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- [References] Calculate AH for the reaction: 2NH3 (g) + O2(g) → N2H4 (1) + H2O(1) given the following data: 2NH3 (g) + 3N2O(g) → 4N2(g) + 3H2O(1) AH =–1010. kJ N2O(9) + ЗH2(9) — N;Ha (1) + Hа0(1) ДН %3D — 317 kJ N2H4 (1) + O2 (9) → N2(g)+2H20(1) ΔΗ--623 k.J На (9) + О2(9) — Н,0(1) AH = -286 kJ ΔΗ- kJ Submit Answer Try Another Version 3 item attempts remainingWrite a balanced chemical equation for the reaction that occurswhen (a) titanium metal reacts with O2(g); (b) silver(I)oxide decomposes into silver metal and oxygen gas whenheated; (c) propanol, C3H7OH(l) burns in air; (d) methyltert-butyl ether, C5H12O(l), burns in air.Chemists working with fluorine and its compounds some- times find it helpful to think in terms of acid-base reac- tions in which the fluoride ion (F¯) is donated and ассеpted. (a) Would the acid in this system be the fluoride donor or fluoride acceptor? (b) Identify the acid and base in each of these reactions: CIF;O2 + BF; CIF,O, · BF, -- TiF, + 2 KF – K2[TiF,]
- 18. (a) Molecule N₂H4 (1) + 2 H₂O2 (1) → N2(g) + 4 H₂O (1) Complete the following table: Lewis Dot Structure (use dots or lines to show bonds) (b) (c) (d) N₂H4 H₂O2 N₂ H₂O Calculate the AH°rxn using average bond energies (Table 9.4 in textbook) Calculate the AH°rxn using the standard enthalpies of formation (Appendix 2 in textbook) Why are these two values slightly different?The lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859 by French physician Gaston Plante and still retains application todaY, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H, SO,() – SO;(9) + H,O() AH-+113. kJ In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb(s) – PbO,(s) - 2 S0, (g) → 2 PbSO,(s) AH= -775. J Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ.2. An experiment was carried out to determine the enthalpy change of combustion of propan-1-ol. The experimental set-up was shown below. a beaker water (500.0 cm³) propan-1-ol (a) Write the equation for the complete combustion of propan-1-ol (C;H¬OH). (b) Give a suggestion to the above set-up so as to minimize heat loss to the surroundings. (c) Burning 2.88 g of propan-1-ol caused the temperature of 500.0 cm³ of water to rise by 46.0°C. Calculate the enthalpy change of combustion of propan-1-ol. (Assume that the specific heat capacity and the density of water are 4.2 J g- K-l and 1.0 g cm- respectively.) (Molar mass of propan-1-ol: 60 g) -3 (d) The enthalpy change obtained in (c) cannot be called as 'standard enthalpy change'. Explain why.
- 9-3. Find the enthalpy change for this reaction using the data below. Clearly show how you got the answer. 2 Al(s) + 3 Ch (g) →2 AICI, (s) Data: (a) 2 Al(s) + 6 HCI(aq) 2 AICI;(aq) + 3 H2(g) AH = - 1049 kJ (b) AICH(s) AlCl3(aq) AH = -323 kJ (c) H2(g) + C2(g) 2 HCl(g) AH = - 185 kJ (d) HCl(aq) HCKG) AH = +74.8 kJThe bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction involved is the oxidation of hydroquinone by hydrogen peroxide to produce quinone and water: CоHа (ОН)2 (ад) + H202(аg) — СөН, О2(ад) + 2H2О() Calculate AH for this reaction from the following data: CвНа (ОН)2(аq) — СеH4О2(ад) + H2(9) ДН — 177.4 kJ H2 (g) + O2 (g) → H2O2(ag) AH = -191.2 kJ H2 (g) + 02 (g) → H2O(g) AH = -241.8 kJ H2O(g) → H20(1) AH = -43.8 kJ ΔΗ kJTo further investigate the reactivity of silver, the student submerges a piece of metallic scandium, Sc (s), in a solution of AgNO3 (aq) and observes that the following reaction occurs. Sc(s) + 3 AGNO3 (ag) →3 Ag(s) + Sc(NO3); (aq) (k) Write the balanced net-ionic equation for the reaction. B IU x² X, 3 Ĉ Ω 0/10000 Word Limit
- [References] Carbon dioxide from the atmosphere "weathers," or dissolves, limestone (CaCO3) by the reaction CACO3 (s) + CO2(9) + H2O(1) → Ca²* (ag) + 2HCO;¯(ag) Obtain AH for this reaction using the following data: AĦ;(CaCO3 (s)) = -1206.9 kJ/mol %3D AH;(CO2(9)) = -393.5 kJ/mol AH;(H20(1)) = –285.8 kJ/mol AH;(Ca* (aq) =-542.8 kJ/mol %3D AH; (HCO; (ag) = -692.0 kJ/mol AH kJ Submit Answer Try Another Version 6 item attempts remaining Visited5 ml of a 0.2 M NH3 solution are added to 5 ml of a 0.1 M NH4Cl solution (Kb for NH3 is = 1.8 × 10-5). Calculate: a) the pH of the resulting solution; b) the ΔpH due to the addition of 5 ml of a 0.01 M HNO3 solution to the solution resulting from part a); c) the ΔpH due to the addition of 10 ml of water to the solution resulting from part a)Write the expression Kc for the following reactions. (a) Fe2+(aq) + Ce4+(aq) ⇋ Fe3+(aq) + Ce3+(aq) (b) CaCO3(s) ⇋ CaO(s) + CO3(g)
