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Problem- Acetic acid has a density 1.05 g/cm3 and mass percentage 99, calculate the molarity, molality, and mole fraction *100g of each solution * MW = 60.05
Solve the above problem in detail no word count
Problem- a) Decide which is more stable: an aryldiazonium cation, or a cyclohexyldiazonium cation? Use resonance structures to justify your answer. b) Upon heating to temperatures above 50oC, aryldiazonium salts decompose and evolve nitrogen gas.
given that the c-to-c bond in ethyne is a triple bond the average c-h bond energy in ch4 is 415 kjmol along with
a compound contains only c h and o. to analyze the compound you determine its empirical formula by analysis for c and h
A gas at 89.0°C occupies a volume of 0.67 L. At what Celsius temperature will the volume increase to 1.12 L
A 2.983 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.910 grams of KI and 50.00 mL of a 0.00894 M KIO3 solution.
Round pertinent Table 1 data to the nearest whole number and, at 3000K, calculate delta Gr and K for: H2O reacts with H(g) and OH(g). Show pertinent work but not arithmetic. Also append correct units to K.
a certain brand of antacid chewing gum was sent to the lab for testing and it was found to have 15 by mass of
A cylinder contains 975 grams of chloroform, CHCl3, How many atoms of carbon are in the sample? How many atoms of chlorine are in the sample?
In a separate experiment, it was found that, for fixed temperature and pressure, a 0.100 L sample of this compound takes 1.73 times longer to effuse than does a 0.100 L sample of Ar(g). What is the molecular formula of the compound? , draw possibl..
During a fire, it was expected by the fire department report that the tank temperature rose to 365 degrees Fahrenheit. Find out the pressure of the oxygen gas in the tank during the fire.
used the balance equation n2 o2-------2no to answer the following questions1.how many grams of no are formed from
Calculate the mass of aluminum deposited on the purified aluminum metal by the application of a current of 1.225 kiloamperes for 30 minutes from a very large quantity of a solution containing Al3+ ion in the Al2O3/Na3AlF6 molten state.
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