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Problem- What is the mass in grams of 0.0015 mol of aspirin, C9H8O4? How many aspirin moleclues are there in this 0.0015 mol sample?
I want you to clarify the chemistry in the above problem
Why does it not make sense to think of sand as just being composed of a bunch of SiO2 molecules
Treatment of cyclohexanone in the presence of sodium borohydride results in a product that can be isolated and purified using distillation. The IR spectrum of this product is shows a very broad peak at 3331cm-1, peaks to right of 3000cm-1
Calculate the volume (in mL) of He collected at STP when 3.60 g of pure 226Ra is stored in a closed container for 135 years.
An empty beaker weighs 41.19 g. When it is completely filled with water (density = 1.0 g/mL), the beaker weighs 92.92 g.
Much commercial hydrochloric acid is prepared by the reaction of concentrated sulfuric acid with sodium chloride: H2SO4 + 2NaCl → Na2SO4 + 2HCl
Diphenylethyne can be prepared from meso-1,2-dibromo-1,2-diphenylethane, by double E2 elimination via the corresponding alkene. a) Which alkene is initially formed?
What volume (in milliliters) of 0.100 M NaOH should be added to a 0.120 L solution of 0.024 M glycine hydrochloride
Draw the skeletal structure of meso-2,6-diaminopimelic acid (meso-2,6-diaminoheptanedioic acid). (Show one wedge bond, one dashed bond, and two sticks attached to the chiral carbon.
What is the value of x in the formula for the hydrate? (hint: remember that x represents the ratio of moles of H2O to moles of hydrate compound, and that moles of hydrate compound equals the moles of anhydrous compound)
1.285g sample of Na2SO4 is exposed to the atmosphere and found to gain 0.393g in mass. What is the percent, by mass, of Na2SO4*H2O in the resulting mixture of anhydrous Na2SO4 and the decahydrate
how much water would be needed to completely dissolve 1.78 of the gas at a pressure of 730 and a temperature of 27? a
In the lower troposphere, ozone is one of the components of photochemical smog. It is generated in air when nitrogen dioxide, formed by the oxidation of nitrogen monoxide from car exhaust, reacts by the following mechanism.
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