Problem 3: a. Calculate the wavelength of light in (nm) with a frequency of 1.53x 10"...
Calculate the enthalpy of decomposition of aluminum chloride in the town 2 AICE() ---> 2Al(s). (g) Use the following four equations: a) 2Al(s) + 6HCl(aq) + 2AICI.(aq) + 3H2(8) AH" --1049 kJ/mol b) HCl(aq) - HC (g) AH':- 74.8 kļ/mol c) H2(g) + Cl:(g) - 2HCI(g) AH", -1845 kJ/mol d) AICI, (s) -- AICI (aq) AH'= -323 kJ/mol
Experiment 13-Post-Lab Assignment 1. Athletes use cold packs containing ammonium nitrate solutions to ice their injuries. A 1.25 G sample of ammonium nitrate is dissolved in 25.0 mL of water to form a solution. The temperature of the solution falls from 25.8°C to 21.9°C. Find the enthalpy of the reaction (AH ), in kJ/mol. Assume the density of water is 1.00 g/mL and the heat capacity of the total solution to be 4.184 J/g °C 2. Calculate AHⓇ in kJ/mol...
Calculate the heart of formation for aluminum chloride using the following thermochemical equations: 2Al (s) + 6HCl (aq) ---> 2AlCl3 (aq) + 3H2 (g) . ΔH = -1049 kJ HCl (g) ---> HCl (aq) . ΔH = -74.8 kJ H2 (g) + Cl2 (g) ---> 2HCl (g) ΔH = -1845 kJ AlCl3 (s) ---> AlCl3 (aq) ΔH = -323 kJ
Use Hess's Law to determine Delta H for the reaction 2 Al(s) + 3 Cl_2(g) rightarrow 2 AlCl_3(s) given: 2 Al(s) + 6 HCl(aq) rightarrow 2 AlCl_3(aq) + 3 H_2(g) Delta H = -1049 kJ HCl(g) rightarrow HCl(aq) Delta H = -74.8 kJ H_2(g) + Cl_2(g) rightarrow 2 HCl(g) Delta H = -185 kJ AlCl_3(s) rightarrow AlCl_3(aq) Delta H = -323 kJ
2Al(s) + 3Cl2(8) - 2AICI,(s) AH =? Use the reactions here to determine the AH' for reaction : ® HCI(g) — HCl(aq) AH;, = -74.8 kJ (a) Hz(8) + C1>(- 2HCl(8) AH) = -185 kJ M AICI;(aq) - AICI,(s) AH = +323 kJ/mol M 2Al(s) + 6HCl(aq) - 2AICI,(aq) + 3H2(g) AH = -10:49 J
calculate the frequency of visible light having a wavelength of 486 nm. calculate the wavelength (nm) of a H atom (1.67 * 10-27 kg) moving at 900 cm/s
8. C alculate the frequency of green light that has a wavelength of 531 nm? 9. Calculate the wavelength of blue light that has a frequency of 6.68 x 10" s 10. Calculate the energy of a photon with a frequency of 7.00 x 1014s I1. Calculate the frequency of a photon if the energy is 7.26 x 1019 J 12. Calculate the wavelength (in nm) of a photon if the energy is 7.26 x 10-19 J.
calculate the wavelength in the unit of nm, frequency in the unit of HZ, and the wavenumber in the unit of cm^-1 of an electromagnetic radiation with the energy f 1.326X 10^-20 J. E=hv V=vλ ν with a line =1/λ where E is the energy (j): h is plank constand, v is frequency, V is the velocity of light, v with a line is the wavenumber, λ is wavelength
calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n=4 to the n=1 principal energy level. E=-2.18x10^-18 J(1/n^2) Constants (c = 2.9979 | 109 m/s; h = 6.626 | 10 " J[s) 1. What is the energy in joules of a mole of photons with visible light of wavelength 486 nm? (246 kJ) 2. Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its...
1. What is the frequency of visible light with a wavelength of 500 nm? 2. For each of the following, describe the relationship as directly or inversely proportional: a) wavelength vs. frequency b) wavelength vs. energy c) frequency vs. energy -372.1 nm and 2. - 376,4 nm 3. When sodium is excited in a flame, two ultraviolet spectral lines at respectively are emitted. Which wavelength represents photons with a) higher energy? b) longer wavelengths? c) higher frequencies?