Practice ProblemATTEMPT
Will the following reaction occur spontaneously at
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- Calculate the equilibrium constant at 25 C for each of the following reactions from the value G given. (a) I2(s)+Cl2(l)2ICl(g)G=10.88kJ (b) H2(g)+I2(s)2HI(g)G=3.4kJ (c) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)G=39kJ (d) 2SO2(g)+O2(g)2SO3(g)G=141.82kJ (e) CS2(g)CS2(l)G=1.88kJarrow_forwardEstimate ΔrG° at 2000. K for each reaction in Question 60.arrow_forwardCalculate E°, G°, and K at 25°C for the reaction 3Mn2+(aq)+2MnO4(aq)+2H2O5MnO2(s)+4H+(aq)arrow_forward
- Calculate E°, G°, and K at 25°C for the reaction 3MnO4(aq)+4H+(aq)+Cl2(g)2Mn2+(aq)+2ClO3(aq)+2H2Oarrow_forwardWithout doing any calculations, predict the sign of rS for the following reaction: Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g) (a) rS 0 (b) rS = 0 (c) rS 0arrow_forwardThe Ksp for a very insoluble salt is 4.2 x 10-47 at 298 K. Whatis ΔG° for the dissolution of the salt in water?(a) -265 kJ/mol (b) -115 kJ/mol (c) -2.61 kJ/mol(d) +115 kJ/mol (e) +265 kJ/molarrow_forward
- Consider the following reaction at 298 K. Cd²+ (aq) + Cu(s) → Cd(s) + Cu²+ (aq) Cd2+ (aq) + 2e → Cd(s) Fre = -0.403 V Cu2+ (aq) +2e → Cu(s) Ee = = 0.337 V red Which of the following statements are correct? (Select all that apply.) On - 2 mol electrons OK >1 The reaction is reactant-favored. OE <0 cell DAG <0 Submit Answer Retry Entire Group 7 more group attempts remainingarrow_forwardCalculate AG°ran for the following reaction of white phosphorous with HCl. 2P (s) + 10HC1 (g)→ 2PCI5 (g) + 5H2 (g) AGʻfof P(s) = 0 KJ/mol AG†of HCl (g) = -95.3 KJ/mol AG°fof H2 (g) = 0 KJ/mol AGʻfof PCI5(s) = -305.0 KJ/molarrow_forwardConsider the following reaction at 298 K. 2+ Pb²+ (aq) + I (aq) → Pb(s) + I₂ (s) Pb²+ (aq) + 2e¯¯ → Pb(s) Ee 2+ red I₂ (s) +2e → I¯ (aq) Eº red -0.126 V = 0.535 V Which of the following statements are correct? (Select all that apply.) AG° <0 The reaction is product-favored. OK <1 On = 2 mol electrons Eº <0 cellarrow_forward
- Corrosion of Fe to its oxides (e.g. Feo, Fe>0a) in moist air is an example of a spontaneous process with negative AG and which requires no added work for the reaction to proceed forward. Select one: O True O Falsearrow_forwardCalculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given.(a) I2(s) + Cl2(g) ⟶ 2ICl(g) ΔG° = −10.88 kJ(b) H2(g) + I2(s) ⟶ 2HI(g) ΔG° = 3.4 kJ(c) CS2(g) + 3Cl2(g) ⟶ CCl4(g) + S2 Cl2(g) ΔG° = −39 kJ(d) 2SO2(g) + O2(g) ⟶ 2SO3(g) ΔG° = −141.82 kJ(e) CS2(g) ⟶ CS2(l) ΔG° = −1.88 kJarrow_forward16) The equilibrium constant for the following reaction at 298 K is Kc=9.1x10−6.2Fe3+(aq) + Hg22+(aq) <--> 2Fe2+(aq) + 2Hg2+(aq)a) What is ΔG° at this temperature?b) If standard-state conditions of the reactants and products are mixed, in which direction does the reaction proceed? c) Calculate ΔG when [Fe 3+]=0.20 M, [Hg22+]=0.010 M, [Fe2+]=0.010 M, and [Hg2+]=0.025 M. In which direction will the reaction proceed to reach equilibrium?arrow_forward
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