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The most common experimental technique to perform elemental analysis is combustion analysis, where a sample is burned in a large excess of oxygen and the combustion products are trapped in a variety of ways. A 99.99% pure,0.4949g sample containing only carbon, hydrogen, and nitrogen is subjected to combustion analysis, resulting in the formation of 1.386g CO2,0.2817g H2O, and0.1877g NO. What is the empirical formula of the sample?
Weigh out some salt (sodium chloride) following the two methods described below. zero the balance, Weigh and record the mass of a 50-mL beaker.
A sample of gas with a volume of 750 mL exerts a pressure of 98 kPa at 30 c. what pressure will the sample exert when it is compressed to 250 mL and cooled to -25 degree celsius.
express the work of isothermal reversible expansion of a vanderwaals gas in reduced variables and find a definition of
A layer of peat beneath the glacial sediments of the last ice age has a carbon-14/carbon-12 ratio that is 21.4% of that found in living organisms. How long ago was this ice age
At a certain temperature, the equilibrium constant for the reaction 2HI(g)39. At a certain temperature, the equilibrium constant for the reaction 2HI(g) H2(g) + I2(g) is 0.49.
Question- A particular monochromatic green light source emits light with a frequency of 594 THz. What is the energy of a photon emitted from this light source
What is the mass of the product after the reaction between 250 mg of trans-cinnamic acid and 0.6 g of pyridinium bromide perbromide with 5% of impurities in 6 mL of acetic acid. Yield is 90%
Treatment of the bicyclic chloride A with lithium in tetrahydrofuran (THF) gave the monocyclic product B, C9H9Li. In deuterated THF, B exhibited a single proton NMR signal at 6.72 ppm
Explain what is the equilibrium constant for the reaction. Define what are the equilibrium concentrations of CaT(-), HCO3(-), and HT(2-) concentration in mol/L
identify the acid(proton donor) and base(proton acceptor) for the reactants in each of the following
The reaction between iron (III) oxide and aluminum, to produce aluminum oxide and iron, has a heat of reaction (ΔH) equal to -851.5 kJ/mole. How much energy is released if 0.56 moles of aluminum are consumed
The mixture did not rotate the plane of polarized light before. How had the mold changed the solution to become optically active?
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