Photolysis of carbon monoxide can occur according to the following rxn: CO + hν --> C...
Photolysis of carbon monoxide can occur according to the following rxn:
CO + hν --> C + O (delta)H = 1079 kJ/mole
What wavelength of light does this correspond to in m and nm?
(1079 kJ/mol) * (1000 J/1 kJ) * (1 mol/6.02*1023 photons) = 1.792 * (10^-18 J/photon)
([6.6 * 10^ -34 J/s) * (3.0*10^8 m/s)] / 1.792 * 10^-18 J/photon = 1.1 * 10^7 m or 110 nm
Homework Answers
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Photolysis of carbon monoxide can occur according to the
following rxn:
CO + hν --> C...
Photolysis of carbon monoxide can occur according to the following rxn: CO + hν C +...
Photolysis of carbon monoxide can occur according to the
following rxn:
CO + hν
C + O
H = 1079 kJ/mole
What wavelength of light does this correspond to? What type of
light is this? Do we need to worry about this reaction happening
near the earth’s surface? Explain why.
We were unable to transcribe this imageWe were unable to transcribe this image
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9. Carbon monoxide (CO) is toxic because it can displace oxygen (O2) from the iron in hemoglobin (Hgb) following the reaction: HgbO2 (s) + CO(g) + Hgbco (s) + O2 (g) AG®rx = -30. kl/mol A. Consider the following reactions involving hemoglobin, O2 and Co: Hgboz (s) + Hgb (s) + O2 (g) AG®rxn = 40. kJ/mol HgbCO (s) -- Hgb (s) + CO (6) AGºrx = ??? Using Hess's law, determine the free energy AG*rn (in kJ/mol) for the...
What is the energy in joules of a mole of photons associated with visible light of...
What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 x 10 m/s; h = 6.63 x 10-34 J·s; NA = 6.022 x 1023 moles) Select one: a. 6.46 x 10-16 J b. 6.46 x 10-25 c. 2.46 x 10-4 J Od. 12.4 kJ O e. 246 kJ
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Need chemistry help with 9 & 10 For the reaction C(s) + H_O(g) rightarrow CO(g) +...
Need chemistry help with 9 & 10
For the reaction C(s) + H_O(g) rightarrow CO(g) + H_2(g) DeltaHdegree = 131.3 kJ/mol and DeltaSdegree = 133.6 J/K middot mol at 298 K. At temperatures greater than degreeC this reaction is spontaneous under standard conditions. A) 983 B) 325 C) 273 D) 710 E) 552 10. A mole of yellow photons of wavelength 527 nm has kj of energy. A) 227 B) 2.74 times 10-^19 C) 4.56 times 10-^46 D) 6.05 times...
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calculate the wavelength of the light emitted by a hydrogen atom
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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...
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Photolysis of carbon monoxide can occur according to the
following rxn:
CO + hν
C + O
H = 1079 kJ/mole
What wavelength of light does this correspond to? What type of
light is this? Do we need to worry about this reaction happening
near the earth’s surface? Explain why.
We were unable to transcribe this imageWe were unable to transcribe this image
9. Carbon monoxide (CO) is toxic because it can displace oxygen (O2) from the iron in hemoglobin (Hgb) following the reaction: HgbO2 (s) + CO(g) + Hgbco (s) + O2 (g) AG®rx = -30. kl/mol A. Consider the following reactions involving hemoglobin, O2 and Co: Hgboz (s) + Hgb (s) + O2 (g) AG®rxn = 40. kJ/mol HgbCO (s) -- Hgb (s) + CO (6) AGºrx = ??? Using Hess's law, determine the free energy AG*rn (in kJ/mol) for the...
What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 x 10 m/s; h = 6.63 x 10-34 J·s; NA = 6.022 x 1023 moles) Select one: a. 6.46 x 10-16 J b. 6.46 x 10-25 c. 2.46 x 10-4 J Od. 12.4 kJ O e. 246 kJ
QUESTION 20 What is the wavelength of a photon that can just break a Nitrogen/Nitrogen Triple bond (N=N). It takes 945 kJ to break one mole of these bonds. You can refer to the following figure to help you : EI h = 6.6 x 10-34 m2 kg/s c = 3 x 108 m/s Na = 6.02x 1023
Need chemistry help with 9 & 10
For the reaction C(s) + H_O(g) rightarrow CO(g) + H_2(g) DeltaHdegree = 131.3 kJ/mol and DeltaSdegree = 133.6 J/K middot mol at 298 K. At temperatures greater than degreeC this reaction is spontaneous under standard conditions. A) 983 B) 325 C) 273 D) 710 E) 552 10. A mole of yellow photons of wavelength 527 nm has kj of energy. A) 227 B) 2.74 times 10-^19 C) 4.56 times 10-^46 D) 6.05 times...
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...
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