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The reaction below is called the Haber Process and it is the main industrial procedure for the production of ammonia today. N.° + 3H, 2 NH2 AH° - -91.8kJ/mol If 19.8 g of H2 reacted in excess N2 how much heat, in kJ, would be released? Question 2 0.5 pts The reaction below is called the Haber Process and it is the main industrial procedure for the production of ammonia today. N2 + 3 2 NH, AH ========= -91.8kJ/mol If-211.77 k of heat was released, how many grams of NH3 was produced? Question 3 1 pts In volcances. carbon disulfide reacts with oxygen to produce carbon dioxide and sulfur dioxide according to the reaction below. - ch In volcanoes, carbon disulfide reacts with oxygen to produce carbon dioxide and sulfur dioxide according to the reaction below. CS2(I)+3O2(g) CO2(g) + 2 502(g) Ifthe following enthalpies of reactions are known, what is the enthalpy, in kJ/mol, of the above reaction? C(s) + O2(g) CO2(g) NH = - -393.5 kJ/mol S(s) + O2(g) SO2(g) AHF = - -296.8 kJ/mol C(s) # 2 S(s) CS2(I) AHF = 87.9 kJ/mol Question 4 Recently Mt. Etna erupted on the island of Sicily. Every year, Mt. Etna releases 2.91 x 107 kg of SO2 into the atmosphere Using the enthalpy of the reaction calculated in Question 3. how much heat. in kJ. is generated from this release? Please report your answers in scientific notation in the fields belo 10 kJ C(s) + 2S(s) CS2(I) AHf - 87.9 kJ/mol Question 4 1 pts Recently Mt. Etna erupted on the island of Sicily. Every year, Mt. Etna releases 2.91x109 kg of SO2 into the atmosphere. Using the enthalpy of the reaction calculated in Question 3, how much heat, in kJ, is generated from this release? Please report your answers in scientific notation in the fields below. - 10 kJ 1 pts Question 5 Emission line spectra for various elements are shown in Table 1 and Table 2 shows the wavelengths forvarious colors Remember E h°c/A. where E is energy, h = J"s, C= 3.00*10³ m/s. À is thewavelength. and ##### of Varous Elements Table 2. Wavelengths of Various Colors Emission line spectra for various elements are shown in Table 1 and Table 2 shows the wavelengths for various colors. Remember, E - h*c/À, where E is energy, h = 6.626*10-34 J*s, C - 3.00*108 m/s,Àis the wavelength, and 1 m = 109 nm. Table 1. Emission Line Spectra of Various Elements Table 2. Wavelengths of Various Colors Element Emission Lines (nm) Color Wavelengths (nm) H 410.2, 434.1, 486.1, 656.3 Violet 380-450 He 447.1, 492.1, 501.5, 587.5 Blue 450-495 Hg 404.7, 435.8, 546.1, 577.0 Green 495-570 Na 588.9.589.5 Yellow 570-590 Mg 487.8,502.5,574.1,710.9 Orange 590-620 Red 620-750 Unknown element A produced line spectra energies of 4.075"10-19 J and 2.796*10-19 J. Using Tables 1 and 2 above, calculate the corresponding wavelengths in nm, identify each line's color, and determine the unknown element. Pay attention to significant digits and the colors should be capitalized, e.g. "Orange" with a capital O. Wavelength 1: nm Unknown element A produced line spectra energies of 4.075*10-19 J and 2.796*10-19 J. Using Tables 1 and 2 above, calculate the corresponding wavelengths in nm, identify each line's color, and determine the unknown element. Pay attention to significant digits and the colors should be capitalized, e.g. "Orange" with a capital O. Wavelength 1: nm Color 1: Wavelength 2: nm Color 2: Element (use the chemical symbol, i.e., hydrogen would be H): Question 6 1 pts Calculate the energy, in kJ, of 1 mole of x-rays that has a wavelength of 2.187 nm. Remember, E = h"c/ 1. where E is energy, h = 6.626"10-34 J*s, C = 3.00*108 m/s, A is the wavelength, 1 m = 10% nm, and 1 mole = 6.022"10²3 -

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