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Would the change in entropy associated with the construction of an octahedral field of ligands about a metal ion be positive or negative? Briefly explain ( I think it's positive but I'm having a tough time explaining). Does this result mean that the change in enthalpy of this process must be negative in order for the process to be spontaneous under standard state conditions? How come?
A solution of 62.4 g of insulin in enough water to make 1.000 L of solution has an osmotic pressure of 0.305 atm at 25°C. Based on these data, what is the molar mass of insulin?
Calculate the mass of ethylene glycol required to lower the freezing point of 200 mL of water/ice by 4.5 degrees celsius. The K(f) for H20 is 1.86 degrees celsius/m. Assume the density of water is 1.00 g/ml.
Use the appropriate standard reduction potentials to calculate the value
An engineer was trying to minimize greenhouse gases from car exhaust and was studying the gases that come from the trail pipe of a car at 800K.
LDA is added to a solution containing methyl pentanoate. After this reaction has gone to completion, 2-butanone is added. Once this reaction is completed an acid workup is performed.
what is the K value for compound Z in the biphasic system, 2) how much do you remove in each individual extraction
Calculate the change in pH when 6.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq)
The normal melting point of benzene is 5.5 degrees Celsius . For the process of freezing, what is the sign for each of the following
(a) Calculate the standard molar enthalpy change (deltaHrxn°) at 400 K (not 298 K) for the following reaction (the cyclotrimerization of ethyne to benzene)
The compound [Fe(CO)4(PMe3) could adopt a trigonal bipyramidal geometry with the phosphine in either an axial or an equatorial position. (a) Indicate the point group of the molecule
If 31.82 g of a metal oxide reacted with excess carbon and 4.08 L of CO2 formed at 100 C and 1.5 atm what is the identity of the metal
Assume you can heat up or cool down the reaction flask as needed for the reaction to proceed with practical rates even if no temperature is indicated in the table
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