Asked by Anonymous
CH4 + 2 Cl2--> CH2Cl2 + 2HCl
Cl-Cl bond energy: 242 kj/mole
1. Calculate the amount of energy (Joules) needed to break a single Cl-Cl bond.
2. Calculate the longest wavelength of light (meters)that can supply the energy per photon necessary to break the Cl-Cl bond.
Cl-Cl bond energy: 242 kj/mole
1. Calculate the amount of energy (Joules) needed to break a single Cl-Cl bond.
2. Calculate the longest wavelength of light (meters)that can supply the energy per photon necessary to break the Cl-Cl bond.
Answers
Answered by
DrBob222
242 kJ/mol = 242,000 J/mol
242,000 J/mol x (1 mol/6.022 x 10^23 molecules) = E for one molecule in joules.
E = hc/wavelength.
242,000 J/mol x (1 mol/6.022 x 10^23 molecules) = E for one molecule in joules.
E = hc/wavelength.
Answered by
Anonymous
24
Answered by
Nosipho
Calculate the total energy required to break bonds of the reactants if c-h is 414 kj mol
O-h 460 kj mol
o=o 499
c=o 799 kj mol
O-h 460 kj mol
o=o 499
c=o 799 kj mol
Answered by
Nosipho
Ch4+2h2o ›2h2oo+co2+energy c-h 414 kj mol
o-h 460 kj mol
o=o 499 kj mol
c=h 799 kj mol
o-h 460 kj mol
o=o 499 kj mol
c=h 799 kj mol
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.