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Leaded gasoline was banned in Canada in 1990. The additive was a compound containing carbon, hydrogen and lead (Pb). When 51.36 g of this compound was burned in excess oxygen, 55.90 g of CO2 and 28.61 g of H2O were produced. Determine the empirical formula of the compound.
Ethanol (without catalyst) yields a di-ether in nearly quantitative yield. Provide the structure of the product. Mechanistically, provide two routes that accound for the observed product.
A gas mixture composed of helium and argon has a density of 0.727g/L at a 755mmHg and 298K .What is the composition of the mixture by volume?
How many photons are required to heat 255 mL of coffee from 25 degrees celcius to 62 degrees celcius?
What is the molarity of the Na 2 S 2 O 3 solution if a 0.150 g sample of KIO 3 required 10.7 mL of Na 2 S 2 O 3 solution for its standardization?
When 157mg of dipentylamine was added to 122mg of benzoic acid and 2 mL of water, a completey homogenous solution was formed. Draw the structures of the species present in water.
what fraction of the day's energy does walking one hour represent? How many kilograms of water would have to be evaporated if this were the only means of heat loss?
a 4.0 gram sugar cube is dissolved in a 350 milliliter teacup. what is the molarity of the sugar solution.
what and how much effect does this have on the measured pressures? What is the effect on the value of?
A solution is made by mixing 12.0 g of NaOH and 75.0 mL of .200 M HNO3. Write a balanced equation for the reaction that occurs between the solutes. Calculate the concentration of each ion remaining in solution. Is the resultant soluiton acidic or ..
A 2.30-g sample of a large biomolecule was dissolved in 16.0 g of carbon tetrachloride. The boiling point of this solution was determined to be 77.85°C.
Would you expect to recover 100% of the desired compound from an impure sample using solution recrystallization?
For the following reaction, if 11.2 L of Nitrogen are reacted to form NH3 at STP, How many liters of Hydrogen will be required to completely consume all of the nitrogen.
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