The specific heat of a 108 g block of material is to be determined. The block is placed in a 25 g copper calorimeter that also holds 60 g of water. The system is initially at 20°C. Then 113 mL of water at 80°C are added to the calorimeter vessel. When thermal equilibrium is attained, the temperature of the water is 54°C. Determine the specific heat of the block.
The specific heat of a 108 g block of material is to be determined. The block...
The specific heat of a 90 g block of material is to be determined. The block is placed in a 25 g copper calorimeter that also holds 60 g of water. The system is initially at 20
2. A 0.825-kg block of iron, with an average specific heat of 5.60 x102 J/kg K, is initially at a temperature of 352°C. It is placed in a calorimeter that has 40.0 g of water at 20.0°C. What is the final thermal equilibrium temperature? If your answer if 100.0°C, calculate the amount of water that remains in liquid form. Treat the mass and heat capacity of the calorimeter as neglible.
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...
An aluminium block is heated to 100 °C and then placed immediately in 100 g of water which is initially at a temperature of 25.0 °C in a coffee cup calorimeter. Once the system reaches thermal equilibrium, the temperature of the water that surrounds the block is 28.0 °C. Calculate the mass of the aluminium block. The specific heat capacity of Al is 0.900 J g^–1 K^–1 and for H2O is 4.184 J g^–1 K^–1
Calculating specific heat capacity A constant-pressure calorimeter is often used to find the specific heat capacity of a substance if it is not known. A known mass of the substance can be heated and added to water of known mass and initial temperature. Since the specific heat capacity of water is known ( C s,water =4.184J/(g⋅ ∘ C)) , the amount of heat transferred to the water can be calculated by measuring the final temperature of the mixture at thermal...
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 28 g block of ice is cooled to −78◦C. It is added to 562 g of water in an 80 g copper calorimeter at a temperature of 21◦C. Find the final temperature. The specific heat of copper is 387 J/kg ·◦C and of ice is 2090 J/kg ·◦C . The latent heat of fusion of water is 3.33 × 105 J/kg and its specific heat is 4186 J/kg ·◦C . Answer in units of ◦C. i need help asap
A 26 g block of ice is cooled to −62 ◦C. It is added to 569 g of water in an 80 g copper calorimeter at a temperature of 27◦C. Find the final temperature. The specific heat of copper is 387 J/kg · ◦C and of ice is 2090 J/kg · ◦C . The latent heat of fusion of water is 3.33 × 105 J/kg and its specific heat is 4186 J/kg · ◦C . Answer in units of ◦C.
A 25 g block of ice is cooled to −74 ◦C. It is added to 559 g of water in an 80 g copper calorimeter at a temperature of 21◦C. Find the final temperature. The specific heat of copper is 387 J/kg · ◦C and of ice is 2090 J/kg · ◦C . The latent heat of fusion of water is 3.33 × 105 J/kg and its specific heat is 4186 J/kg · ◦C . Answer in units of ◦C.
SPECIFIC HEAT OF A METAL Specific heat is an intensive property, which is the amount of heat required to raise the temperature of 1 gram substance by 1°C. Specific heat units areJ/g °C. Solve the following problems using your lecture notes: 1. When 8.50 g of metal, initially at 82 °C, is placed in 45 g water at 20°C, the final temperature of the metal and water is 22 °C. Calculate the specific heat of the metal in J/gºC. (specific...