A 0.26 kg iron horseshoe that is initially at 787 ◦C is dropped into a bucket...

A 0.26 kg iron horseshoe that is initially at 787 ◦C is dropped into a bucket containing 20 kg of water at 34◦C. What is the final equilibrium temperature? Neglect any energy transfer to or from the surroundings and assume the specific heat of iron is 448 J/kg · ◦ C . The specific heat of water is 4186 J/kg · ◦ C . Answer in units of ◦C

Solutions

Expert Solution

It is based on the law of conservation of energy, which says that energy is neither created nor destroyed during a chemical reaction. In calorimetry, this means that the heat gained by the water in the calorimeter must have been released by the sample or the reaction taking place in the calorimeter.

genius_generous answered 1 year ago

Next > < Previous

Related Solutions

A 1.50-kg iron horseshoe initially at 550°C is dropped into a bucket containing 18.0 kg of...

A 1.50-kg iron horseshoe initially at 550°C is dropped into a bucket containing 18.0 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 blacksmith heats a 1.4 kg iron horseshoe to 500?C , then plunges it into a...

A blacksmith heats a 1.4 kg iron horseshoe to 500?C , then plunges it into a bucket containing 20 kg of water at 15?C What is the equilibrium temperature? Express your answer using two significant figures. .

A 10.8 kg of nickel initially at 202 ∘C is dropped into an insulated basin containing...

A 10.8 kg of nickel initially at 202 ∘C is dropped into an insulated basin containing 23.6 kg of water initially at 27.8 ∘C. Assume that he water does not undergo any phase change when the hot metal was initially dropped into the water. a) Assuming no heat losses from the container, what is the final equilibrium temperature between the water and the nickel? ∘C b) What would the equilibrium temperature be if the nickel had lost 479 kJ of...

Model 2 - Oxidation of Iron C) 1.00 kg iron reacts with 0.86 kg oxygen from...

Model 2 - Oxidation of Iron C) 1.00 kg iron reacts with 0.86 kg oxygen from the atmosphere to produce iron(III) oxide {aka rust}. In model C, what is the total mass of iron and oxygen in kg? Convert to your answer to grams and show how you would do this mathematical operation, and what is the maximum possible mass of iron(III) oxide product? Please explain your answer

A 100 g piece of copper, initially at 95,0 C , is dropped into 200 g...

A 100 g piece of copper, initially at 95,0 C , is dropped into 200 g of water. If initial temperature of water is 1 5 C, what is final temperature of the system, if the heat lost to surounding is ignored please, step by step solution.

A 7.0-kg rock at a temperature of 30°C is dropped into a shallow lake at 30°C...

A 7.0-kg rock at a temperature of 30°C is dropped into a shallow lake at 30°C from a height of 1.0×10^5 m. What is the resulting change in entropy of the universe? (b) If the temperature of the rock is 100°C when it is dropped, what is the change of entropy of the universe? Assume that air friction is negligible (not a good assumption) and that c=860J/kg·K is the specific heat of the rock.

at the local county fair, you watch as a blacksmith drops a 0.50kg iron horseshoe into...

at the local county fair, you watch as a blacksmith drops a 0.50kg iron horseshoe into a bucket containing 25kg of water. If the initial temperature of the horseshoe is 450C and the initial temp of water is 23C, what is the equilibrium temp of the system?

A 50-g cube of ice, initially at 0.0°C, is dropped into 200 g of water in...

A 50-g cube of ice, initially at 0.0°C, is dropped into 200 g of water in an 80-g aluminum container, both initially at 30°C. What is the final equilibrium temperature? (Specific heat for aluminum is 900 J/kg×°C, the specific heat of water is 4 186 J/kg×°C, and Lf = 3.33 ´ 105 J/kg.)

An iron boiler of mass 180 kg contains 730 kg of water at 11 ∘C. A...

An iron boiler of mass 180 kg contains 730 kg of water at 11 ∘C. A heater supplies energy at the rate of 58,000 kJ/h. The specific heat of iron is 450 J/kg⋅C∘, the specific heat of water is 4186 J/kg⋅C∘, the heat of vaporization of water is 2260 kJ/kg⋅C∘. Assume that before the water reaches the boiling point, all the heat energy goes into raising the temperature of the iron or the steam, and none goes to the vaporization...

A 116-g cube of ice at 0 ∘∘C is dropped into 1.26 kg of water that...

A 116-g cube of ice at 0 ∘∘C is dropped into 1.26 kg of water that was originally 84.1∘C. What is the final temperature of the water after the ice melts and the water comes to thermal equilibrium? This problem requires a lot of algebra. You will make fewer errors if you solve for the answer using symbols and then plug in the numbers. The specific heat of water and the latent heat of fusion for water are given in...

Subjects