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Primary and global quantum yields in photochemistry. Define them and give their formulas. Differentiate between them.
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- D21 1120 Ch-13 Homework - General Chemistry II W 1120 Ch-12 Homewart Write a balanced chemical equation for each reaction. (Include states-of-matter under the given conditions in your answer.) (a) combustion of acetylene (ethyne, C₂H₂(g)) to form carbon dioxide gas and water vapor The reactants are acetylene and oxygen (because this is a combustion reaction) and the products are carbon dioxide gas and water. The Help chemPad XX (b) synthesis of NO(g) from N₂O(g) and NO₂(g) The reactants are N₂O and NO2, and the product is NO. The balanced chemical equation is the following. Help chemPad XX¹ chemPad XX Greek ← ->> (c) reaction of solid carbon graphite with water vapor to produce carbon monoxide gas and hydrogen gas The reactants are C and H₂O, and the products are CO and H₂. The balanced chemical equation is the following. Greek → Help Greek -19 Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane using average bond enthalpies (use exam data sheet values). H–C≡C–H(g) + 2H2(g) → H3C–CH3(g)4. Photochemical smog is a type of air pollution in the troposphere of our planet produced when sunlight acts upon motor vehicle exhaust gases to form harmful substances such as ozone (O3). For example, nitrogen dioxide (NO2) reacts with atmospheric oxygen (O2) in the presence of light to produce ozone (O3) and nitrogen monoxide (NO).
- Part 1.) 4NH3 (g) +502 (g) - -- > 4 NO (g) 6H2O (g)Write the formation reactions for the compounds shown and their enthalpy of formation values. NO is already provided. rxn 1: -- 1/2 N2 (g) + 1/2 O2 (g) > NO ( g) delta H fNO = ?, rxn 2: N2 (g) + H2 (g) - - > NH3 (g) delta HfNH 3 = ?, rxn 3: H2(g) + O2 (g) - > H 20 (g) delta H fH2O = ? In the delta sheet given I found deltaHf NO +91.3 kJ/mol, deltaHfNH3 = 45.9 kJ/mol, deltaHfH2O -241.8 kJ/mol. Part 2.) Using these three formation reactions (rxn) determine the enthalpy of the rxn. deltaHrxn using Hess's law.NUMBER 63 and 64 and 65Using the table of average bond dissociation enthalpies at 25°C, determine which of the following reactions are energetically favorable at room temperature. Assume that ▲S = 0. Q.CH2=CH2 + 2H2 + N2 --> H2NCH2CH2NH2
- The chart shows average CO2 emissions for fossil fuel vehicles (gasoline, diesel, and hybrid gas‑electric), as well as electric vehicles. The ordinate is mg CO2 per mile driven per pound mass of the vehicle (called curb weight). For electric vehicles, CO2 emission varies in U.S. states because of the mix of fuels used to generate electricity. If electricity came entirely from solar power, there would be little CO2 associated with its production. California has the lowest CO2 emission for producing electricity and Ohio has the highest because it depends heavily on coal‑fired power plants. The chart does not include CO2 emission from manufacturing vehicles. When normalized for distance driven by each kind of vehicle before it is scrapped, CO2 emission associated with manufacturing electric vehicles is estimated to be 25–75% greater than CO2 emission associated with manufacturing gasoline and diesel vehicles. If manufacturing were included, CO2 emission associated with electric vehicles…cigarette lighters burn butane, C4H10. write a balanced equation, assuming complete combustion, that is, plenty of oxygen.Because carbon and silicon are both elements in group 14 on the periodic table, we expect them to react with other elements in similar ways. To some extent, they do, but in some cases, carbon and silicon compounds that seem to have analogous structures have very different chemical characteristics. For example, carbon tetrachloride, CCl4, is very stable in the presence of water, but silicon tetrachloride, SiCl4, reacts quickly with water. The unbalanced equation for this reaction is SiCl4 + H2O → Si(OH)4 + HCl Balance this equation. Write a conversion factor that could be used to convert between moles of SiCl4 and moles of H2O. How many moles of SiCl4 react with 24 moles of water? Write a conversion factor that could be used to convert between moles of Si(OH)4 and moles of water. How many moles of Si(OH)4 form when 4.01 moles of H2O react with an excess of SiCl4?
- Use the indicated average bond enthalpies to estimate the change in enthalpy, ΔHo, for the reaction between methane and iodine to produce iodomethane and hydrogen iodide: CH4(g) + I2(g) → CH3I(g) + HI(g) ΔHo = ? It may be helpful to draw the Lewis electron dot structure for each reactant and product; all reactants and products have single bonds. average bond enthalpies (kJ) C - H 413 , C - I 240 , H - I 299 , I - I 151 Express your answer in units of kilojoules, but do not include the units on your submitted answer.Thank you!Carbon dioxide emissions associated with a one-night stay in a hotel room are calculated at 29.53 kg of CO2 per room day for an average hotel. The 200 rooms of your hotel are all occupied for two days during a college football game. How much CO2 did the guests and hotel release into the atmosphere?