A jar of tea is placed in sunlight until it reaches an equilibrium temperature of 32.6 ◦C . In an attempt to cool the liquid, which has a mass of 189 g , 98.8 g of ice at 0.0 ◦C is added. At the time at which the temperature of the tea is 28.6 ◦C , find the mass of the remaining ice in the jar. The specific heat of water is 4186 J/kg · ◦ C . Assume the specific heat capacity of the tea to be that of pure liquid water. Answer in units of g.
A jar of tea is placed in sunlight until it reaches an equilibrium temperature of 32.6...
7. A cube of ice is taken from the freezer at -4.0 °C and placed in a 70 g aluminum calorimeter filled with 450 g of water at room temperature of 25.0 °C. The System reaches an equilibrium temperature of 20.0°C. Calculate the mass of the ice cube. Given that, Latent heat of fusion of ice Specific heat capacity of water 4186 Jkg-1 °C-1 Specific heat capacity of aluminum 880 Jkg-1K-1 333700 Jkg-1
A piece of solid lead weighing 32.6 g at a temperature of 311 °C is placed in 326 g of liquid lead at a temperature of 367 °C. After a while, the solid melts and a completely liquid sample remains. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is ΔHfus = 4.77 kJ/mol at its melting point of 328 °C, and the molar heat capacities for...
PROBLEM 5-8 points You are making iced tea. The tea itself is initially at a temperature of 50.0 °C. You then toss in an ice cube with a mass of 50 and an initial temperature of -20.0 °C. The ice cube melts, and the final temperature of the mixture is +30.0 °C. For this problem, use the following values: c for liquid water is 4000 J/(kg "C), c for solid water is 2000 J/(kg°C), and the latent heat of fusion...
You order a 16 oz glass of tea (where the mass of water is 474 grams) from a local restaurant. The tea is freshly brewed and has an initial temperature of 20.73 °C. You add ice to cool it. If the heat of fusion of ice is 6.020 kJ/mol and each ice cube contains exactly 1 mol of water (assume the ice does not add anymore volume), how many ice cubes are necessary to cool the tea to 0.240 °C?...
You order a 16 oz glass of tea (where the mass of water is 474 grams) from a local restaurant. The tea is freshly brewed and has an initial temperature of 28.93 °C. You add ice to cool it. If the heat of fusion of ice is 6.020 kJ/mol and each ice cube contains exactly 1 mol of water (assume the ice does not add anymore volume), how many ice cubes are necessary to cool the tea to 1.54 °C?...
You order a 16 oz glass of tea (where the mass of water is 474 grams) from a local restaurant. The tea is freshly brewed and has an initial temperature of 25.43 °C. You add ice to cool it. If the heat of fusion of ice is 6.020 kJ/mol and each ice cube contains exactly 1 mol of water, how many ice cubes are necessary to cool the tea to 2.83 °C? The specific heat of the "tea" is 4.184...
You order a 16 oz glass of tea (where the mass of water is 474 grams) from a local restaurant. The tea is freshly brewed and has an initial temperature of 20.39 °C. You add ice to cool it. If the heat of fusion of ice is 6.020 kJ/mol and each ice cube contains exactly 1 mol of water, how many ice cubes are necessary to cool the tea to 2.62 °C? The specific heat of the "tea" is 4.184...
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.
Calculate the final equilibrium temperature when 10.0 grams of steam initially at 100 degree C is mixed with 450 grams of liquid water and 110 grams of ice at 0 degree C in a calorimeter. That is, the liquid water AND the ice are initially at 0 degree C. Ignore any heat energy exchanges with the calorimeter and the surroundings. If you conclude that the final temperature of the system is 0 degree C, then what mass of ice remains,...
The temperature of 2.7 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 333.5 × 103 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. m = kg