Four small ice cubes (26g each) are placed in 224g of water in a container which...

Four small ice cubes (26g each) are placed in 224g of water in a container which is thermally insulated. The water is originally at 26 degrees C while the ice cubes are at -17 degrees C.

(a) What are the 3 possibilities of this system's end point?(What are the three outcomes that might happen to the ice)

(b) What is the final temperature at thermal equilibrium?

(c) If only 2 ice cubes are placed in the container, what is the final temperature?

(d)If only 1 ice cube is placed in the container, what is the final temperature?

(e) In each step b through d indicated whether any ice melts? And how much?

pls include a picture

Expert Solution

Solution in the uploaded images

genius_generous answered 2 years ago

Two 20.0g ice cubes at -15.0C re placed into 255g of water at 25.0C. a.) Calculate...

Two 20.0g ice cubes at -15.0C re placed into 255g of water at 25.0C. a.) Calculate the amount of heat required to heat to and completely melt the ice at the melting point. b.) If that heat came from the water, what temperature would the liwuid water drop to in melting ice? c.) What would the final temperature be when the water from the melted ice reached therma equilibrium with water originally in the glass?

two 20g ice cubes at -21 c are placed into 215g of water at 25 c...

two 20g ice cubes at -21 c are placed into 215g of water at 25 c assuming no energy is transfered to or from the surroundings, calculate the final temperature of the water after all the ice melts.

Two 20.0 g ice cubes at −11.0 ∘C are placed into 225 g of water at...

Two 20.0 g ice cubes at −11.0 ∘C are placed into 225 g of water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H2O(s)H2O(s) 37.7 J/(mol⋅K) heat capacity of H2O(l)H2O(l) 75.3 J/(mol⋅K) enthalpy of fusion of H2OH2O 6.01 kJ/mol Tf= ∘C

Ice cubes usually float in a glass of water. If you push the ice cubes down...

Ice cubes usually float in a glass of water. If you push the ice cubes down to the bottom of the glass (using a straw), would they cool the water more, or less, quickly? Explain.

A glass of ice water containing nine ice cubes will be colder than a similar-size glass of ice water containing only three ice cubes.

A glass of ice water containing nine ice cubes will be colder than a similar-size glass of ice water containing only three ice cubes. True False Heat is released when a liquid freezes into a solid. True False All intermolecular forces are broken when a liquid vaporizes into a gas. True False Dispersion forces result from the temporary distortion of the electron cloud in an atom or molecule which increases in magnitude with increasing size. True False Dipole-dipole forces...

Two 20.0-g ice cubes at –21.0 °C are placed into 295 g of water at 25.0...

Two 20.0-g ice cubes at –21.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. heat capacity of H2O(s) 37.7 heat capacity of H2O (l) 75.3 enthalpy of fusion of H2O 6.01

Two 20.0-g ice cubes at –19.0 °C are placed into 245 g of water at 25.0...

Two 20.0-g ice cubes at –19.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. Heat capacity of H20(s) = 37.7J/(mol*K) Heat cap of H20(l) 75.3 J/(mol*K) enthalpy of fusion of H20 = 6.01 kJ/mol

Two 20.0-g ice cubes at –16.0 °C are placed into 275 g of water at 25.0...

Two 20.0-g ice cubes at –16.0 °C are placed into 275 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. Given the Following Values: Heat Capacity of H2O (s) = 37.7 J/mol*K Heat Capacity of H2O (l) = 75.3 J/mol*K Enthalpy of Fusion of H2O = 6.01 kJ/mol

Two 20.0-g ice cubes at –20.0 °C are placed into 225 g of water at 25.0...

Two 20.0-g ice cubes at –20.0 °C are placed into 225 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.

Two 20.0-g ice cubes at –19.0 °C are placed into 215 g of water at 25.0...

Two 20.0-g ice cubes at –19.0 °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 of the water after all the ice melts.

Question