Problem 13.1.12 Use Figure 1.3 to predict whether each of the following compounds is considered soluble or insoluble: a. KCl b. NaNO3 c. AgCl d. BaSO4 e. Ca3(PO4)2 f. Pb(ClO3)2 g. (NH4)2S h. PbCl2 (in cold water) i. FeS j. Al2(SO4)3 Step-by-Step Solution: Step 1 of 3 2 October 2015 DeltaHof o kJ/mol o Enthalpy DeltaGo o Gibbs free energy o kJ/mol DeltaSo o Entropy o J/mol spontaneous: occurs by itself (no action from the outside system is required) o asking if spontaneous under conditions nonspontaneous - does not occur by itself (action from the system required ) Entropy (S) o a measure of chaos/disorder of a system o S increases when: solid -> liquid solid or liquid -> gas solid or liquid -> solution chemical reaction produces an increase in number of gas molecules when a substance is heated o S = k lnW k = boltzmann constant = 1.38 x qo^23 J/k Third law of thermodynamics o S of a perfect crystal at 0K = 0 S is state function o DeltaS = Sf - Si (enthalpy final minus enthalpy initial o DeltaS(rxn) = Sum of the enthalpy of the products minus sum of the enthalpy of the reactants Second law of thermodynamics o for spontaneous reactions the something of the universe must increase o entropy universe is equal to the everything idk Step 2 of 3
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