Solution:
At equilibrium,
Heat added = heat removed
Answer : option 3
You have hot water of a mass Minitially at 80°C. You add ice, initially at 0°C,...
A block of ice with a mass of 1.25kg is initially at -40 degrees C. It is placed into a thermally isolated container with 0.500kg of water at 75 degrees C. How much of the ice melts? Cice= 2.10 kJ/kgK Cwater= 4.186 kJ/kgK Csteam= 2.00 kJ/kgK Lf= 334 kJ/kg Lv= 2265 kJ/kg
Initially you have mW = 3.4 kg of water at TW = 54°C in an insulated container. You add ice at TI = -21°C to the container and the mix reaches a final, equilibrium temperature of Tf = 25°C. The specific heats of ice and water are cI = 2.10×103J/(kg⋅°C) and cW = 4.19×103 J/(kg⋅°C), respectively, and the latent heat of fusion for water is Lf = 3.34×105 J/kg. (11%) Problem 7: Initially you have mw = 3.4 kg of...
Please show the work to how you got the answer 14) of ice, initially at 0°C, are required to bring the mixture to 10°C? The specific heat of water (and tea) is 4186 J/kg K, and the latent heat of fusion of ice is 3.34 x 105 J/kg. 14) A person makes iced tea by adding ice to 1.8 kg of hot tea, initially at 80°C. How many kilograms B) 1.7 kg C) 14 kg D) 1.0 kg A) 1.2...
A beaker with negligible mass contains 0.50 kg of water at a temperature of 80 °C. How many grams of ice at a temperature of -20 °C must be dropped in the water so that the final temperature of of the system is 30 °C? (Cice = 2100 J/ (kg °C) ), Cwater = 4190 J/ (kg °C) ), LF = 3.33 x 105 J/kg Could you also show how LF is used?
Four ice cubes at exactly 0 ∘C with a total mass of 52.0 g are combined with 155 gof water at 90 ∘C in an insulated container. (ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C) If no heat is lost to the surroundings, what is the final temperature of the mixture?
Four ice cubes at exactly 0 ∘C with a total mass of 54.0 g are combined with 125 g of water at 75 ∘C in an insulated container. (ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C) If no heat is lost to the surroundings, what is the final temperature of the mixture?
1) An aluminum calorimeter of mass 58 g, has 155 g water, both at a temperature of 21°C. A 108-g piece of metal originally kept in boiling water (T = 100°C) is transferred to the calorimeter. The final equilibrium temperature of the mixture is 26.6°C. Calculate the specific heat of the metal (in J/kg). Specific Heats: Al = 900 J/kg, water =4186 J/g 2) How much heat, in kilo-joules, is required to convert 19 g of ice at -13°C into...
Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g are combined with 130 g of water at 75 ∘C in an insulated container. (ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C) If no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using two significant figures.
Three 101.0-g ice cubes initially at 0°C are added to 0.820 kg of water initially at 19.5°C in an insulated container. (a) What is the equilibrium temperature of the system? °C (b) What is the mass of unmelted ice, if any, when the system is at equilibrium? kg
1. 0.25-mol ice at -5 °C is mixed with n-mol hot water initially at 45 °C in an isobaric adiabatic calorimeter at 1 atm. The final temperature of the mixture becomes 10 °C, and the ice is melted into liquid water. Assume the density of ice is 0.917 g/mL and the density of water is 1.000 g/mL. The molar heat capacity Com of liquid water is 75.291 J/mol K, the molar heat capacity Cm of ice is 38.09 J/mol-K, and...