Question

In: Physics

A 0.420 kg iron horseshoe that is initially at 450°C is dropped into a bucket containing...

A 0.420 kg iron horseshoe that is initially at 450°C is dropped into a bucket containing 19.7 kg of water at 22.6°C. What is the final equilibrium temperature (in °C)? Neglect any heat transfer to or from the surroundings. Do not enter units.

Expert Solution

Since there is no heat transferred from surroundings heat gained by system is zero

Here heat will be transferred from iron to water

Let heat energy gained by water be Q₁

Let heat lost by iron be Q₂

Let the temperature of water be t₁ = 22.6⁰ C

Let the temperature of iron be t₂ = 450⁰ C

Since no heat is transferred from surroundings, heat lost by iron is equal to heat gained by water

So, Q₁ = -Q₂ (-ve sign represent the loss of heat)

Q₁ + Q₂ = 0

then m_1* s₁ * t₁ + m₂ * s₂ * t₂ = 0

where m₁ is the mass of water = 19.7 kg

s₁ is the specific heat of water = 4190 J/kg K

m₂ is mass of iron = 0.42 kg

s₂ is the specific heat of iron = 470 J/kg K

t₁ = T_f - 22.6 , t₂ = T_f - 450 where T_f is the final temperature

So, 19.7 * 4190 * (T_f - 22.6) + 0.42 * 470 * (T_f - 450) = 0

82543 * T_f - 1865471.8 + 197.4 * T_f - 88830 = 0

82740 * T_f - 1954301.8 = 0

So, T_f = 1954301.8/82740.4 = 23.61⁰ C

so final temperature is T_f = 23.61⁰C

Here since mass of water is too high compared to iron,so final temperature is near to temperature of water

genius_generous answered 6 days ago

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 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

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...

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. .

1. In carbonitriding of an iron-carbon alloy (steel) initially containing 0.05 wt% C and no nitrogen...

1. In carbonitriding of an iron-carbon alloy (steel) initially containing 0.05 wt% C and no nitrogen is subjected to carbonitriding at an elevated temperature and in an atmosphere that gives a surface carbon concentration constant at 0.5 wt% and surface nitrogen concentration constant 0.2 wt%. Find the ratio of the diffusion coefficients ‘C in steel’/‘N in steel’ if after 36 h the concentration of carbon at a position 0.4 mm below the surface is 0.35 wt%, and the concentration of...

A 25 g piece of hot iron is dropped into a glass of ice water containing...

A 25 g piece of hot iron is dropped into a glass of ice water containing 15.0 g of ice and 50.0 g of water. If the iron loses 8.00 kJ of energy to the ice water in achieving equilibrium, what is the equilibrium temperature? ∆Hfus = 6.01 kJ/mol

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 62.5 g of iron with a heat capacity of .450 J/C is heated to 100...

A 62.5 g of iron with a heat capacity of .450 J/C is heated to 100 degree C. It is then transferred to a coffee cup calorimeter containing 52.7 g of water (specific heat of 4.184J/g C) initially at 20.63C. if the final temp of the system is 29.59 what was the heat capacity of the calorimeter?

1.45 kg of ice at -5 ∘C is dropped into 31 kg of water at temperature 15.3 ∘C . Part...

1.45 kg of ice at -5 ∘C is dropped into 31 kg of water at temperature 15.3 ∘C . Part A - Final Temperature What is the final temperature of the system? (If I've set the problem up right, you should be given numbers such that all of the ice has melted.) Tf = ∘C Part B - Entropy of Warming Ice What is the change in entropy of the ice, as it warms up before melting? S = J/K Part C - Entropy...

Asample of a food material weighing 10 kg is initially at 450% moisture content dry basis....

Asample of a food material weighing 10 kg is initially at 450% moisture content dry basis. It is dried to 10% moisture content wet basis. How much water is removed from the sample per kg of dry solids?