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A 1.0 µL sample of an equal volume mixture of 2-pentanone and 1-nitropropane is injected into a gas chromatograph. The densities of these compounds are 0.8124 g/mL for 2-pentanone and 1.0221 g/mL for 1-nitropropane.What mass of each compound was injected?The peak areas produced on this injection were 1917 units for 2-pentanone and 1717 units for 1-nitropropane. Calculate the response factor for each compound as area per mg.An unknown mixture of these two components produces peak areas of 1501 units (2-pentanone) and 1712 units (1-nitropropane). Use these areas and the response factors above to determine the weight % of the components in the unknown sample.
a mixture of gases containing .20 mol of SO2 and .2 mol of O2 in a 2.0L flask reacts to form SO3. If the temperature is 25C, what is the pressure in the flask after reaction is complete?
calculate the number of moles of AgCrO4(Ksp=9.0x10^12) that will dissolve in 1.00L of 0.010 M K2CrO4 solution. what will be the ion concentrations at equilibrium?
Which of the following chlorides is the most ionic. Please explain a) CH2Cl2 b) SiCl4 c) SCl2 d) PbCl2
Specify what ions are present in solution upon dissolving each of the following substances in water. ZnCl2
a throttling valve has inlet conditions of saturated vapor r-134a at 600 kpa exits at 240 kpa. the kinetic energy in
calculate the mass percent, the mole fraction, and the partial pressure of CO2 in the container after cooling back down to the initial temperature.
Calculate the [CH3CO2H] ionized in solution for 0.1M acetic acid knowing that ph= 2.9 [H+]= 1.26 x 10^-3 M , [OH-]= 7.94 x 10^-12 M
a solution is made by mixing 500 ml of .167 m naoh with 500 ml of .1 m ch3cooh. calculate the equalibrium
hydrogen is collected over water, two gases are present hydrogen and water vapor.calculate partial pressure of hydrogen gas. Barometric pressure = 773.94 mmhg.
For the following reaction, 5.07 grams of carbon disulfide are mixed with excess chlorine gas. The reaction yields 9.09 grams of carbon tetrachloride.
tris acid dissociation constant is 8.32 x 10 -9. I have 0.1 m soln of tris in protonated form, o.1m soln of HCL and NAOH, and ample distilled water. Describe the preparation of 1L soln of 0.02m tris buffer, ph is 7.8
what is the solubility of O2 at an elevation of 12,000 ft where the atmospheric pressure is 0.657 atm? Assume the temperature is 25°C, and that the mole fraction of O2 in air is 0.209 at both 12,000 ft and at sea level.
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