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When 0.78 g of an unknown gas in contained solely in a 560 mL container, the pressure is 780 Torr at 5 degrees Celcius. What is the molar mass of the gas in grams/mole?
When relatively small amounts of magnesium burns, the fires are extinguished using commercially available dry powder. Why might this fire rekindle days later as someone tries to remove the residue with water?
In the tin oxide laboratory activity, what was the color of the vapor emitted when the nitric acid was added to the tin.
0.158g of a barium halide is completely precipitated out of H2SO4 and 0.124g of barium sulfate are produced. what is the true formula of the compound.
Which of the following molecules would be expected to be MOST water soluble?
Calculate the volume of a balloon at the final temperature if this balloon at temperature of 279K and an initial volume of 2.3L is warmed to 406K.
The specific heat capacity of silver is 0.240 J/(g x degrees C). Calculate the energy (in kJ) required to raise the temperature of 263 g Ag from 273K to 278 K.
2KClO3 + heat > 2KCl + 3O2, How many moles of O2 form as 3.0 mol of KClO3 are totally consumed.
Calculate the molarity of 52.56 grams of Al2(SO4)3 in 1.80 L of solution.
Consider the following reaction: CO(g)+H2O(g)in equilibrium with CO2(g)+H2
At 20 degrees C the vapor pressure of pure methanol (CH3OH) is 89.0 torr and of pure water (H2O) is 17.5 torr. A solution of methanol and water has a total vapor pressure of 52.9 torr at 20 degrees C.
The wavelength corresponding to threshold frequency to tungsten surface is 230nm . Calculate the kinetic energy of the photoelectron ejected from the surface of tungsten metal.
Compute the concentrations of all species in a 0.900 M sodium sulfite solution. If it is given that the ionization constants for H2SO3 are Ka1=1.4x10^-2 and Ka2=6.3x10^-8.
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