A 1.50-kg iron horseshoe initially at 650°C is dropped into a bucket containing
ID: 1477412 • Letter: A
Question
A 1.50-kg iron horseshoe initially at 650°C is dropped into a bucket containing 12.0 kg of water at 20.0°C. What is the final temperature of the water–horseshoe system? Ignore the heat capacity of the container and assume a negligible amount of water boils away. A 1.50-kg iron horseshoe initially at 650°C is dropped into a bucket containing 12.0 kg of water at 20.0°C. What is the final temperature of the water–horseshoe system? Ignore the heat capacity of the container and assume a negligible amount of water boils away.Explanation / Answer
mi = mass of iron = 1.50 kg
T = equilbrium temperature
Ti = temperature of iron = 650 C
Tw = Temperature of water = 20 C
mw = mass of water = 12 kg
heat lost by horshoe = heat gained by water
mi Ci (650 - T) = mw Cw (T - 20)
1.5 (450) (650 - T) = 12 (4186) (T - 20)
T = 28.4
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.