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Chemistry
- Which of the following is true for a particular reaction if AG° is -40.0 kJ/mol at 290 K and -20.0 kJ/mol at 390 K? A) ΔΗ >0 , ΔS 0 Β) ΔΗ 0, AS< 0 D) ΔΗ < 0, ΔS 0 E) None of these +arrow_forwardCalculate AS° values for the following reactions by using tabulated Sº values from Appendix C. (a) 2 PCl3(g) + O₂(g) = 2 POCI3(9) As° = -178.4 ✓ J/K (b) 2 Na(s) + 2 H₂O(g) 2 NaOH(aq) + H₂(g) AS⁰ = -197.62 X J/K (c) Cl₂(g) + H₂(g) = 2 HCl(g) As° = 20.066 XJ/K (d) Be(OH)₂(s) = Be0(s) + H₂O(g) As° = 157.02 XJ/Karrow_forward19. Ammonia can be formed by the reaction of hydrogen with nitrogen gas 3H2 (g) + N2 (g) → 2NH3 (g). The value of AH° is –92.38 kJ/mol, and that of AS° is -198.2 J/mol·K. Determine AG° at 25°C. (A) -59.0 kJ/mol (B) 151 kJ/mol (C) -33.3 kJ/mol (D) -151 kJ/molarrow_forward
- c) SO d) CO 0. Sodium reacts violently with water according to the equation: 2 Na(s) +2 H;0() 2 NaOH(aq) + H:(g) resulting solution has a higher temperature than the water prior to the addition of sodium. What are the signs of AH and AS for this reaction? a) AH is negative and AS is negative. b) AH is negative and AS is positive. e) AH is positive and AS is negative. d) AH is positive and AS is positive. (END)arrow_forwardOne of the reactions that destroys ozone in the upper atmosphere is NO(g) + O3(g) ⇒ NO2 (g) + O2(g) Substance and State AGf (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate ΔG° (at 298 K) for this reaction. AG = -198 kJ b Calculate K (at 298 K) for this reaction. K =arrow_forwardQuestion 4 4.1 When 0.50 mol of an ideal gas is expanded isothermally and reversibly at 298 K from a volume of 10.0 L to 25.0 L, (a) What is the 4Sgas? (b) How much work was done? (c) What is the 4Ssurr? (d) What is the 4Stotal? 4.2 At 25.0 °C the equilibrium constant for the reaction: CO(g) + H₂O(g) = CO2(g) + H2(g) is 1.00 x 10-5, and AS° is 41.8 J K-1 mol-¹. Calculate 4Gº and AH° at 25.0 °C.arrow_forward
- Given: P4(s)+5O2(g)⟶P4O10(s) ΔG°=−2697.0 kJ/mol 2H2(g)+O2(g)⟶2H2O(g) ΔG°=−457.18 kJ/mol 6H2O(g)+P4O10(s)⟶4H3PO4(l) ΔG°=−428.66 kJ/mol Net Equation: 3/2 H2 (g) + ¼ P4 (s) + 2 O2 (g) → H3PO4 (l) Using Hess’s law to determine the standard free energy of formation, ΔG∘f, for phosphoric acid.arrow_forwardCalculate ∆G (in kJ) at 35.4oC for a reaction that has Keq = 105arrow_forwardAG° is -32.7 kJ/mol of N2 for the reaction at 100°C N2(g)+3H2(g)=2NH3(g) Calculate AG for the same reaction under the following nonstandard conditions: In which direction must the reaction proceed to reach equilibrium? [N2]= 2.00 M, [H2]= 7.00 M, [NH3] = 0.021 M, and T = 100°C. 2.arrow_forward
- Calculate the ΔGo for the following equation. Sb4O6(s) + 6C(graphite) ⟶ 4Sb(s) + 6CO(g) Group of answer choices -1131.02 kJ/mole 445.27 kJ/mole -445.27 kJ/mole -1131.02 kJ/mole 445.27 kJ/mole -445.27 kJ/mole 1131.02 kJ/mole 1131.02 kJ/molearrow_forwardThe ΔG°rxn for this reaction is -107.8 kJ/mol. Given the values for ΔGf°; what is the ΔGf° for A2B(l)? 2AC(g) + B2(g) → A2B(l) + BC2(g) Substance ΔGf° (kJ/mol) AC(g) -174.3 B2(g) 173.3 BC2(g) 169.9arrow_forwardOne of the reactions that destroys ozone in the upper atmosphere is NO(g) + O3(g) ⇒ NO2 (g) + O2(g) Substance and State AGf (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate AG (at 298 K) for this reaction. ΔG° kJ Submitarrow_forward
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