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- Given the following information, Calculate delta G(degree). Give your answer in kJ. 3Ag+ (aq) + Cr (s) → 3 Ag (s) + Cr3+ (aq) __________________________________________ Ag+(aq) + 1 e- → Ag (s) 0.80 V Cr3+(aq) + 3 e - → Cr (s) -0.74 VFor a redox reaction, when Ecell∘ > 0, then _____________ A) the reactants are less abundant than the products in the equilibrium mixture. B) the reaction is spontaneous under both standard and nonstandard conditions. C) K < 1 D) Δ?∘ΔG∘ > 0Calculate the standard free-energy change and theequilibrium constant Kp for the following reaction at 25°C. CO(g) + 3H2(g) <----> CH4(g) + H2O(g)
- DeltaH=21 T=21.2 degrees C DeltaS= 0.071 Is the dissolution process studied today, NaNO3 (s) → Na+ (aq) + NO3– (aq) spontaneous or nonspontaneous? How can you tell? What is the sign of ∆G? 2. Using the class’s mean value for ∆H, and the Gibbs-Helmholtz equation, estimate the value for ∆S for the dissolution process. 3. Based on your observation about the spontaneity of the reaction and the sign of ∆H, is the value of ∆S that you calculated a minimum or a maximum? Explain. 4. Looking at the chemical equation above, would you predict that the sign of ∆S for the dissolution process is positive or negative? Explain. 5.Does the sign of your calculated entropy change agree with your prediction in question 4?If not, give a possible explanation. 6.Is a spontaneous process necessarily exothermic? Give examples to support your answer.Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. Substance ΔG°f(kJ/mol) M2O(s) −8.40 M(s) 0 O2(g) 0 M2O(s)↽−−⇀ 2M(s)+12O2(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? Δ?∘rxn= kJ/mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? ?=What is the entropy at SATP of a reaction where ∆Hºrxn=12.5 kJ and Keq=32.1?
- Using any data you can find in the ALEKS Data resource, calculate the quilibrium constant K at 25.0°C for the following reaction. Fe2O3(s)+ 3H2(g)→ 2Fe(s)+ 3H2O(l) Round your answer to 2 significant digits. delta G of Fe2O3=-742.2 kj/mol h2=0 Fe=0 H20=-237.1kj/mola) calculate deltaS surr for the following reaction: CO(g)+ 2H2(g)= CH3OH(liq) occurring at 1 atm and 298.0 K. deltaH is -128.2 kJ/mol b) What is the sign of deltaS standard rxn c) What is the deltaS univ, describe how you got the sign1. Which of the following is consistent with a spontaneous process in the forward direction? a.ΔSuniverse < 0, ΔG > 0 b.ΔSuniverse > 0, ΔG > 0 c.ΔSuniverse < 0, ΔG < 0 d.ΔSuniverse > 0, ΔG < 0 2. Using the thermodynamic data provided below, calculate the standard change in entropy when one mole of sodium sulfate is dissolved in water. Calculate the ΔGo and predict whether the solubility of sodium sulfate increase or decrease if the temperature of the system is increased? a.259 kJ mol-1; solubility is unaffected by temperature b.1.03 kJ mol-1; solubility decreases with increasing temperature c.259 kJ mol-1; solubility increases with increasing temperature d. -1.03 J mol-1; solubility increases with increasing temperature
- Ag+ (aq) + Cl– (aq) → AgCl (s) Delta S = ? What is the entropy change when silver chloride form?Predict the sign of delta S and then calculate delta S for the following reaction. 2CH3OH(g)+3O2(g)---> 2CO2(g)+4H2O(g)Calcium oxide (CaO), also called quicklime is prepared by decomposing limestone (CaCO3) in a kiln at high temperature and the reaction proceeds as: CaCO3 (s) CaO (s) + CO2 (g) Given : At T= 25 °C, then T=298 K AH° +177.8 kJ/mol AS° +160.5 J/K mol Calculate Gibbs Free Energy change (AG) for the reaction. -130.0 kJ/mol -160.5 kJ/mol +130.0 kJ/mol +160.5 kJ/mol