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A bottle contains 6.0 fluid ounces of alcohol. What is the mass of alcohol in the bottle?
Note: 1 fluid ounce = 29.56 mL; the density of the alcohol is 0.87 g/mL.
A solution is prepared by dissolving 0.15mol of acetic acid and 0.15mol of ammonium chloride in enough water to make 1.0 L of solution. Find the concentration of ammonia in the solution.
The activation energy for a particular reaction is 64 kJ/mol. By what factor will the rate constant increase when the temperature is increased from 50 oC to 80 oC
Explain why the Rf values changed when the eluant was changed from 100% petroleum ether to a 95:5 mixture of petroleum ether-ethyl acetate.
A 20.5 g sample of protein dissolved in water to prepare 500ml solution shows an osmatic pressure of 3.72 torr at 27 degrees C. Estimate the molar mass of the protein
How do you determine what pH range a certain solution would be a good buffer in?
what mass of KO2 in grams is required to react with 8.90-L of CO2 at 22.0 C and 767mm Hg? first calculate the number of moles of CO2 (R=0.08026 L*atoms/ mol*K) find moles of Co2 and mass of KO2 in grams?
Question- How many ounces of mercury are in 1.0 cubic meters of mercury. Given- the density of mercury is 13.55g/cm3 and 1 ounce =28.35g
Cannot be determined from the information provided. 9. Starting with the initial concentrations provided in the question above, what will be the equilibrium concentration of CO2? a) 1.6 M b) 1.8 M c) 2.0 M d) 2.2 M 10. What is KC for this process ..
what minimum mass of succimer in rm mg is needed to bind all of the lead in a patients bloodstream? assume that patient
Determine the mass of 28.56 mL of acetone and express your answer in grams? also find out the volume, of 6.54 g of acetone and express your answer , in mL?
Consider two analgesics derived from salicylic acid: acetylsalicylic acid (aspirin) and methyl salicylate (oil of wintergreen, found in muscle relaxants like "BenGay").
A 4.00-g sample of iodine was reacted completely with excess bromine. The mass of the compound formed was 11.56 g. Determine the empirical formula.
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