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A 1.200 gram sample of C7H6O2 was dissolved in 11.42 grams of lauric acid, and it was determined that the freezing point of the lauric acid was lowered by 1.680 Celcius. The value of Kf of the lauric acid is 3.90 Celcius m^-1. Assume that the compound does not dissociate in lauric acid.
Calculate the molar mass of the C7H6O2 from the information provided.
Compute pH and [OH-] for each of the following solutions. (a) 8.1×10-2M Na2CO3, (b) 0.15M NaCN
The selection of enantiomerically pure (1S)-[endo]-(-)-borneol in the upcoming experiment presents a great opportunity to review some stereochemistry basics
Assume that the heat required for the vaporization of the alcohol comes only from the aluminum block and that the alcohol vaporizes at 25. Suppose that 1.15 of rubbing alcohol evaporates from a 65.0 aluminum block.
CO(g) + 2H2(g) = CH3OH(g) , what is the equilibrium constant? , where CH3OH = 0.0412 atm, H2 = 0.274 atm, CO = 0.914 atm.
For each of the following, calculate the concentration of Tris, Tris-H+ and the pH of the solution in each of the following solutions.
Organic chemistry solution - First question wants the product of certain oxidation reaction of chromic acid with a secondary alcohol and primary alcohol.
600 mL of water is heated from 20c to 85 c to make a cup of tea. How much heat flows into the water? NOTE: density and specific heat capacity of water 1.00g/mL and 4.18J/(g.c) respectively.
Find the pH of a solution that has a weak acid concentration of 1.72 M and a weak base concentration
What mass of carbon monoxide in grams is present in a room measuring 8.5 12.0 18.4 ft ?
A solution of ethanol (C2H5OH) in water is prepared by dissolving 57.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 255.0 mL of solution.
the specific heat of an unknown metal is found to be 0.233 j kg. The law of dulong and petit predicts a molar heat capacity of J/K mol. Use this law to estimate the molar mass of the element.
Write the balanced equation for the decomposition of one mole of NH4CO2NH2. b) Calculate K at 313 K.
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