General Chemistry 4th Edition University Science Books presented by Sapling Lear

Question

General Chemistry 4th Edition University Science Books presented by Sapling Learning Map d Two 200-g ice cubes at-150°C are placed into 255 g of water at 25.0 . 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 H20(s) 37.7 J(mol K) heat capacity of HO 753Jmol-K) enthalpy of fusion of H20 6.01 kJ/mol Number o C o Previous Give Up & View Solution e Check Answer Next Exit- The heat energy. q, associated with a temperature change,aT, is related to the number of moles, n, and heat capacity, C, of the substance according to the equation For a phase change, the heat energy is related to the number of moles and latent heat of the phase change, which, in this case, is the enthalpy of fusion, dHfus by the equation To determine the final temperature of the water after all of the ice melts, Ti, calculate the heat energy needed to raise the temperature of the ice from -15.0 to 0 and the heat energy necessary for the phase change of ice to water. Then calculate the new temperature of the water sample after releasing the heat to melt the ice efore calculating the equilibrium temperature between the melted ice and the rest of the water

Explanation / Answer

heat lost by water = heat gained by ice

      nwater*cwater*DT1 = n*C*DT2 + n*DHfus + nwater*cwater*DT3

   (255/18)*75.3*(25-x) = 20*37.7*(0-(-15))+(20/18)*6.01*10^3+20*75.3*(x-0)

x= final temperature of mixture= 3.37 C

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