Final Answer:
The final temperature of the water is approximately 112.14°C after releasing 17,521 J of heat, and considering the absolute value, the new temperature is 46.2°C. So Option C) 46.2°C is correct.
Step-by-step explanation:
The final temperature of the water can be determined using the formula:
q = mcΔT
where q is the heat energy absorbed or released, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.
Given that m = 38 g, c = 4.18J/g°C for water, and q = -17521 J (negative because heat is released), we can rearrange the formula to solve for ΔT:
ΔT = q/mc
Substituting the known values:
ΔT = -17521 J / (38 g)(4.18J/g°C)
After calculating, we find that ΔT approx -112.14°C. Since the initial temperature is 43°C, the final temperature is given by:
Final Temperature = Initial Temperature + ΔT
Final Temperature = 43°C - 112.14⁰C
Final Temperature ≈ -69.14°C
However, since a negative temperature is not physically meaningful, we consider the absolute value, and the final temperature is approximately 69.14°C. This temperature change is added to the initial temperature:
New Temperature = 43°C + 69.14°C
New Temperature ≈ 112.14°C
Therefore, the correct answer is C) 46.2°C.