Question

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.

Homework Answers

Answer #1

Let us denote water by symbol 1 and iron by symbol 2
volume of water is 50.0 mL and density is 1 g/mL. So,
mass of water = density * volume
= 1 g/mL * 50.0 mL
= 50.0 g
m1 = 50.0 g
T1 = 25.0 oC
C1 = 4.184 J/goC
m2 = 37.8 g
T2 = 51.3 oC
C2 = 0.449 J/goC
T = to be calculated

Let the final temperature be T oC
use:
heat lost by 2 = heat gained by 1
m2*C2*(T2-T) = m1*C1*(T-T1)
37.8*0.449*(51.3-T) = 50.0*4.184*(T-25.0)
16.9722*(51.3-T) = 209.2*(T-25.0)
870.6739 - 16.9722*T = 209.2*T - 5230
T= 27.0 oC

Answer: 27.0 oC

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
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 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.
A hot lump of 38.038.0 g of iron at an initial temperature of 79.7 °C79.7 °C...
A hot lump of 38.038.0 g of iron at an initial temperature of 79.7 °C79.7 °C is placed in 50.0 mL H2OH2O 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)?0.449 J/(g·°C)? Assume no heat is lost to surroundings.
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 hot lump of 46.2 g of copper at an initial temperature of 93.9 °C is...
A hot lump of 46.2 g of copper at an initial temperature of 93.9 °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 copper and water given that the specific heat of copper is 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 27.5 g of copper at an initial temperature of 54.7 °C is...
A hot lump of 27.5 g of copper at an initial temperature of 54.7 °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 copper and water given that the specific heat of copper is 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 26.3 g of aluminum at an initial temperature of 67.2 °C is...
A hot lump of 26.3 g of aluminum at an initial temperature of 67.2 °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 aluminum and water given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 42.6 g of aluminum at an initial temperature of 62.2 °C is...
A hot lump of 42.6 g of aluminum at an initial temperature of 62.2 °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 aluminum and water given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings. Please show all work
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....