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- 1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change to decompose 1.00 mol of HgO(s) to O2(g) and Hg(l)? 3633 kJ −90.8 kJ 90.8 kJ 363.3 kJWhat is the major organic product of the following reaction? H,0/ heat HO2C. .co.CH .co.H HO,C HO HOC (A) (В) (C) (D)Which of the products in the reaction below is the predominant product? CH3 H,SO4 -OH heat (1) (2) (3) (4) Product (1) oa. ob. Product (2) Product (3) C. Product (4) od.
- a) 4-Pentenoic acid + H, KMn04 / OH B 0-10°C NaBH4 b) CH,=CH-CH,-CH,-C -Co,H Mg Co c) 5-Chloro-1-pentene Etz0 Br2 Na,Cr0, d) Toluene CH;Br H3o*, heat F CyH-Bro Fe Na,Cr,0, H30*, heatC+½ 020l co CO (s) 2 (g) CO+ 2 02(a) (g) AH = - 111 kJ %3D CO, 2 (g) Is this reaction endothermic or exothermic? (g) AH = - 394 kJ %3D -11 K3+(-394 C6st O2 (9)-yCO26) AH=-505 KJ Exothermic 2. a) Explain how AT would be affected if a greater amount of surrounding solvent (water) is used, assuming the mass of salt remains constant? b) Explain how qien would be affected if a greater amount of surrounding solvent (water) is used? Explain. If the following enthalpies are known: AH = - 95KJ 2 C+D A+2B- C) AH = + 50kJ B+XCalculate AHo for the reaction: 20:Helg) + 70:(g) 4 CO(g) + 6 H2O(g) If. C:Halg) + 302(g)-2 COg) + 2 H2O (g) CaHi(g) + Hz(g) - CzHs(g) H2(g) + % Oz(g) - H2O(g) AH = -1323 kJ AH =-137 KJ AH = -242 kJ
- H2SO4 + 2 KOH→ 2H2O + K2SO4; A) Determine the moles of KOH needed to react with 5.5 moles of H2SO4. B) Determine the moles of H2O produced from 5.5 moles of H2SO4.Name: m NetID: 17. Given the following set of reaction data, H2 (8) + 02(8) –H,O(1) 2B(s) +3H2(g) → B,H6(g) 2B(s) + O2(g) – B,O3(s) AH = -285.83 kJ mol-1 AH= 36.4 kJ mol- AH = –1273.5 kJ mol¬1 wilc pd mol determine the heat of reaction (in kJ mol¯l) for the following reaction. B2H, (g) + 302(8) B2O3(s) + 3H2O(1) lo sb 1ooleps laoin bss jo bra usido AH = ? kJ mol-1 s 26 air jes o s be noi A: -2167 s heet tGive the missing reactant: CO₂CH3 A | O A. I O B. II O C. III O D. IV + [ ² ] ? || heat 4 CO₂CH3 IV
- Q4. Another way to calculate AH values that cannot be measured experimentally is with standard heats of formation. a) Using the AH;° values provided, calculate AHrxn for NaC2H3O2(s) +3 H20(1) → NaC2H3O2 3H20(s) with the equation: ΔΗΜΟΣn, ΔΗΡ(products) -Σ n, ΔΗΡ(reactants) NaC;H3O2(s) NaC2H3O2 3H2O(s) H2O(1) AH (kJ/mol) - 708.8 - 1604 - 285.8at 25oC, Ka for aspirin (C9H8O4) is 3.0 x 10-4. Calculate Δ Go (kJ/mol) for the reaction: C9H8O4(aq) + H2O(l) = H3O+(aq) + C9H7O4-(aq)Give the organic product formed. x. d OA. I OB. II O C. III O D. IV heat 11 H H x x xB H ? ||| IV