Calculate ΔE in kJ/mol if the electron "falls" from n = 2 to n =
1 (known as a 2→1 transition).
A. -1
B. -984
C. 984
D. 1
Calculate ΔE in kJ/mol if the electron "falls" from n = 2 to n = 1...
1. Calculate the energy difference (ΔE) for the electron transition of n = 6 to n = 2 for 1.00 mol of hydrogen atoms. Enter your answer in scientific notation. 2. Calculate the energy difference for the transition of n = 2 to n = 6 for 1.00 mol of hydrogen atoms. Enter your answer in scientific notation.
Be sure to answer all parts. A. Calculate the energy difference (ΔE) for the electron transition of n = 3 to n = 2 for 1.00 mol of hydrogen atoms. Enter your answer in scientific notation. B. A lithium flame has a characteristic red color due to emissions of wavelength 671 nm. What is the mass equivalence of 6.0 mol of photons of this wavelength (1 J = 1 kg·m2/s2)?×10 kg (Enter your answer in scientific notation.)
An ionic compound, MBr, has ΔE for (M+1/2Br2 => MBr) = -500 kJ/mol. Given the information below, calculate its lattice energy. M(s) => M(g) ΔE = +140 kJ/mol M(g) => M+(g) + 1 e- ΔE = +500 kJ/mol Br2(l) => 2Br(g) ΔE = +200 kJ/mol Br(g) + 1 e- => Br-(g) ΔE = -325 kJ IE1 of Br(g) = +1143 kJ/mol
What is the change in energy, ΔE, in kilojoules per mole of hydrogen atoms for an electron transition from n=4 to n=2? Express your answer in kilojoules per mole to three significant figures.
1.. Suppose that you shine light of energy 1050 kJ/mol on an H atom in the ground state. What happens to the light and to the electron? Group of answer choices a. The light is not absorbed and the final energy of the electron is -1312 kJ/mol. b.. The light is absorbed and the final energy of the electron is −328 kJ/mol. c.. The light is not absorbed and the final energy of the electron is −1050 kJ/mol. d.. The...
Calculate w and ΔE when 2 mol of liquid ZnC4H10 is vaporized at 265 K and 760 mm Hg. The ΔH vaporization is 39.9 kJ/mol at 265 K.
1. Finally, calculate the energy in kJ/mol corresponding to the removal of an electron from a hydrogen atom originally in the ground state (i.e., from n=1 to n=∞). Show all your work.
For ammonia, ΔHvap = 23.6 kJ/mol at its boiling point, -33 oC. Calculate the values for ΔS, q, w, and ΔE for the vaporization of ammonia at -33 oC and 1 atmosphere pressure.
Calculate the energy for the transition of an electron from the n=1 level to the n= 7 level of a hydrogen atom. AE = Joules Is this an Absorption (A) or an Emission (E) process? Calculate the energy for the transition of an electron from the n=1 level to the n=5 level of a hydrogen atom. AE = Joules Is this an Absorption (A) or an Emission (E) process? Calculate the energy of an electron in the n= 3 level...
PLEASE SHOW WORK 1. Calculate the energy (1) change associated with an electron transition from n = 2 to n=5 in a Bohr hydrogen atom. (3 points) Rydberg constant, Ry = 1.096776 x 10' m' hcRy = 2.18 x 10'8; Planck's constant, h = 6.626 x 1034 JS c = 2.998 x 109 m/s 2. a) Draw all the possible resonance structures for the carbonate ion. (3 points) b) What is the molecular geometry of the carbonate ion? 3. Using...