A 0.07 kg ice cube at -300C is placed in 0.43 kg of 30.30C water in a very well-insulated container. What is the final temperature in degrees Celsius?
Specific heat of ice = 2000 J/(kg.K), Specific heat of water = 4186 J/(kg.K), Latent heat of fusion of ice = 33.5 x 104 J/kg.
A 0.07 kg ice cube at -300C is placed in 0.43 kg of 30.30C water in...
A 0.0600 kg ice cube at −30.0°C is placed in 0.537 kg of 35.0°C water in a very well insulated container. What is the final temperature? The latent heat of fusion of water is 79.8 kcal/kg, the specific heat of ice is 0.50 kcal/(kg · °C), and the specific heat of water is 1.00 kcal/(kg · °C).
A 0.0575 kg ice cube at −30.0°C is placed in 0.617 kg of 35.0°C water in a very well insulated container, like the kind we used in class. The heat of fusion of water is 3.33 x 105 J/kg, the specific heat of ice is 2090 J/(kg · K), and the specific heat of water is 4190 J/(kg · K). The system comes to equilibrium after all of the ice has melted. What is the final temperature of the system?
A 0.0725 kg ice cube at −30.0°C is placed in 0.497 kg of 35.0°C water in a very well insulated container, like the kind we used in class. The heat of fusion of water is 3.33 x 105 J/kg, the specific heat of ice is 2090 J/(kg · K), and the specific heat of water is 4190 J/(kg · K). The system comes to equilibrium after all of the ice has melted. What is the final temperature of the system?
An 80g ice cube at 0 degrees Celsius is placed in 798g of water at 30 degrees Celsius. What is the final temperature of the mixture? The latent heat of fusion for water is 3.33x10^5J/kg and the specific heat of water is 4186J/(kg x degrees Celsius).
A 0.0400-kg ice cube at −30.0°C is placed in 0.350 kg of 35.0°C water in a very well-insulated container. What is the final temperature in degrees Celsius?
A 0.0500-kg ice cube at −30.0°C is placed in 0.450 kg of 35.0°C water in a very well-insulated container. What is the final temperature in degrees Celsius?
The temperature of 2.26 kg of water is 34 °C. To cool the water, ice at 0 °C is added to it. The desired final temperature of the water is 11 °C. The latent heat of fusion for water is 33.5 × 104 J/kg, and the specific heat capacity of water is 4186 J/(kg·C°). Ignoring the container and any heat lost or gained to or from the surroundings, determine how much mass m of ice should be added.
A 0.0550-kg ice cube at -30.0°C is placed in 0.300 kg of 35.0°C water in a very well-insulated container. What is the final temperature in degrees Celsius? X °C + Additional Materials eBook
A 29.0 g ice cube at -15.0oC is placed in 180 g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...
How much heat is required to change 456 g of ice at -20.0Degree C into water at 25.0Degree C? specific heat of water = 4186]/(kg-K); specific heat of ice = 2090 J/(kg.K) and latent heat of fusion of water = 33.5 times 10^4 J/kg.