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Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. 2 HNO3(aq) + NO(g) ? 3 NO2(g) + H2O(l) K = ? Delta-G°f (kJ/mol) -110.9 87.6 51.3 -237.1
Calculate the heat required to convert 25.0 g of C2Cl3F3 from a liquid at 5.00 degress celsius to a gas at 82.00 degrees celsius.
Determine the concentration of hemoglobin solution knowing that its absorbance is 0.65. The pathlength is 1 cm and the extinction coefficient is 3.9 x 105 M-1cm-1.
calculate the freezing point and boiling point of each of the following solutions: a)65.0g of glucose,C6H12O6, anonelectrolyte, added to .112kg of water
identify the following compound from its IR and proton NMR spectra. C5H6O: IR: 3300 (sharp), 2102, 1634 cm-1 NMR: ? 3.10 (1H, d, J = 1 Hz); ? 3.79 (3H, s); ? 4.52 (1H, doublet of doublets, J = 10 Hz and 1 Hz); ? 6.38 (1H, d, J = 10 Hz)
Why must the spot applied to a TLC plate be above the level of the developing solvent
The melting point of a pure compound is known to be 110-111°. Describe the melting behavior expected if this compound is contaminated with 5% of an impurity.
Ten kg of steam at 500 bar is expanded at constant pressure until its pressure increases to seven times its initial value of 0.01 m^3. (a) Determine the initial and final temperature of the steam. (b) Calculate the heat that must be supplied to ca..
An experiment shows that a 248 -mL gas sample has a mass of 0.433 g at a pressure of 749 mmHg and a temperature of 29*C. What is the molar mass of the gas
When 2-methylpropene is treated with sulfuric acid the resulting mixture can be used to convert benzene to tert-butylbenzene
What is the maximum mass of ammonia that can be produced from a mixture of 155.3 g of N2 and 35.98 g of H2? 2. Which element would be left partially unreacted? (enter nitrogen or hydrogen)
Compute the unsaturation number (aka index of hydrogen deficiency) associated with C4H3NO2S. Interpret your results. If there are no triple bonds in this compound, can you suggest a reasonable structure for the compound
Element Z has two naturally occurring isotopes Z-79 ( 78.918 amu) and Z-81 (80.916 amu) . Calculate the atomic mass of element Z given the abundance of the Z-81 is 49.31 %
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