A 20.0-g sample of ice at 210.0oC is mixed with 100.0 g of water at 80.0oC. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 Jg-1oC-1 and 4.18 Jg-1oC-1, respectively, and the enthalpy of fusion for ice is 6.01 kJ/mol.
Answer to relevant QuestionsAn ice cube tray contains enough water at 22.0oC to make 18 ice cubes, each of which has a mass of 30.0 g. The tray is placed in a freezer that uses CF2Cl2 as a refrigerant. The heat of vaporization of CF2Cl2 is 158 J/g. ...The critical point of NH3 is 132oC and 111 atm, and the critical point of N2 is –147oC and 34 atm. Which of these substances cannot be liquefied at room temperature no matter how much pressure is applied? Explain. Consider the following data for xenon: Triple point: ...... –121oC, 280 torr Normal melting point: ... –112oC Normal boiling point: ... –107oC Which is more dense, Xe(s) or Xe(l)? How do ...Consider a cation in a trigonal hole. What size ion will just fit in the hole if the packed spheres have radius R? Which ion in each of the following pairs would you expect to be more strongly hydrated? Why? a. Na+ or Mg2+ b. Mg2+ or Be2+ c. Fe2+ or Fe3+ d. F- or Br- e. Cl- or ClO4- f. ClO4- or SO4 2-
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