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 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
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 °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 °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 °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 °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 –21.0 °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 −12.0 ∘C are placed into 255 gof 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.
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?
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...