Calculate the change in enthalpy for the reaction (?Hrxn) per mole using equation 8 and Table 2. Is this an exo- or endothermic reaction? Explain the reasoning behind your choice. If the heat capacity of the calorimeter was 25 J/oC, what would the new change in enthalpy (?Hrxn) for this reaction be? (Use equation 7 to recalculate the value from #10) _ kJ/mol ? [Equation 7: - q(rxn) = q(soln) + q(calorimeter)ġ4. What happens is that one or more of the ligand water molecules get replaced by a negative ion in the solution - typically sulphate or chloride. Calculate the heat of reaction in kJ per mole of NH4NO3 _ kJ/mol ?ġ3. Calculate the change in enthalpy (?Hrxn) for this reaction. the heat either released or absorbed by the reaction (?Hrxn) _+752.4_ Jġ1. ![]() calculate the heat associate with water, qH2O _ _-752.4_ J All the three complexes have water and chloride ion as ligands. change in temperature of the water (?T) -3.6 Â☌ĩ. Calcium chloride (exothermic) and ammonium chloride (endothermic) are added to water. Initial temperature of water, Ti 22.5Â☌Ħ. Replacement of the water by sulfate ions You can do this simply by warming some chromium (III) sulfate solution. Complete and balance the following chemical reaction: NH4NO3(s) + H2O(l) -> ?Ĥ. What happens is that one or more of the ligand water molecules get replaced by a negative ion in the solution typically sulfate or chloride. Calculate the Heat of Solution in both per mole (Molar Heat of solution) and per gram (Gram Heat of Solution).ġ. Press Tab to enter the content editor.Ĥ) The solid in question #2 and #3 was aluminum sulfate, Al2(SO4)3. Recalculate the heat released including the correction for the calorimeter. Calculate the heat released as the solid dissolved, assuming no heat lost to the calorimeter.ģ) The calorimeter in #2 was found to have a heat capacity of 8.20 J/Â☌. The final temperature of the solution was 25.3Â☌. Cl 35.5 g/mol NaCl 23.0 g/mol + 35.5 g/mol 58.5 g/mol Total number of moles (1 mole / 58.5 g) 6 g 0.62 moles Now determine moles per liter of solution: M 0.62 moles NaCl / 0. Which is strongerâthe attractive forces between the water molecules and the individual chromium and chloride ions, or the combination of the ionic bond strength of CrCl2 and intermolecular forces between water molecules? Explain.Ģ) A solution was formed by combining 25.0 g of solid A with 60.0 ml of distilled water. Is the heat of solution exothermic or endothermic?Ĭ. ![]() Describe the direction of the heat transfer.ī. ![]() When chromium chloride, CrCl2, is dissolved in water, the temperature of the water decreases.Ī.
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