+ + 1. Using two or more of the following. N.(g) lo.(g) → N.O.(a) AH-83.7 kJ N.(g) O(g) → 2NO(g) AH 180.4 kJ IN.(g) + O.(g) → NO.(g) AH = 33.2 kJ IN(9) H.(g) → NH(g): AH = 45.9 kJ + determine AH for the following reaction. NO(g) + NO:(g) → N₂O(g)

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Ignition wires heat sample Water Stirrer Thermometer Insulated Sample Burning Steel outside dish sample bomb chamber Combustion (bomb) calorimeter. In an experiment, a 0.4370 g sample of benzoic acid (CH6O₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.043 x 10³ g of water. During the combustion the temperature increases from 22.78 to 25.08 °C. The heat capacity of water is 4.184 J-g¹. C¹. The heat capacity of the calorimeter was determined in a previous experiment to be 893.1 J. "C Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of benzoic acid based on these data. CHO₂(8)+(15/2)O₂(g) → 3H₂O(l) +7C0₂ (9) + Energy Molar Heat of Combustion= kJ/mol

A)When 1 mole of CO(g) reacts with Cl2(g) to form COCl2(g) according to the following equation, 108 kJ of energy are evolved. CO(g)+Cl2(g)---->COCl2(g) Is this reaction endothermic or exothermic? What is the value of q? ---- kJ   B) When 2 moles of H2S(g) react with O2(g) to form H2O(g) and SO2(g) according to the following equation, 1.04×103 kJ of energy are evolved. 2H2S(g)+3O2(g)----->2H2O(g)+2SO2(g) Is this reaction endothermic or exothermic?  What is the value of q? ------ kJ

Calculate AH for the following reaction, given the data in the table below: H2SO4(1) → SO3(g) + H2O(g) AH = ??? kJ/mol H2S(g) + 202(g) → H2SO4(1) AH = -698.0 kJ H2S(g) +202(g) → SO3{g) + H2O(1) AH = -203.0 kJ H2O(1) → H2O(g) AH = +29.32 kJ

Consider these reactions: AH = -184.6 kJ Reaction 1: H₂(g) + Cl₂ (g) → 2HCl(g) Reaction 2:20F2 (g) O2(g) +2 F2 (g) AH = -49.4 kJ Reaction 3: N₂(g) + 2O2(g) → 2NO2(g) AH = +66.4 kJ Use Reaction 1. Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,891.0 kJ of energy is released from the system. Answer: g (mass must be positive; round to nearest whole number)

Given the reactions, X(s) + O₂(g) — XO(s) XCO3(s) what is AH for this reaction? X(s) + 1/2O₂(g) + CO₂(g) AH = XO(s) + CO₂(g) AH = -545.7 kJ AH = +433.9 kJ XCO3(s) kJ

a. Hydrogen cyanide is used in the manufacture of clear plastics such as Lucite and Plexiglas. It is prepared from ammonia and natural gas (CH4). 2NH3 (g) + 302 (9) + 2CH4 (g) → 2HCN(g) + 6H2O The reaction evolves 939 kJ of heat per 2 mol HCN formed. Is the reaction endothermic or exothermic? endothermic exothermic b. If 8 mol of HCN is produced, what is the value of q? kJ

When 2 moles of C2H6(g) react with O2(g) to form CO2(g) and H2O(g) according to the following equation, 2.86×103 kJ of energy are evolved. 2C2H6(g)+ 7O2(g)----->4CO2(g) + 6H2O(g) Is this reaction endothermic or exothermic? _________(endothermic or exothermic)What is the value of q? _______ kJ

Predict the enthalpy change for the reaction below, by combining reactions A-C.   NO (g) + O (g)NO2 (g) ΔH=??   A. O3 (g)  3/2 O2 (g) ΔH=-142.3 kJ/mole B. O2 (g)  2 O (g) ΔH=495.0 kJ/mole C. NO (g) + O3 (g)  NO2 (g) + O2 (g) ΔH=-198.9 kJ/mole

Calculate AH for the reaction. Enter your answer in the provided box. CH3OH + HCI →→→ CH₂Cl + H₂O kJ/mol