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A 1.6 g sample of a molecular compound is dissolved in 104 g of tetrachloromethane (carbon tetrachloride). The normal boiling point of the solution is 61.51degreesC, the normal boiling point of CCl4 is 61.2degreesC. The boiling point constant for CCl4 is 4.95 K · kg/mol. What is the molar mass of the compound? Answer in units of g/mol
A 135 mL sample of a 15.0 M ethylene glycol (rm C_2H_6O_2) solution is diluted to 1.50 L.What is the freezing point of the final solution.
Find out what will be the half-lives if [NOBr]o = 0.054 M - The rate constant for the second order reaction Is 0.80 M-1s-1 at 10 degree celsius temperature
A 100 mm diameter silicon wafer is oxidized completely. What is the thickness of the resulting SiO2 wafer? The molecular weight of Si is 28 g/mol and of SiO2 is 60 g/mol.
How many moles of methane occupy a volume of 2.00 l at 50.0*C and0.500 atm? (R=0.0821 atm*L/molxK)
A solution is made by mixing 506 mL of water and 198 mL ethanol. What is the concentration of ethanol in units of volume/volume percent.
Calculate the heat of neutralization when it is given that : heat capacity of the calorimeter =28.7 J/oC ,the specific heat of the mixture =4.184 J/goC, density of the solution =1.02 g/mL.
A 250.0 mL aliquot of 2.50 M H2SO4 solution is mixed with a 250.0 mL aliquot of 4.00 M HNO3 solution. What is the molarity of hydrogen ions in the combined solution.
Consider the following data: expect a BeF2 molecule to be linear but an SF2 molecule to be angular. Explain the decreasing melting point from NaF to Nai.
A 0.1752g sample of silver nitrate was dissolved in 502.3g of distilled water. Calculate the weight molarity of silver in this solution.
An unknown mass of each of sand, initially at 24.0, absorbs 1970 of heat. The final temperature is 62.2 degrees C. Find the mass of sand.
Calculate how many atoms of potassium A three mole sample of K2S would have and Calculate the current for diffusion-controlled electrolysis
The enthalpy of formation of ethanol, C2H5OH, is 277.o kJ/mol at 298.15K. Calculate the enthalpy of combustion of one mole of ethanol, assuming that the products are CO2 and H2O.
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