A blacksmith drops 1.5 kg piece of iron heated to 525°C into 2 L of water with temperature of 70°C. What will be the final temperature of water? Calculate amount of evaporated water, and final temperature.
SOLUTION :
Heat flows from higher temperature object to lower temperature object when they come in contact with each other. This process continues until temperature of both the objects become equal. This is the final equilibrium temperature.
Let the final temperature be tF º C when iron metal piece at 525º C is dropped in the water which is at 70º c.
So,
Heat given up by iron metal = Heat received by water
=> mM * sM * (525 - tF) = mW * sW * (tF - 70)
(Where, mass m is in grams, specific heats is in J / g ºC and temperature is in º ç)
=> (1.5 * 1000) * 0.450 * (525 - tF) = 2000 * 4.18 * (tF - 70)
=> 675 * (525 - tF) = 8360 * (tF - 70)
=> 8360 tF + 675 tF = 8360*70 + 675 * 525
=> 9035 tF = 939575
=> tF = 939575 / 9035
=> 103.9928 º C = 104º C = Final temperature of water (ANSWER).
Heat available for vaporisation
= 2000 * 4.18 * (104 - 100) = 33440 J
Latent heat of water for vaporisation = 2230 J / g
So, amount of water vaporised
= 33440 / 2230
= 15 g (ANSWER).
And after vaporisation final temperature of water = 100º C (ANSWER).
A blacksmith drops 1.5 kg piece of iron heated to 525°C into 2 L of water...
At the local county fair, you watch as a blacksmith drops a 0.520-kg iron horseshoe into a bucket containing 26.5 kg of water. If the initial temperature of the horseshoe is 454°C, and the initial temperature of the water is 23.1°C, what is the equilibrium temperature of the system? Assume no heat is exchanged with the surroundings. Do not enter unit. b) Suppose the 0.520-kg iron horseshoe had been a 1.07-kg lead horseshoe instead. What would the equilibrium temperature be...
A blacksmith cools a 1.80 kg chunk of iron, initially at a temperature of 650.0∘C, by trickling 30.0 ∘C water over it. All the water boils away, and the iron ends up at a temperature of 120.0∘C. 1- How much water did the blacksmith trickle over the iron?
A blacksmith cools a 1.22-kg chunk of iron, initially at a temperature of 650.0∘C, by trickling 15.8 ∘C water over it. All the water boils away, and the iron ends up at a temperature of 120.0∘C. Part A How much water did the blacksmith trickle over the iron? Express your answer with the appropriate units. mwater mwater = 109g SubmitPrevious AnswersRequest Answer Incorrect; Try Again; One attempt remaining
A 1.5 kg block of iron at 30 ∘C is rapidly heated by a torch such that 17 kJ is transferred to it. What temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? If that same amount of heat (17 kJ ) was quickly transferred to a 890 g pellet of copper at 34 ∘C, what temperature would the copper reach before it begins losing heat to the surroundings? Use...
A blacksmith forging a 930.0-g knife blade drops the steel blade, initially at 670.0°C, into a water trough containing 38.0 kg of water at 23.0°C. Assuming none of the water boils away or is lost from the trough and no energy is lost to the surrounding air, what is the final temperature of the water-knife blade system? Assume Csteel = 450 J/(kg . °C).
A blacksmith forging a 945.0-g knife blade drops the steel blade, initially at 690.0°C, into a water trough containing 44.0 kg of water at 21.5°C. Assuming none of the water boils away or is lost from the trough and no energy is lost to the surrounding air, what is the final temperature of the water–knife blade system? Assume Csteel = 450 J/(kg · °C).
Calculate the molar heat capacity of iron, A 45.61g piece of iron heated to 96.32˚C is transferred to a calorimeter containing 80.00g water initially at 24.91˚C. The temperature of the system at thermal equilibrium is 28.04˚C.
A student drops a 0.35 kg piece of steel at 42°C into a contaoner of water at 22°C. The student also drops a 0.55 kg chunk of lead into the same container at the same time. The temperature of water remains the same. what is the temperature of the lead?
GENERAL CHEMISTRY HELP A 15 g g piece of iron (Cp=0.444 J/(g•°C)) is heated to a temperature of 100°C and placed into a bucket containing 2 kg of water (Cp = 4.184J/(8.°C)) initially at 25°C. Eventually, the water will be warmer than the iron. the iron will be warmer than the water. the iron will be colder than the water. the iron and the water will be at the same temperature. O the temperature will be the average of 100°C...
A piece of iron is recovered from a murder scene. It is heated to 103.7oC and then put into a calorimeter containing 100.0 mL of water at room temperature, (25.0oC). The temperature of the water increases to 57.8oC. What is the mass of the iron piece?