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The experimental melting point we obtained at the end for the cis and trans mixture of 4-t-butylcyclohexanols was 68-70 degrees Celsius. How do you interpret the experimental MP for this lab when the theoretical melting point is 82-83 for trans and 81-82 degrees for cis? Does it melt as expected for a mixture of cis and trans isomers?
Explain what it means that the atomic mass of naturally occurring Ag, is a mixture of its two isotopes forms, is 107.868 u.
a positive ion ESI mass spectrum of a protein showed a peak at m/z = 1001 resulting from the adition of 10 protons. what is the actual mass of the uncharged protein?
At a constant pressure of 1.50 atm what is the enthalpy change delta H for a reaction where the internal eneergy change delta E is 58.0 kJ
Calculate the heat that must be supplied to 0.104g of Ne(g) at 0.250 atm to raise its temperature from 22.0 degree Celsius to 60.0 degree Celsius at
The densities of ice and water at 0 C are 0.9168 and 0.9998 respectively. if delta h for the fusion process at atmospheric pressure is 0.625 what is delta u.
In an airplane, a gas sample occurs at a volume of 1.5 L at 760.0 torr. Suppose, while flying, the airplane loses pressure and the volume of the gas increases to 11.40 L.
Express your answer to three significant figures and include the appropriate units. 0.037 Correct Part B What pressure is required to achieve a concentration of 7.10×10?2 at 20?
change in enthalpy at 25 C and 1 atm for the reaction of 5.00 mol of elemental iron with excess oxygen gas?
The pH at 25 °C of an aqueous solution of the sodium salt of p-cresol (NaC7H7O) is 11.60. Calculate the concentration of C7H7O- in this solution, in moles per liter. Ka for HC7H7O is equal to 6.7E-11.
Calculate the molarity and mole fraction of a 1.43 m solution of acetone (CH3COCH3) dissolved in ethanol (C2H5OH). (Density of acetone = 0.788 g/cm3; density of ethanol = 0.789 g/cm3.)
If a sample of 0.230 grams of KCN is treated with an excess of HCL, calculate the amount of HCN formed, in grams.
A student followed the procedure of this experiment to determine the solubility product of zinc(II) iodate, Zn(IO3)2. Solutions of ZN(NO3)2 of known initial concentrations were titrated with 0.200 M KIO3 solutions to the first appearance of a whit..
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