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Hydrogen sulfide is found at a concentration of 3 parts per million in air. Using the temperature and pressure conditions that are considered "standard" for air quality work, this concentration means that there are [Blank] milligrams of hydrogen sulfide in each cubic meter of air. Report your answer to the nearest 100th (0.00) of a milligram.
if you had excess chlorine how many moles of of aluminum chloride could be produced from 17 grams of aluminum
To a second 25.00 mL part, 10.00 mg of lead was added and extracted into a second 10.00 mL portion of the same organic solvent. This solution gave A = 0.525. What was the concentration of lead, in mg/mL, in the original sample?
Determine what type of bond is expected for a compound formed between Magnesium and Oxygen Based on these values,?
A student following the procedure in this experiment prepared three solutions by adding 11.50, 23.00, and 34.50 mL of a 7.60 x 10-2M NaOH solution to 50.00 mL of a .112M solution of a weak acide.
Detremine the volume of CO2 produced at the temperature of 23 degree celsius and pressure of 0.985atm?
A student has spilled some acid onto their arm. One lab partner suggests pouring some base on it to neutralize the acid but the TA quickly interjects that would be a bad idea and has the student begin washing their arm
Calculate the density of Slackium Oxide. (g/cm^3) What is the Volume of unit cell (cm^3)
What is the concentration of the HNO3 solution? (b) How many moles of NaOH were in excess after the first addition?
Calculate the solubility (in M units) of ammonia gas in water at 298K and a partial pressure of 6.50bar . The Henry's law constant for ammonia gas at 298K is 58.0 M/atm
The atomic mass of boron is 10.81 g/mol. The two naturally occuring isotopes are B-10 with a mass of 10.0129 amu and B-11 with a mass of 11.0093 amu. Determine the percent of naturally occuring B-10.
Calculate the number of moles in each of the following quantities.a) atoms of each element in 3.35 moles of aspirin(C9H8O4)
What is the theoretical yield of bromobenzene in this reaction when 30.0 g of benzene reacts with 65.0 g of bromine?
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