Question

Test Tube 1: Draw an energy diagram of the process and label the energy changes including the enthalpy of solution. -5.anL of d;Stile water nCl2 .5 cacle in AX 27Cterf 26 2 5 min 23'c terr 20 23 As you draw the energy diagram, consider the entire solvation process as a series of steps. Name the strongest attractive forces that exist in the 1) solid and 2) liquid that must be broken? 1) Will breaking these forces be an endothermic or exothermic process?endothesmk Name the attractive force (IPF) that is being created?n-dpole force 4) 2) 2) 3) Will this step be endothermic or exothermic? 5) Was the enthalpy of solution (the overall energy change) endothermic or exothermic? (Optional question) Use the calorimetry equation to calculate the energy of solution for calcium chloride. You will need the following values: mass of the water in the test tube (assume a density of 1.00 g/mL) temperature change of the water Specific heat capacity of water (4.184 J/g * C) Moles of calcium chloride dissolved You are looking for an energy change with units of J/mol Write an equation for the process that took place in test tube 1 and include the energy term with the correct sign. Test Tube 2: Draw an energy diagram of the process and label the energy changes including the enthalpy of solution. Write the equation for the process that took place in test tube 2. Make sure it has the correct mass and charge balance and it reflects the net change that took place. Add "energy" to the appropriate side of the equation. (Optional question -if Gibbs free energy was covered) What allows this process to occur spontaneously when it is increasing the potential energy of the system? What other term is increasing that compensates for the increase in energy? Explain why this increases when a solution is formed.

I dont need help with test tube 2, only one im having trouble with it. I dont under really what to do for the optional part.

Answer 1

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