A 50.0 g piece of hot iron is placed in 165 g of water with an...
A 50.0 g piece of hot iron is placed in 165 g of water with an initial temperature of 22.8°C. The temperature of the combination rises to 25.7°C. What was the initial temperature of the iron? The specific heat of iron is 0.449 J/gK and the specific heat of water is 4.18 J/gK.
Homework Answers
A 50.0 g piece of iron metal is heated to 200. oC. Then, the iron is...
A 50.0 g piece of iron metal is heated to 200. oC. Then, the iron is placed into a water bath which is at 25.0oC. Eventually, both the iron and the water reach a temperature of 30.0oC. Determine the mass of water used in the experiment. (Specific heat for water is 4.184 J/g . oC ; the specific heat for iron is 0.449 J/g . C )
A hot lump of 42.5 g of iron at an initial temperature of 98.4 °C is...
A hot lump of 42.5 g of iron at an initial temperature of 98.4 °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 30.9 g of iron at an initial temperature of 86.4 °C is...
A hot lump of 30.9 g of iron at an initial temperature of 86.4 °C is placed in 50.0 mL H, 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.
Determine the final temperature (in K) if a 10.0 g piece of hot iron, at 77⁰C,...
Determine the final temperature (in K) if a 10.0 g piece of hot iron, at 77⁰C, is placed in 50.0 g of cold water at 20⁰C. (Specific heat capacity of iron is 0.45Jg·K and that of water is 4.184 Jg·K )
1/2 H2(g) + 1/2012(g) - HCl(g) Question 18 (1 point) A piece of iron (mass =...
1/2 H2(g) + 1/2012(g) - HCl(g) Question 18 (1 point) A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/gºC and water = 4.18 J/gºC. 308 K 348 K 325 K 287 K 388...
A 33.3 g hot piece of metal at 450K is placed in pure water that has...
A 33.3 g hot piece of metal at 450K is placed in pure water that has a volume of 155.0 mL which has an initial temperature of 5.3°C. After five minutes, equilibrium is established. What is the final temperature of the water in Celsius if the metal has a specific heat 0.33 J/g°C
QUESTION 1 A 34.6 g piece of metal, initially at 96.0 °C is placed in 50.0...
QUESTION 1 A 34.6 g piece of metal, initially at 96.0 °C is placed in 50.0 g of water (C = 4.18 J/gº) initially at 21.0 °C in an insulated container. The system comes to thermal equilibrium (the metal and the water are at the same temperature) at 23.1 ° C. Calculate the specific heat of the metal. C=/ 8°C)
L JU" 10- 32) 32) A piece of iron (mass = 25.0 g) at 398 K...
L JU" 10- 32) 32) A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 250 mL of water at 298 K Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 gºC and water = 4.18 JgPC A) 287 K B) 388 K C) 348 K D) 325K E) 308 K
A 130.0 g piece of copper (specific heat 0.38 J/g･°C) is heated and then placed into...
A 130.0 g piece of copper (specific heat 0.38 J/g･°C) is heated and then placed into 400.0 g of water initially at 20.7°C. The water increases in temperature to 22.2°C. What is the initial temperature of the copper? (The specific heat of water is 4.18 J/g･°C and the density of water is 1.00 g/mL).
A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed...
A
hot lump of 32.3 g of copper at an initial temperature of 96.5°C is
placed in 50.0 mL 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 0.385J/g°C and
the specific heat of water is 4.184J/g°C?
4. A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed in 50.0 mL H20 initially at 25.0°C...
A hot lump of 30.9 g of iron at an initial temperature of 86.4 °C is placed in 50.0 mL H, 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.
1/2 H2(g) + 1/2012(g) - HCl(g) Question 18 (1 point) A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/gºC and water = 4.18 J/gºC. 308 K 348 K 325 K 287 K 388...
QUESTION 1 A 34.6 g piece of metal, initially at 96.0 °C is placed in 50.0 g of water (C = 4.18 J/gº) initially at 21.0 °C in an insulated container. The system comes to thermal equilibrium (the metal and the water are at the same temperature) at 23.1 ° C. Calculate the specific heat of the metal. C=/ 8°C)
L JU" 10- 32) 32) A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 250 mL of water at 298 K Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 gºC and water = 4.18 JgPC A) 287 K B) 388 K C) 348 K D) 325K E) 308 K
A
hot lump of 32.3 g of copper at an initial temperature of 96.5°C is
placed in 50.0 mL 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 0.385J/g°C and
the specific heat of water is 4.184J/g°C?
4. A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed in 50.0 mL H20 initially at 25.0°C...
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