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Determine the molar volume (in cm^3/mol) of carbon (diamond) by using the density of diamond (3.51 g/cm^3) and the mass of a mile of carbon (12.01 g/mol)
When the ore lead (ll) sulfide burns in oxygen, the products are lead (ll) oxide and sulfur dioxide. Part A: Balance the equation: express the answer as a chemical equation. identify all of the phases in your answer
what is the pressure in torrs of the volume of a sample of a gas is 7.6 liters when 0.46 moles of gas are at 54 degrees
On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of the following pairs.
Each 1.000 g of 238U that decays eventually produces 0.866 g of 206Pb. If the half-life of 238U is 4.468 x 10^9 years, what is the age of a mineral that has a 238U/206Pb mass ratio of 2.00?
Assuming 100% dissociation, calculate the freezing point and boiling point of 1.83 m AgNO3(aq). Constants may be found here.
The partial molar volumes of water and ethanol in a solution with x(H2O) = 0.40 at 25 degrees C are 16.9 and 57.5 cm^3/mol, respectively.
A 1.0 ounce piece of chocolate contains 15mg of caffeine, and a 6.0 ounce cup of regular coffee contains 105mg of caffeine. How much chocolate would you have to consume to get as much caffeine as you would from 2.0 cups of coffee.
chlorine dioxide clo2 si a reddish-yellow gas that is soluble in water. in basic solution it gives clo3- and clo2-
If each mole of gas occupies 59 L under the conditions of the explosion, how many liters of gas are produced. Express your answer using two significant figures. How many grams OF N2are produced in the detonation
Above what Fe2 concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 9.39? The Ksp of Fe(OH)2 is 4.87×10-17
The side chains of asparagine and glutamine can undergo hydrolysis in aqueous acid. Draw the reactants and products for the deamination reaction. Name the products.
A 2.000-L flask was filled with 0.0393 mol SO2 and 0.0197 mol O2. At equilibrium at 907 K, the flask contained 0.0299 mol SO3. How many moles of each substance were in the flask at equilibrium
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