delta S of the reaction = delta S of the products - delta s of the reactants
Part A
delta S of the reaction = [96.2 J/mol K] - [72.7 J /mol K + 56.5 j/mol K]
= -33 J/mol K
Part B
delta S of the reaction = [3 (213.6 J /mol -K) + 4(4 69.9 J / mol-K) ] - [269.9 J / mol K +205.0 J / mol K]
delta S of the reaction = [640.8 J /mol K + 1879.6 J / mol K] - [474.9 J/mol K]
delta S of the reaction = 2045.5 J/mol K
Part C
delta S of the reaction = [94.6 J/mol K ] - [192.3 J/mol K + 186.8 J/mol K]
delta S = -284.5 J/mol K
Use the standard molar entropies to calculate Delta Sdegree_rtimes n for the following reactions: Ag^++(aq) +...
For which of the following processes would Delta S degree be expected to be most positive? a) O_2(g) + 2H_2(g) rightarrow 2 H_2O(g) b) H_2O(l) rightarrow H_2O(s) c) NH_3(g) + HCl(g) rightarrow NH_4Cl(g) d) 2NH_4NO_3(s) rightarrow 2 N_2(g) + O_2(g) + 4H_2O(g) e) N_2O_4 rightarrow 2NO_2(g)
Calculate the standard molar entropies at 25 oC for the following reactions. 2CH_4(g) + O_2(g) right arrow 2 CH_3OH(I) 4 Al(s) + 3 O_2(g) right arrow Al_2O_3(s)
What molar ratio Write a balanced chemical equation which corresponds to the following equilibrium constant question K = [NO^-_2] [H_3O^+]/[HNO_2] HNO_2(aq) + H_2O(l) NO^-_2(aq) + H_3O^+(aq) NO^-_2(aq) + H_3O^+(aq) HNO_2(aq) + H_2O(l) NO^-_2 (aq) + H_3O^+(aq) HNO_2(aq) + H_2O(l) NO^-_2 (aq) + H_3O^+(aq) HNO_2(aq) H^+(aq) + OH^-(aq) H_2O(l) HNO_2(aq) NO^-_2 (aq) + H_3O^+(aq) For the equilibrium PCl_5(g) PCl_3(g) + Cl_2(g), K_c = 4.0 at 228 degrees C. If pure PCl_5 is placed in a 1,00-L container and allowed to come...
Given reactions 1 and 2 below, calculate delta H degree_Rxn and delta U degree_Rxn for reaction 3. Rxn 1 H_2(g) + I_2(s) rightarrow 2 HI(g) delta H degree_Rxn = +52.96 kJ/mol Rxn 2 2H_2(g) + O_2(g) rightarrow 2 H_2 O(g) delta H degree_Rxn = -483.64 kJ/mol Rxn 3 4 HI(g) + O_2(g) rightarrow 2 I_2(s) + 2 H_2O(g) delta H degree_Rxn = ? delta U degree_Rxn = ?
To decide whether AgCl should dissolve in water ( spontaneous reaction ) at 25 degrees celcius, the delta H and T delta S must be used in the Gibbs Free Energy equation to calculate delta G AgCl (s) + H2O (I) -> Ag+ + Cl- + H2O Standard Enthalpies of formation and standard entropies of common compounds substance state AgCl s -127010 96.20 Cl- aq -167080. 56.50 Ag+ aq. 105790. 72.70
Use data from Appendix C to calculate Delta G degree for the combustion of methane. CH_4(g) + 2 O_2 (g_ rightarrow CO_2(g) + 2 H_2O(g)
Consider the following reaction: Ca(s) + 2 H_2O(l) rightarrow Ca(OH)_2(s) + H_2(g) Calculate the heat of reaction based on the following information: 2H_2(g) + O_2(g) rightarrow 2 H_2O(l) DeltaH = -572 kJ/mol CaO(s) + H_2O(l) rightarrow Ca(OH)_2(s) DeltaH = -64 kJ/mol CaCO_3(s) rightarrow CaO(s) + CO_2(g) DeltaH = +178.1 kJ/mol 2 Ca (s) + O_2(g) rightarrow 2 CaO(s) DeltaH = -1270 kJ/mol 13. Acetylene is used in blow torches, and bums according to the following equation: 2 C_2H_2(g) + 5...
Calculate the enthalpy of formation of SO_2(g) from the standard enthalpy changes of the following reactions: SO_2(g) + O_2(g) rightarrow 2 SO_3(g) Delta H degree _r times n = - 196 kJ S(s) + 3 O_2(g) rightarrow 2 SO_3(g) Delta H degree _r times n = - 790 kJ S(s) + O_2(g) rightarrow SO_2(g) Delta H degree _r times n = Number _______ kJ
Calculate the standard change in free energy (Delta G degree) for the following redox reaction: Ag^+ (aq) + Sn (s) rightarrow Ag (s) + Sn^2+ (aq)
Classify the following reactions as either: combination, decomposition, combustion, precipitation (metathesis) or redox reactions. C(s) + 4 HNO_3 (aq) rightarrow 4 NO_2 (g) + 2 H_2 O (I) + CO_2 (g) HCI (aq) + NH_3 (aq) rightarrow NH_4 CI(aq) 2HI (g) rightarrow H_2 (g) + I_2 (g) Cu(NO_3)_2 9aq) + Na_2 S (aq) rightarrow CuS(s) + 2 NaNO_3 (aq) Zn(s) + 2 AgNO_3 (aq) rightarrow Zn(NO_3)_2 (aq) + 2 Ag(s) H_2 SO_3 (aq) + 2 KOH(aq) rightarrow K_2 SO_3 (aq)...