minimum no. of ice piece =28 pieces
2. What is the smallest number of ice cubes at 0 deg. C, each containing one...
Approximately how many ice cubes must melt to cool 1150 milliliters of water from 29°C to 0°C? Assume that each ice cube contains 1 mole of H2O and is initially at 0°C. ∆H(fusion) = 6.02 kJ/mol; ∆H(vaporization) = 40.7 kJ/mol c(solid) = 2.09 J/g°C; c(liquid) = 4.18 J/g°C; c(gas) = 1.97 J/g°C Enter your answer numerically.
Please Help!!!! QUESTION 19 1.3 kg of ice at 0 deg C is dropped into a cooler containing 14 kg of water at 1 7 deg C. Given a latent heat of fusion of water/ice of 79.7 cal/g and a specific heat of water of 1.00 cal/g deg C, what is the final temperature of the mixture (in deg。? QUESTION 20 In a similar situation to the previous problem, what is the smallest mass of ice (in kg) at 0...
ch.11 Four ice cubes at exactly 0 ºC with a total mass of 52.0 g are combined with 135 g of water at 90 °C in an insulated container. (AH..-6.02 kJ/mol. Cwater-4.18J/ 6C) V Part A If no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using two significant figures. OVO AXT ? Given that the heat of freezing of water is-6.02 kJ/mol, that the heat capacity of H.O() is 752...
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?
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∘C with a total mass of 51.5 gg are combined with 125 gg of water at 75 ∘C∘C in an insulated container. (ΔH∘fusΔHfus∘=6.02 kJ/molkJ/mol, cwatercwater=4.18J/g⋅∘CJ/g⋅∘C) If no heat is lost to the surroundings, what is the final temperature of the mixture? Answer in Celsius
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
Two 20.0 g ice cubes at -12.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T. of the water after all the ice melts. heat capacity of H,O() heat capacity of H,O(1) enthalpy of fusion of H,0 37.7J/(mol-K) 75.3 J/(mol-K) 6.01 kJ/mol Ti = 24.99 "C Incorrect
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