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Explain A sample of an unknown gas effuses in 10.9 min. An equal volume of H2 in the same apparatus under the same conditions effuses in 2.18 min. Define what is the molar mass of the unknown gas?
nitrogen and hydrogen gases react to form ammonia gas as followsn2g3h2g--gt2nh3gat a certain temperature and pressure
Iron has a density of 7.9 g/ cm3. What is the mass of a cube of iron with the length of one side equal to 55.0 mm.
how can we calculate the weight of CaCO3 per 10^6 ml unknown sample.the weight of CaCO3 per 25 ml of unknown sample is 5.71*10^-3
Which of the following ideal aqueous solutions would be predicted to have the highest boiling point
Consider formic acid, HCOOH (Ka= 1.9 x 10^-4) and its conjugate base, HCOO^- with a Kb of 5.3 x 10^-11. Write a net iconic equation for the reaction in aqueous solution between HCOOH and NaOHl, and calculate K.
22.05 mL of a sodium hydroxide solution is needed to react completely with 0.5210 g of KHP (molar mass+204.22) What is the concentration of the sodium hydroxide solution
Consider the mechanism of reduction of WO3. At least two mechamisms are possible to the formation of HxWO3 during intercalation of WO3
What causes the colors of fireworks. Where do the colors come from? How do we get so many different colors. Give at least onr example of a compound responsible for such characteristic color.
How many milliliters of a 0.150 M magnesium hydroxide solution are needed to neutralize 1.282 L of a hydrochloric acid solution that is 0.1048 M
A voltaic cell consists of a Hg/Hg2^2+ electrode(E degrees=0.85V) and a Sn/Sn^2+ electrode(E degrees=-0.14V). Calculate[Sn^2+]if [Hg2^2+]=0.36 M and Ecell=1.04V at 25 degrees C.
Determine the maximum number of electrons that could be emitted from metal by a burst of light with a total energy (E)of 9.86× 10^(-7) Joules?
The equilibrium constant for the reaction H2(g) + I2(g) 2HI(g) is 62.5 at 800 K. What is the equilibrium concentration of I2 if at equilibrium [HI] = 0.22 M and [H2] = 0.10 M
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