mass of the water, c is the specific heat capacity, and δT is the change in temperature.

The specific heat capacity of water is given to be 4.184 J/g°C. We rearrange the formula to solve for the change in temperature (δT):
δT = q / (mc)

Plugging in the values, we get:
δT = 12,300 J / (190.8 g × 4.184 J/g°C)
δT ≈ 16.53°C

Since the initial temperature of the water is 35°C, the final temperature is:
35°C + 16.53°C ≈ 51.53°C

Therefore, the closest answer to the final temperature of the water is Option D, which is 50°C.