Question

Exactly 14.1 mL of water at 31.0 degrees C are added to a hot iron skillet....

Exactly 14.1 mL of water at 31.0 degrees C are added to a hot iron skillet. All of the water is converted into steam at 100 degrees C. The mass of the pan is 1.45 kg and the molar heat capacity of iron os 25.19 J/(mol degrees C). What is the temperature change of the skillet?

Homework Answers

Answer #1

Heat lost by iron = heat gained by water

nFe X CFe X ΔT = energy needed to raise temperatute from 32oC to 100oC + heat needed vaporise the water.

nFe = no. of moles of iron, CFe = heat capacityof iron , ΔT = change in temperature.

nFe X CFe X ΔT = nH2O X CH2O X ΔT + ΔH X n

nFe = mass in grams / molar mass = 1450 / 55.84 = 25.96

nH2O =14.1 / 18 = 0.783 Moles 14mL of water = 14 g (because density = 1)

25.96 X 25.19 X ΔT = 0.783 X 75.24 X (100-31) + 40.65 X 0.783

ΔT = 4096.3 / 653.93 = 6.26oC

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Exactly 10.8 mL of water at 30.0 degrees C are added to a hot iron skillet....
Exactly 10.8 mL of water at 30.0 degrees C are added to a hot iron skillet. All of the water is converted into steam at 100 degrees C. The mass of the pan is 1.20 kg and the molar heat capacity of iron is 25.19 J/(mol*degrees C). What is the temperature change of the skillet?
Exactly 17.7 mL of water at 35.0 °C are added to a hot iron skillet. All...
Exactly 17.7 mL of water at 35.0 °C are added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the pan is 1.20 kg and the molar heat capacity of iron is 25.19 J/(mol·°C). What is the temperature change of the skillet?
Exactly 16.7 mL of water at 32.0°C are added to a hot iron skillet. All of...
Exactly 16.7 mL of water at 32.0°C are added to a hot iron skillet. All of the water is converted into steam at 100°C. The mass of the pan is 1.10kg and the molar heat capacity of iron is 25.19J/(Mol x °C). What is the temperature change of the skillet?
1. A hot lump of 46.2 g of iron at an initial temperature of 77.9 °C...
1. A hot lump of 46.2 g of iron at an initial temperature of 77.9 °C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water given that the specific heat of iron is 0.449 J/(g·°C)? Assume no heat is lost to surroundings. 2.When 1422 J of heat energy is added to 40.8 g of hexane, C6H14, the temperature increases by 15.4 °C....
A hot lump of 45.0 g of iron at an initial temperature of 68.2 degrees celsius...
A hot lump of 45.0 g of iron at an initial temperature of 68.2 degrees celsius is placed in 50.0 mL of H2O initially at 25.0 degrees celsius and allowed to reach thermal equillibrium. What is the final temperature of the iron and water given that the specific heat of iron is 0.449 J/(G x degrees celsius)? Assume no heat is lost to surroundings.
A water drop slung onto a skillet with a temperature between 100°C and 200°C will remain...
A water drop slung onto a skillet with a temperature between 100°C and 200°C will remain a liquid for about 1 second. However, if the skillet is much hotter the drop can last several minutes. This is due to the Leidenfrost Effect, named after an early investigator (circa 1756). The longer lifetime is due to the support of a thin layer of air and water vapor that separates the drop from the metal (by a distance L, as shown in...
A 20.95 g piece of iron and a 25.20 g piece of gold at 100.0 celsius...
A 20.95 g piece of iron and a 25.20 g piece of gold at 100.0 celsius were dropped into 570.0 ml of water at 27.95 celsius. The molar heat capacities of iron and gold are 25.19 J/(mol*celsius) and 25.41 J/(mol*celsius), respectively. What is the final temperature of the water and pieces of metal?
An iron boiler of mass 180 kg contains 770 kg of water at 21 ∘C. A...
An iron boiler of mass 180 kg contains 770 kg of water at 21 ∘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...
An iron boiler of mass 180 kg contains 770 kg of water at 21 ∘C. A...
An iron boiler of mass 180 kg contains 770 kg of water at 21 ∘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...
An iron boiler of mass 180 kg contains 850 kg of water at 23 ∘C. A...
An iron boiler of mass 180 kg contains 850 kg of water at 23 ∘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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT