What maximum wavelength (in nm) of fight is necessary to break the bond in a nitrogen molecule
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Chemistry
- Selenium tetrafluoride is produced from a reaction of elemental Se with chlorine trifluoride according to the balanced chemical equation: 3 Se(g) + 4 CIF3(g) → 3 SEF4(g) + 2 Cl2(g) AHrxn = -1874 kJ Using AHrxn and the table of bond energies below, determine the bond energy of the Se-F bonds in SeF4. Note that all bonds in the reactants and products are single bonds. Bond Bond Energy (k.J/mol) CI-F 253 CI-CI 243 The units are kJ/mol. Do not include units in your answer. Scientific notation is optional. To write scientific notation in Canvas, type "e" to replace "x 10". For example, "1 x 1014" is written "1e+14" in Canvas.arrow_forwardA.) Which C–O bond has the smallest bond energy? CO32– CO2 CO B.) Which reaction is exothermic? 2CO(g) + O2(g) → 2CO2(g) CO2(g) → C(s) + O2(g) CO2(g) + H2O(l) → 2H+(aq) + CO32–(aq)arrow_forwardHow many nonbonding pairs (or lone-pairs) of electrons are found on the central atom in the Lewis structure of XeF2 molecule? (A) 0 (B) 1 (C) 2 (D) 3arrow_forward
- Consider hypothetical elements X2 and Y2. Suppose the enthalpy of formation of the compound XY is – 84 kJ/mol, the bond energy for X2 is 105 kJ/mol, and the bond energy for Y2 is 58 kJ/mol. A)Estimate the XY bond energy, Ed, in units of kJ/mol. B)If the dissociation of a X-Y molecule were accomplished by the absorption of a single photon whose energy was exactly the quantity required, what would be its wavelength in nm? C)Would a green-light photon (λgreen=550 nm) be able to break the above X-Y bond? Explain.arrow_forward6i)The lattice energy of NaBr is –752 kJ/mol. This energy corresponds to which reaction below? A. Na(s) + 1/2 Br2(g) → NaBr(s) B. Na(g) + Br(g) → NaBr(s) C. Na(g) + Br(g) → NaBr(s) D. Na+(g) + Br–(g) → NaBr(s) E. Na+(aq) + Br–(aq) → NaBr(s)arrow_forwardHydrazine, N2H4, burns in oxygen as follows: N2H4 + O2 → N2 + 2H2O [The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496] Draw the chemical structures of the reactants and products and give the formula to calculate enthalpy change in a reaction, ΔH.arrow_forward
- The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy. (А) С-С (В) С-С (А,B) (C) N-N (D) N=N (С.D)arrow_forward1) What do you predict the average bond length and average bond energy values for the F-F bond based on the chart below? WIll it be higher than, lower than, or the same as the other bonds shown in the chart. Justify your answer. Bond Average Bond Length (PM) Average Bond Energy (KJ/MOLE) CL-CL 199 243 Br-Br 228 193 I-I 267 151 2) Explain how a stable covalent bond is formed in terms of attractive and repulsive forces. Note: Please briefly explain, Thank you.arrow_forwardFructose, C6H1206(S), consists of 5 C-C single bonds, 7 C-O bonds, 7 C-H bonds, and 5 O-H bonds with average bond energies of 348 kJ/mol, 360 kJ/mol, 412 kJ/mol, and 463 kJ/mol respectively. The bond energy for C=O is 799 kJ/mol and O=O is 498 kJ/mol. The molar mass of fructose is 180.12 g/mol. Estimate the change in enthalpy if 2.56 g of fructose undergoes complete combustion at standard temperature and pressure.arrow_forward
- Which atom in the C-F bond has a partial negative charge (δ⁻)?arrow_forwardDraw the Lewis structure for the chlorine trifluoride (CIF3) molecule. Ċ C C X S 1 [] ?arrow_forwardThe enthalpy change for the reaction between two molecules of carbon oxysulfide (COS) to form one molecule of CO2 and one molecule of CS2 as shown below, is -3.2 x 10-24 kJ per molecule of COS. The bond energy for the C-S bond in CS2 has been determined to be 552 kJ/mol. 1st attempt O See Hint What is the apparent bond energy of a carbon-sulfur bond in COS? Use the bond energies below. kJ Bond Energy Bonds (kJ/mole) C=S 552arrow_forward
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