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If large quantities of chloroform an anesthetic, carbon tetrachloride (commonly utilized in the past for dry cleaning, and tetrachloroethene previously used as a degreasing agent were spilled in the environment, which compound would you expect to have higher concentrations in the air above the site explain your answer.
consider the decomposition of liquid benzene to gaseous acetylene according to the following reaction C6H6=3C2H2 what is the delta H for the formation of 1 mole of acetylene?
Pure gold has a density of 19.32 g/cm3. How large would a piece of gold be if it had a mass of 318.97 g
we place an excess ( more than can dissolve) of PbCl2 into 100 ml. of water and find that at equilibrium [Cl]=0.032 M . Calculate kc for the following reaction : PbCl2 = Pb+2Cl
Starting with butyramide as your only source of carbon, make butyl butyrate.
Two 20.0-g ice cubes at -16.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.
hexane has a normal boiling point of 68.7 c. what is the mole fraction of a nonvolatile solute in a hexane solution
The reduction reaction has the product 4-tert-butylcyclohexanol which is a mixture of cis and trans isomers. Methanol is the solvent, but I don't think that goes into the balanced equation.
For the strong base solution 4.0×10?3 M Ca(OH)_2, determine [OH^-], [H_3O^+], pH, and pOH.
Calculate the amount of energy needed in calories to heat 145 g of water from 22.3 degrees celsius to 75.0 degrees celsius. (water in j/g degree celsius = 4.184, cal/ g degree celsius = 1)
A sample of a gas in a piston/cyclinder apparatus occupies 33.1 mL at 1.14 atm and 23.3°C. If the volume of the sample is increased to 77.4 mL and the temperature changes to 39.9°C, what is the new pressure, in atm, of the sample
A thermometer containing 9.5 of mercury has broken. If mercury has a density of 13.6 , what volume spilled?
Calculate the percent error in your Hess's Law enthalpy value (-686 kJ/mol). The accepted textbook value is -601.7kJ/mol.
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