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I am having trouble getting the right answer to these few questions and I am very much in need of...
I am having serious trouble figuring out how to start these two questions d. What is...
I
am having serious trouble figuring out how to start these two
questions
d. What is the wavelength of the photon that would just ionize the ground-state atom to H*? 7. An energy of 1.09x103 kJ/mol is required to convert gaseous carbon atoms to gaseous C" ions and electrons. What is the maximum wavelength, in nm, of electromagnetic radiation with suffi- cient energy to cause ionization to a single carbon atom? In what region of the electromagnetic spectrum is this...
31. When 9.42 g of methane (CH4) is burned in a bomb calorimeter (heat capacity =...
31. When 9.42 g of methane (CH4) is burned in a bomb calorimeter (heat capacity = 2.677 × 103 J/°C), the temperature rises from 24.00 to 27.08°C. How much heat is absorbed by the calorimeter? CH4(g) + 2O2(g) → CO2(g) + 2H2O(l); ΔH° = –1283.8 kJ a. 745 kJ b. 4.84 × 103 kJ c. 8.24 kJ d. 753 kJ e. 1.28 × 103 kJ 32. Which of the following statements is incorrect concerning the wave function? The wave function...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom in the gas phase? Justify your answer with a calculation. 7. The energy of an electron in a hydrogen atom is -4.45 x 100 J. What energy level (n) does it occupy? Is there another valid energy level at -2.69 x 1020 ? If so, what is this other energy level? 8. What is the...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom in the gas phase? Justify your answer with a calculation. 7. The energy of an electron in a hydrogen atom is -4.45 x 100 J. What energy level (n) does it occupy? Is there another valid energy level at -2.69 x 1020 ? If so, what is this other energy level? 8. What is the...
Answer all parts Use the Bohr model to address this question. When a hydrogen atom makes...
Answer all parts
Use the Bohr model to address this question. When a hydrogen atom makes a transition from the 7h energy level to the 2 counting the ground level as the first, what is the energy E of the emitted photon in electron volts? eV What is the wavelength à of the emitted photon in nanometers? nm At what radius r does an electron in the 5th energy level orbit the hydrogen nucleus? Express your answer in nanometers. nm
I need the answers to these nine questions. They are attached below. Please answer all of...
I need the answers to these nine questions. They are attached
below. Please answer all of them. Thank you so much in advance!
Which of the following is the correct statement? ● A photon of yellow light has more energy than a photon of ultraviolet light. O A photon of yellow light has less energy than a photon of ultraviolet light. O A photon of yellow light has less energy than a photon of red light. O A photon of...
4) 74 kJ are required to heat 1 cup of water fronm room temperature to boiling....
4) 74 kJ are required to heat 1 cup of water from room temperature to boiling. The wavelength of microwave radiation in a microwave oven is 2.3 x 10-3 m. How many moles of photons are required? 5) Cesium requires a minimum energy of 188 kJ/mol for an electron to be ejected. What is the wavelength of light in nm that possesses the minimum amount of energy needed to cause the electron to eject? 5.4 Balmer-Rydberg 6) Use the Balmer-Rydberg equation to calculate...
05 Question (4 points) When a hydrogen atom absorbs a photon of electromagnetic radiation (EMR), the...
05 Question (4 points) When a hydrogen atom absorbs a photon of electromagnetic radiation (EMR), the internal energy of the atom increases and one or more electrons may be energized into an excited state. The release of this extra energy as the excited state electron transitions back to a lower energy state results in the emission of a photon. These energy changes are responsible for the emission spectrum of hydrogen (shown below) and are described by the Bohr equation. AE...
Please explain. 0/4 pts Question 5 Electrons exist in orbitals within an atom. Bohr's model described a single elec...
Please explain.
0/4 pts Question 5 Electrons exist in orbitals within an atom. Bohr's model described a single electron system well. But the energy level for orbitals change when as you add a second and more electron. In a single electron system, there are (a)_orbital(s) at the n-2 level. These n-2 orbital(s) exist at (b) sub-level(s) in the atom. In a multi-electron system, (c)_orbital(s) at the n-2 level. These n-2 orbital(s) exist at (d)sub-level(s) in the atom. Bohr was never...
Answer all questions correctly in pen in the examination booklet (10 pts. each) I) An electron...
Answer all questions correctly in pen in the examination booklet (10 pts. each) I) An electron falling from the n-6 level of a hydrogen atom emits light with a wavelength of 1094 nm. To what level did the electron fall? (10 pts.) fal m m.) are nossible. If not possible.
I
am having serious trouble figuring out how to start these two
questions
d. What is the wavelength of the photon that would just ionize the ground-state atom to H*? 7. An energy of 1.09x103 kJ/mol is required to convert gaseous carbon atoms to gaseous C" ions and electrons. What is the maximum wavelength, in nm, of electromagnetic radiation with suffi- cient energy to cause ionization to a single carbon atom? In what region of the electromagnetic spectrum is this...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom in the gas phase? Justify your answer with a calculation. 7. The energy of an electron in a hydrogen atom is -4.45 x 100 J. What energy level (n) does it occupy? Is there another valid energy level at -2.69 x 1020 ? If so, what is this other energy level? 8. What is the...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom in the gas phase? Justify your answer with a calculation. 7. The energy of an electron in a hydrogen atom is -4.45 x 100 J. What energy level (n) does it occupy? Is there another valid energy level at -2.69 x 1020 ? If so, what is this other energy level? 8. What is the...
Answer all parts
Use the Bohr model to address this question. When a hydrogen atom makes a transition from the 7h energy level to the 2 counting the ground level as the first, what is the energy E of the emitted photon in electron volts? eV What is the wavelength à of the emitted photon in nanometers? nm At what radius r does an electron in the 5th energy level orbit the hydrogen nucleus? Express your answer in nanometers. nm
I need the answers to these nine questions. They are attached
below. Please answer all of them. Thank you so much in advance!
Which of the following is the correct statement? ● A photon of yellow light has more energy than a photon of ultraviolet light. O A photon of yellow light has less energy than a photon of ultraviolet light. O A photon of yellow light has less energy than a photon of red light. O A photon of...
05 Question (4 points) When a hydrogen atom absorbs a photon of electromagnetic radiation (EMR), the internal energy of the atom increases and one or more electrons may be energized into an excited state. The release of this extra energy as the excited state electron transitions back to a lower energy state results in the emission of a photon. These energy changes are responsible for the emission spectrum of hydrogen (shown below) and are described by the Bohr equation. AE...
Please explain.
0/4 pts Question 5 Electrons exist in orbitals within an atom. Bohr's model described a single electron system well. But the energy level for orbitals change when as you add a second and more electron. In a single electron system, there are (a)_orbital(s) at the n-2 level. These n-2 orbital(s) exist at (b) sub-level(s) in the atom. In a multi-electron system, (c)_orbital(s) at the n-2 level. These n-2 orbital(s) exist at (d)sub-level(s) in the atom. Bohr was never...
Answer all questions correctly in pen in the examination booklet (10 pts. each) I) An electron falling from the n-6 level of a hydrogen atom emits light with a wavelength of 1094 nm. To what level did the electron fall? (10 pts.) fal m m.) are nossible. If not possible.
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