Estimate the energy difference between AU° and AH° (that is: AU° – ▲H°), in kJ mol−, for the following reaction at 298 K: a. -10.1 kJ mol-1 b. -7.74 kJ mol-1 c. +2.48 kJ mol-¹ d. +6.41 kJ mol-¹ e. +13.3 kJ mol−¹ 2 NaOH(s) CO2(g) →>> Na2CO3(aq) + H2O(l)
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- Do you expect the constant ,1 in (9.30) describing the susceptibility of the covalent bond to be positive or negative? Why?The amount of saturation not only has an effect on the chemical but also the physical properties of the fat. For example, animal fat which is about half saturated and half unsaturated fat is a solid at room temperature but vegetable fat which is about 85 % unsaturated fat is a liquid at room temperature. This is because saturated fats are more linear compared to unsaturated which are nonlinear (bent), meaning that saturated fats are capable of more of what kind of interaction? Hydrogen bonding van der Waals Ionic bonding Covalent bondingThe dissociation energy of a carbon–bromine bond is typicallyabout 276 kJ/mol. (a) What is the maximum wavelengthof photons that can cause C—Br bond dissociation?(b) Which kind of electromagnetic radiation—ultraviolet,visible, or infrared—does the wavelength you calculated inpart (a) correspond to?
- NB Assume the densities of all solutions are 1.0 g/mL and their specific heat capacities 4.184 J/g .K Molar Mass of KCl: 74.55 g/mol Help from calculating qr to average ethalpy.determine hvap for these valuesAn important reaction in the formation of photochemicalsmog is the photodissociation of NO2:NO2 + hv---->NO(g) + O(g) The maximum wavelength of light that can cause this reactionis 420 nm. (a) In what part of the electromagnetic spectrumis light with this wavelength found? (b) What is themaximum strength of a bond, in kJ/mol, that can be brokenby absorption of a photon of 420-nm light? (c) Write out thephotodissociation reaction showing Lewis-dot structures.
- especially for B TO X, D to Y, and G to H, I => React with (CH3CO)2O , : N (C2H5) 3part 6b: g,h,iThere is some indication that other hydrogen ring compounds and ions in addition to H3 and D3 species may play a role in interstellar chemistry. According to J.S. Wright and G.A. DiLabio (J. Phys. Chem. 96, 10 793 (1992)), H5−, H6, and H7+ are particularly stable whereas H4 and H5+ are not. Confirm these statements by Hückel calculations.