Question

In: Chemistry

Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g are combined...

Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g are combined with 120 g of water at 75 ∘C in an insulated container. (ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C) 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.

Solutions

Expert Solution

no of moles of ice = W/G.M.Wt   = 53.5/18   = 2.97moles

heat lose of hot water                     =       heat gain of ice

mct                                            = ΔH∘fus*no of moles + mct

120*4.18*(75-t2)                            = 6020*2.97+53.5*4.18*(t2-0)

                          t2                            = 27C0   >>>>>>answer


Related Solutions

Four ice cubes at exactly 0 ∘C with a total mass of 51.5 g are combined...
Four ice cubes at exactly 0 ∘C with a total mass of 51.5 g are combined with 130 g of water at 85 ∘Cin 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?
Ice cubes at 0 c are poured into a glass that contains 150 g of liquid...
Ice cubes at 0 c are poured into a glass that contains 150 g of liquid water at 20 c. The contents of the glass are gently stirred and after short time the ice melts and the liquid cools to 0 c. No appreciable heat exchange with the environment takes place. a) calculate the entropy change of the universe (system plus environment) during the process. Cp=Cv = 4.18 kj/kgK b)if the same process were performed reversibly, how much useful work...
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
Given 319.5 g of hot tea at 72.0 ∘C, what mass of ice at 0 ∘C...
Given 319.5 g of hot tea at 72.0 ∘C, what mass of ice at 0 ∘C must be added to obtain iced tea at 13.5 ∘C? The specific heat of the tea is 4.18 J/(g⋅∘C), and ΔHfusion for ice is +6.01 kJ/mol.
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.
Two 20.0-g ice cubes at –21.0 °C are placed into 225 g of water at 25.0...
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.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT