Of ice at -S °C is added to 40 kg of water initially at 20 °C. Assume that the container is well ...
Three 110.0-g ice cubes initially at 0°C are added to 0.860 kg of water initially at 21.0°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? 1 kg
A chunk of ice (T = -20 degree C) is added to a thermally insulated container of cold water (T = 0 degree C). What happens in the container? The ice melts until thermal equilibrium is established. Some of the water freezes and the chunk of ice gets larger. The water cools down until thermal equilibrium is established. None of the above things happen.
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
200 gr of water in a thermally insulated container. 200 gr of water is initially at 25 o C in a thermally insulated calorimeter. a) If 50 gr of ice at –15 o C is dropped into this calorimeter what is the final temperature after thermal equilibrium is established. b) If Instead 300 gr of ice at –30 o C is added how much ice will remain when equilibrium is reached? c) In part (a) what is the change in...
Three 110.0-g ice cubes initially at 0°C are added to 0.900 kg of water initially at 21.0°C in an insulated container. (a) What is the equilibrium temperature of the system? 9.13 Your response differs significantly from the correct answer. Rework your solution from the beginning and check each step carefully.°C (b) What is the mass of unmelted ice, if any, when the system is at equilibrium? The correct answer is not zero. kg
Problem 5 20 points You place into an insulated container a 1.5 kg of copper initially at 70°C. You add to the insulated container water, initially at 20°C to obtain a final temperature of the system equal to 50°C. The specific heat of some materials are given in the table below: Aluminum Copper Material J/g/°C Glass Gold Ice Iron Rubber Silver Water zinc 0.79 0.13 2.1 0.46 0.24 4.2 0.39 0.89 0.38 2 a) [5 points) What is the variation...
5.45 kg block of ice at 0°C is added to an insulated container partially filled with 11.9 kg of water at 15.0°C (a) Find the final temperature, neglecting the heat capacity of the container (b) Find the mass of the ice that was melted. 3.21 Your response differs from the correct answer by more than 10%. Double check your calculations. kg GETTING STARTED | I'M STUCK! EXERCISE HINTS: If 9.00 kg of ice at -5.00°C is added to 12.0 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...
1.) 40 g of liquid water at 30 C and 20 g of ice at 0 C are mixed together in an insulated container. Assuming there is not heat lost to surroundings, what will the temperature be when the mixture has reached thermal equilibrium. (show your work) 2.)20 g of ice at 0 C and 10 g of steam at 100 C are mixed together in an insulated container. Assuming there is not heat lost to surroundings, what will the...
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?