When 1.4 × 105J of energy is removed from 0.9 kg of water initially at 20 ∘C will all the water freeze? The heat of fusion for water at 0 ∘C is Lf =3.35×105J/kg. The specific heat of water is c = 4180 J/kg⋅ ∘C. How much remains unfrozen?
When 1.4 × 105J of energy is removed from 0.9 kg of water initially at 20...
Determine the energy needed to change a 0.35 kg block of ice at 0 ∘C into water at 23 ∘C. The heat of fusion for water at 0 ∘C is Lf = 3.35×105J/kg. The specific heat of water is c = 4180 J/kg⋅∘C.
How much heat must be removed to completely freeze 15 kg of water initially at 95°F? For water : Cice = 2100 J kg.K Cwater = 4186 kg K Lf=3 J . 34 x 10° ke, L, = 2. 26 x 100 kg
The largest of the Great Lakes, Lake Superior, contains about 1.20 × 1016 kg of water. If the lake had a temperature of 8.98◦C, how much energy would have to be removed to freeze the whole lake at 0◦C? The specific heat of water is 4186 J/kg · ◦C and its latent heat of fusion is 3.33 × 105 J/kg. Answer in units of J.
z.hopts) How much energy(in kJ) must be removed from 71.8g of liquid water at 25.7°C to ice at -16.1°C? Given: Heat of fusion of water = 333J/g 71081 25.7--161 Ice specific heat capacity = 2.06 J/gK water specific heat capacity = 4.184 J/gK
How much heat must be removed from 456 g of water at 25.0 degree C to change it into ice at -10.0 degree C? The specific heat of ice is 2090 J/kg K. the latent heat of fusion of water is 33.5 times 10^4 J/Kg, and the specific heat of water is 4186 J/kg K.
An insulated beaker with negligible mass contains liquid water with a mass of 0.235 kg and a temperature of 67.8 ∘C . How much ice at a temperature of -21.3 ∘C must be dropped into the water so that the final temperature of the system will be 25.0 ∘C ? Take the specific heat of liquid water to be 4190 J/kg⋅K , the specific heat of ice to be 2100 J/kg⋅K , and the heat of fusion for water to...
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,...
We want to determine how much the room temperature increases when a kg of ice freezes.Suppose you have a freezer that needs 1 J of energy for every 3 J of heat it removes.How much thermal energy must be removed from 1 kg of water at room temperature? How much electrical energy is used to freeze the ice?What is the total energy, including waste heat, that is dumped into the kitchen? If the kitchen contains 40 kg of air, how...
1. How much heat is needed to raise the temperature of 3 kg of water from 20oC to 40oC? Give answer in kJ (1kJ = 1000 J) (round answer to 3 sig fig) 2. How much heat is needed to raise the temperature of 3 kg of ice from -40oC to -20oC? (round answer to 3 sig fig) Specific heat of water: C = 4180 J/kgK Specific heat of ice: C = 2090 J/kgK Specific heat of ethanol: C= 2440...
What mass of this substance must evaporate to freeze 210 g of water initially at 24 ∘C? (The heat of fusion of water is 334 J/g; the specific heat of water is 4.18 J/(g⋅K).)