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Calculate the mass of ethylene glycol, C2H6O2 , that must be added to 1.000 kg of ethanol, C2H5OH, to reduce its vapor pressure by 13.2 torr at 35°C. The vapour pressure of pure ethanol at 35°C is 1.00 x 10 -2 torr.
The molar heat capacity of silver is 25.35 J/mol * C. How much energy would it take to raise the temperature of 8.60 g of silver by 11.1 C?
If the heat of combustion for a specific compound is -1390.0 kJ/mol and its molar mass is 61.39 g/mol, how many grams of this compound must you burn to release 821.90 kJ of heat.
Suppose that 160 g of ethanol at 30?C is mixed with 230 g of ethanol at 76?C at constant atmospheric pressure in a thermally insulated vessel.
Considering the mixture of the two compounds and range of the melting points, the reason recrystallization was difficult was due to a broad melting point range.
What is the pKa for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?
Determine the molar mass of the substance if 120.0 grams of a pure sample contained 24.0 mol of the substance. Express your answer in g/mol.?
2.914 gram sample of gypsum, a hydrated salt of calcium sulfate, CaSO4, is heated at a temperature greater than 170 degrees celcius in a crucible until a constant mass is reached.
Consider a cylindrical container partially filled with ethanol (C2H6O). Using the model in which ethanol vapor pressure is a result of equilibrium between the rate of ethanol evaporation and condensation.
A student analyzed and recorded two potassium emission spectra: 1) one using 0.10 M Potassium sulfate solution; 2) one using 0.10M Potassium nitrate solution;. Determine why will significant differences be observed in the two emission spectra.
Use the density of copper (8.95 g/cm3) and its molar mass (63.55 g/mol) to calculate an approximate atomic radius for copper.
A sample of chlorine, which has an average atomic mass of 35.86, consists of two isotopes with mass of 35 and 37. What is the percent (to 0.1%) abundance of the 37 isotope?
Estimate the heat released when ethene CH2 CH2 reacts with hydrogen gas to give CH3CH3.
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