50. Using bond energies given in Table 1 on page 307, determine the enthalpy change for the reaction given by the following balanced chemical equation: (5.3) mm H,(g) + Cl,(g)→ 2 HCI(g)
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- Ozone, O3(g)O3(g), is a form of elemental oxygen that is important in the absorption of ultraviolet radiation in the stratosphere. It decomposes to O2(g)O2(g) at room temperature and pressure according to the following reaction: 2O3(g)→3O2(g)ΔH=−284.6kJ What is the enthalpy change for this reaction per mole of O3(g)O3(g)?A piece of parmesan cheese is burned in a soda can calorimeter, and heats up 0.235 kg of water by 2.85 °C. The calorimeter was calibrated and had a calorimetry constant of 8.50 kcal/kg・°C. Given that protein contains 4.00 kcal/g, calculate the mass in g of the protein contained in the parmesan. Assume that the cheese is composed primarily of protein.2. Calcium carbide, CaC2, is the raw material for the production of acetylene (used in welding torches). Calcium carbide is produced by reacting calcium oxide with carbon. Carbon monoxide is also produced in this reaction. When one mole of calcium carbide is formed, 464.8 kJ is absorbed (a) Write a thermochemical equation for this reaction.(b) Is the reaction exothermic or endothermic?(c) What is ΔH when 1.00 g of CaC2(s) is formed?(d) How many grams of carbon must react to produce 3.03x103 kJ of heat?
- d) Given the following data, calculate the enthalpy change for the formation of 60 g of heptane, C7H16. 7 C (s) + 8 H2 (g) —> C7H16 (g) C7H16 (g) + 11 O2 (g) —> 7 CO2 (g) + 8 H2O (l) ∆??? = -6230.0 kJ/mol C (s) + O2 (g) —> CO2 (g) ∆??? = -393.5 kJ/mol H2 (g) + ½ O2 (g) —> H2O (l) ∆??? = -285.8 kJ/molWhen 0.776g of sodium metal is added to an excess of hydrochloric acid, 8070 J of heat are produced. What is the enthalpy of the reaction as written? 2Na(s) +2HCI(aq) --->2NaCl+H2(g) Enthalpy of reacyion in kJ ?If the complete reaction of 45.0 g of B(s) requires 74.93 kJ of heat to be absorbedfrom the surroundings, what is the enthalpy change of the following equation in kJ/mol rxn? 2B(s) + 3H2(g) -> B2H6 (g) ∆H rxn = ? kJ/molrxn
- When 0.638 of sodium metal is added to an excess of hydrochloric acid, 6630j of heat are produced. What is the enthalpy of the reaction as written? 2Na(s)+2HCl(aq)⟶2NaCl(aq)+H2(g) Enthalpy of reaction:When 2 moles of H2S(g) react with O2(g) to form H2O(l) and SO2(g) according to the following equation, 1.12×103 kJ of energy are evolved. 2H2S(g) + 3O2(g)---->2H2O(l) + 2SO2(g) Is this reaction endothermic or exothermic? _________(endothermic or exothermic)What is the value of q? ________kJThe same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O in Joules? What is qdissolution in Joules? What is the ΔHdissolution in kilojoules per mole? Is the reaction endothermic or exothermic?
- Oxygen difluoride reacts with water vapor to produce 318 kJ of heat by the following equation: OF2 (g) + H2O (g) → 2 HF (g) + O2 (g) Calculate ΔHo of OF2 in kJ/mol for the reaction below.Nitroglycerin, C3H5(NO3)3(l), is an explosive most often used in mine or quarry blasting. It is a powerful explosive because four gases (N2, O2, CO2, and steam) are formed when nitroglycerin is detonated. In addition, 6.26 kJ of heat are given off per gram of nitroglycerin detonated. (a) Write a balanced thermochemical equation for the reaction. (b) What is H when 4.65 mol of products are formed?Methane (CH4) burns according to the equation CH4 (g) + 2 O2(g) ➞ CO2(g) + 2 H2O(l) with the liberation of 990 kJ per mole of methane reacted. How many grams of oxygen must react with methane in order to release 1780 kJ of energy?