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The enthalpy of formation of ethanol, C2H5OH, is -277.0 kJ/mol at 298.15k. calculate the enthalpy of combustion of one mole of ethanol, assuming that the products are CO2 (g) and H2O.
The bond energy of hydrogen is 51 kJ/mol (0.52 eV/molecule). Based on this information, how much energy should be required to break all of the hydrogen bonds in one gram of ice, thus separating the H2O molecules into independent units. Give answer..
vAt a particular temperature, K = 2.0 10-6 mol/L for the following reaction. 2 CO2(g) 2 CO(g) + O2(g) If 1.7 mol CO2 is initially placed into a 3.7-L vessel, calculate the equilibrium concentrations of all species. [CO2] [CO] [O2]
Where would we predict benzene to absorb if we treated the pi-electrons as particles on a ring (radius 1.39 A)? What is the % error? I'll give you a hint.
Explain why the wild horse analogy can be used to help explain a certain type of chemical bonding
Without referring to the appendix, calculate the quantity (Delta rG - Delta rA) for the following reaction at 298 K: C(s) + CO2(g) --> 2CO(g) Assume ideal gas behavior.
a silver chloride precipitate weighing 0.2255 grams was obtained from 0.3448 grams of a soluble salt mixture. calculate
An aqueous solution contains metal cations Hg^+2 and Mn^+2 belonging to groups 2 and 3 respectively. Thioacetamide which produces H2S is added and the solution is buffered to a pH of 8 by addition of NH3/NH4Cl
Liquid dimethyl disulfide (CH3SSCH3) flows through a pipe with a mass flow rate of 29.0 g/s. Given that the density of dimethyl disulfide
a specific brand gourmet chocolate candy contains 7.00g of dietary fat in each 22.7 piece. how many kilograms of
Consider the titration of 80.0 mL of 0.0200 M HONH2 (a weak base; Kb = 1.10e-08) with 0.100 M HBrO4. Calculate the pH after the following volumes of titrant have been added- (a) 0.0 mL pH = (b) 4.0 mL pH = (c) 8.0 mL pH = (d) 12.0 mL pH = (e) 16.0..
What is the pH halfway to the equivalence point for the titration of 0.20 M CH3NH2 with 0.20 M HCl? (Kb of CH3NH2 = 4.4 x 10-4)
If 77.0 mL of hydrogen gas is collected over water at 50.0 degrees celsuis and 763 mm Hg, what is the volume of dry gas at standard conditions? The vapor pressure of water is 92.5mm Hg at 50.0 degrees celsuis .
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