Question

If 339.2 g sample of iron is placed in 1.025 L of water initially at 22.761oC...

If 339.2 g sample of iron is placed in 1.025 L of water initially at 22.761oC and both substances reach a final temperature of 27.488oC, what is the initial temperature (in oC) of the metal? Assume all heat is transferred between the water and the iron.  

Homework Answers

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
If 264.6 g sample of iron is placed in 1.005 L of water initially at 19.884oC...
If 264.6 g sample of iron is placed in 1.005 L of water initially at 19.884oC and both substances reach a final temperature of 28.151oC, what is the initial temperature (in oC) of the metal? Assume all heat is transferred between the water and the iron.
An 65.73 g sample of aluminum is placed on a 56.35 g sample of copper initially...
An 65.73 g sample of aluminum is placed on a 56.35 g sample of copper initially at 111.86oC. If the heat is only transferred between the metals (with no loss to the surroundings) and the final temperature of both metals is 36.38oC, what is the inital temperature (in oC) of aluminum?
An 50.04 g sample of aluminum is placed on a 25.84 g sample of copper initially...
An 50.04 g sample of aluminum is placed on a 25.84 g sample of copper initially at 97.16oC. If the heat is only transferred between the metals (with no loss to the surroundings) and the final temperature of both metals is 53.87oC, what is the inital temperature (in oC) of aluminum
A metal sample weighing 72.1 g is placed in a hot water bath at 95.0 oC....
A metal sample weighing 72.1 g is placed in a hot water bath at 95.0 oC. The calorimeter contains 42.3 g of deoinized water. The initial temperature of the water is 22.3 oC. The metal is transferred to the calorimeter and the final temperature reached by the water + metal is 32.2 oC. A. Calculate ∆T for the water (Tfinal – Tinitial). B. Calculate ∆T for the metal. C. The specific heat of water is 4.18 J/goC. Calculate the specific...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling...
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
A hot lump of 47.6 g of iron at an initial temperature of 50.8 °C is...
A hot lump of 47.6 g of iron at an initial temperature of 50.8 °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.
A hot lump of 37.8 g of iron at an initial temperature of 51.3 °C is...
A hot lump of 37.8 g of iron at an initial temperature of 51.3 °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.
A hot lump of 44.5 g of iron at an initial temperature of 74.5 °C is...
A hot lump of 44.5 g of iron at an initial temperature of 74.5 °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.
A hot lump of 46.0 g of iron at an initial temperature of 91.5 °C is...
A hot lump of 46.0 g of iron at an initial temperature of 91.5 °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.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT