Considering each of the following values and neglecting entropy, tell whether the starting material or product is favored at equilibrium: (a) ΔHo = 80 kJ/mol; (b) ΔHo = −40 kJ/mol.
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Considering each of the following values and neglecting entropy, tell whether the starting material or product is favored at equilibrium: (a) ΔHo = 80 kJ/mol; (b) ΔHo = −40 kJ/mol.
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- For a reaction with ?H° = 40 kJ/mol, decide which of the following statements is (are) true. Correct any false statement to make it true. (a) The reaction is exothermic; (b) ?G° for the reaction is positive; (c) Keq is greater than 1; (d) the bonds in the starting materials are stronger than the bonds in the product; and (e) the product is favored at equilibrium.Which of the following statements about the reaction H2(g)+O2(g)→H2O(l)H2(g)+O2(g)→H2O(l) is true? (i) This is an example of an acid–base reaction. (ii) O2O2 is oxidized in this reaction. (iii) H2H2 is reduced in this reaction. Which of the following statements about the reaction is true? (i) This is an example of an acid–base reaction. (ii) is oxidized in this reaction. (iii) is reduced in this reaction. iii only i only ii and iii ii only None of them are true.How do I (a) determine the energy change in the following reaction2 O2 + CH4→ CO2 + 2 H2Ogiven the following bond dissociation energies:C-C 340kJ/mol; C-H 420kJ/mol; O=O 490 kJ/mol; O-H 460 kJ/mol; C=O 720 kJ/mol. (b) Is the reaction exothermic or endothermic? Explaination?
- 3 Draw labelled energy level diagrams for the following reactions: a S(s) + O₂(g) → SO₂(g) AH = -297 kJ mol-¹ b 6C0₂(aq) + 6H₂O(l) → C6H₁206(aq) + 60₂(g) AH=+2800 kJ mol-¹ C6H₁206Given: 2MNO(s) + O2(g) → 2MnO2(s) ArH = –269.6 kJ · mol-1The ΔHac of nitrogen dioxide is -937.86 kJ/mole. The ΔHf of nitrogen dioxide is +33.2 kJ/mole. Propose a reasonable explanation for this difference
- Formation of ammonia from nitrogen and hydrogen is an exothermic process. Which of the following statements is true about the bonds that are broken and formed during this reaction? N2(g) + 3H2(g) ---> 2NH3(g) a.) products have lower PE because product bonds are weaker than reactants b.) products have higher PE because product bonds are stronger than reactants c.) products have higher PE because product bonds are weaker than reactants d.) products have lower PE because product bonds are stronger than reactantsConsider the following reaction: 3 C(s) + 4 H₂(g) →→ C3H8(g) Which of the following statements is correct about this reaction? Use the following reactions and thermodynamic data: Reaction: C3H8(g) + 5 O2(g) → 3 CO₂ (g) + 4H₂O C(s) + O₂(g) → CO₂(g) 2 H₂(g) + O₂(g) → 2H₂O(g) AG=-23.4 kJ AS >0 The reaction is non-spontaneous The reaction is spontaneous not enough information is given AS <0 AG rxn (kJ) -394.4 -457.1 kDetermine, at 298 K, Δr1H0, the standard enthalpy of the reaction (1) between hydroquinone with hydrogen peroxide to produce quinone. C6H4(OH)2(aq) + H2O2(aq) → C6H4O2(aq) + 2 H2O (ℓ) (1) Knowing the standard reaction enthalpies, at 298 K, of the following reactions: (2) C6H4(OH)2 (aq) → C6H4O2 (aq) + H2 (g) ; Δr2H0 = + 177.4 kJ mol−1 (3) H2 (g) + O2 (g) → H2O2 (aq) ; Δr3H0 = −191.2 kJ mol−1 (4) H2 (g) + ½O2 (g) → H2O (g) ; Δr4H0 = −241.8 kJ mol−1 (5) H2O (g) → H2O (ℓ) ; Δr5H0 = −43·8 kJ mol−1
- The reaction of quicklime, CaO, with water produces slaked lime, Ca(OH)2, which is widely used in the construction industry to make mortar and plaster. The reaction of quicklime and water is highly exothermic: (a) What is the enthalpy of reaction per gram of quicklime that reacts? (b) How much heat, in kilojoules, is associated with the production of 1 ton of slaked lime?calculate the reaction energy of the following reactions and then determine if they are endothermic or exothermic:CH4 + 2O2 => CO2 + 2H2OUse the thermodynamic quantities given below to calculate the theoretical ΔH for this reaction: NH3 + HCl → NH4Cl ΔH°f for NH3 (aq) = - 80.29 kJ/mol ΔH°f for HCl (aq) = - 167.2 kJ/mol ΔH°f for NH4+ (aq) = - 132.5 kJ/mol ΔH°f for Cl- (aq) = - 167.2 kJ/mol I found this answer to be -52.21 kJ/mol 6. What is the percent error of experimental results when using the theoretical value calculated in Question 5? I need help finding this