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"Air" bags for automobiles are inflated during a collision by the explosion of sodium azide, NaN3. The equation for the decomposition is2NaN3(s) ? 2Na(s) + 3N2(g). What mass of sodium azide would be needed to inflate a 9.8-L bag to a pressure of 2.2 atm at 25°C?
It is assumed that the relative standarddeviation of the method is sr ? s = 4 ppt forcarbon and 6 ppt for hydrogen. The means of the reported resultsare 68.5% C and 4.88% H. At the 95% confidence level, is there anyindication of systematic error i..
consider the following equilibrium system H2(g)+ Br2(g)=2HBr(g) Keq= 14.8 A closed container is initially filled with equal moles of H2 and Br2.When equilibrium is reached the (HBr) is 0.329 mol/L What is the initial (H2)
What is the molar mass of the unknown gas? Express your answer to four significant figures and include the appropriate units.
For the saturated fatty acid palmitate, how many QH2, NADH, and acetyl-CoA molecules can be generated by complete ?-oxidation? How many total ATP can be produced from palmitate? If a single cis-double bond is added, how many total ATP can be made?
Who does the first ionizaiton energy of the alkali metal in a given period compare with the first ionization energy of the halogen in the same period. What is the result in terms of how these elements tend to react with each other
calculate the concentration of all soluble Hg(II) species. Which Hg(II) species is most prevalent? Assume there are no solids present, that the major ligands present are Cl- and OH-, and ignore activity corrections.
At least how many standard solutions would you need to make calibration graph, assuming that the graph is expected to be a straight line? Explain your answer. Do not include the data from distilled water
Calculate the molality of a hydrochloric acid solution that is 26.4% by mass and has a density of 1.19 g mL^-1
At standard temperature, a gas has a volume of 241 mL. The temperature is then increased to 138C, and the pressure is held constant. What is the new volume?
C2H6+O2 ---> CO2+H2O Calculate the mass of H2O that should form if 1.5 g of C2H6 is combusted in the presence of 2.5 g of O2.
Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO3 and 295 mL of water. Density of water is 0.997 g/mL.
The mass of 322 mL of hydrogen gas at 4.0 atm and -73°C is 1.21 grams. What is the density of hydrogen gas at STP?
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