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The mass of the dry gas is 872 mg. A fragment of the tank indicates that the gas is a monoatomic element. Write out the full name of the gas.
A cylinder of compressed gas rolls off a boat and falls to the bottom of a lake. Eventually it rusts and the gas bubbles to the surface. A chemist collects a sample of the gas with the idea of tryin
Mixtures of helium and oxygen are used in scuba diving tanks to help prevent "the bends". For a particular dive, 18.9 L of oxygen gas at 25.0oC and 1.25 atm, and 7.58 L of helium gas at 25.0oC and 1
Rank the following compounds in order of lowest to highest melting point. KCl CH3-O-CH3 CH3-CH2-CH3 CH3-CH2-NH2
Determine the following characteristics of the titration curve for 25.0 mL of 0.400 M NH3(aq) titrated with 0.335 M HI(aq). (For NH3, Kb = 1.8x10-5.) (1a) The initial pH : (1b) The volume of HI(aq)
What is the strongest type of intermolecular force in the following compounds? dipole-dipole, london desperison or hydrogen bounding
Sodium hydroxide is slowly added to a 225 mL of a solution that is 3.0*10^-2 M Ba2+ and 1.5*10-3 M Cr3+. Which will precipitate first
Treatment of gold metal with BrF3 and KF produces Br2 and KAuF4, a salt of gold. Write a balance chemical equation and identify the oxidizing agent and reducing agent in the reaction
Write and balance the chemical equation for combustion of C13H24O. What is the sum of all of the coefficients in the correctly balanced chemical equation
Aluminum reacts with oxygen gas in a combination reaction to produce aluminum oxide. How many moles of oxygen gas are needed to react with 1.64 moles of aluminum
How many grams of precipitate are formed when 50.00 mL of 2.00 M NaOH and 30.00 mL of 0.125 M Fe(NO3)3 are mixed? Which one is limited
copper (II) iodide and ammonium acetate are soluble salts E. silver bromide and calcium acetate are insoluble salts F. nickel (II) bicarbonate and lead (II) sulfate are insoluble salts G. barium bro
The synthesis of imines and enamines typically occurs under mildly acidic conditions, yet the reaction that you will perform in this experiment is successful without the need of such acid. Why
Initial temp of HCL solution: 22 degree c Mass of magnesium: 0.6 g Moles of mag: 0.025 highest temp of mixture: 63 degree c Delta T: 41 degree c Heat gained by solution
I have 3 forms of a chemical BH+(aq), B(aq), B(organic), and other Ions H+(aq), OH-(aq), Na+(aq),Cl-(aq) in a solution. What would the charge balance be
Mass of magnesium: 0.6 g Moles of magnesium. Mass of magnesium oxide: 1.00 g Moles of magnesium oxide
A 2 mL sample was taken of a solution of barium iodate at 10 degree C. the sample was mixed with 2 mL of 0.5 M KI and 2 mL of 1M HCl. The transmittance of the mixture was read and compared to a cali
A bar house with volume of 500 m^3, has 50 smokers in it. Each begins to smoke 2 cigarettes per hour at time t=0 hr. An individual cigarette emits about 1.4 mg of formaldehyde (HCHO).
The transmittance of the mixture was read and compared to a calibration curve which indicated a concentration of I3^- as 5.52*10^-4 M. Calculate the following: c.) The concentration in moles/L of IO
The transmittance of the mixture was read and compared to a calibration curve which indicated a concentration of I3^- as 5.52*10^-4 M. Calculate the following a.) the molesof I3^- in the mixture
Calculate the pH at the equivalence point for the titration of 0.190 M methylamine (CH3NH2) with 0.190 M HCl. The Kb of methylamine is 5.0× 10-4.
Calculate the distances NH3 gas and HCL gas would travel in this experiment if a 100.00-cm tube were used, based on the accepted molar masses of the two gases.
A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H2S was bubbled through the acidic solution. A precipitate formed and was filtered off.
Calculate the change in pH when 4.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Calculate the change in pH when 4.00 mL of 0
What will be the concentration of Ca2 (aq) when Ag2SO4(s) begins to precipitate. What percentage of the Ca2 (aq) can be separated from the Ag (aq) by selective precipitation