history of Nanotechnology

Congenital Galactosemia typically appears only in infants because with maturation, most children develop another enzyme capable of metabolizing galactose. Its incidence is about 1 per 18,000 births. If the infant does not receive treatment then there is a 75% chance of death. Thus, in the United States infants are screened for galactosemia. Galactosemia can be confused with lactose intolerance but galactosemia is a considerably more serious condition because consumption of galactose can cause permanent damage to their bodies. What dietary changes should be made?

Compound (A) forms only proprionaldehyde (B) upon ozonolysis and reduction with (CH3)2S. Treatment of (A) with aqueous chlorine affords (C) (C6H13ClO). Exposure of (C) to aqueous NaOH produces racemate (D) (C6H12O). (Think about intramolecular SN 2 reaction Williamson ether synthesis). Compound (D) is also formed by the reaction of peracid with (A). What are the structures of (A), (B), (C) and (D)? Illustrate and explain. Show mechanism of aqueous chlorine reaction and indicate the arrows and lone pairs.

The following reaction forms 15.8 g of Ag:

2 Ag2O---> 4 Ag + O2

What total volume of gas forms if it is collected over water at a temperature of 25 and a total pressure of 752mmHg?

At STP how many grams of Mg are required to produce 245 mL of H ₂ in the reaction shown below?

Mg(s) + 2 HCl(aq) → H₂(g) + MgCl₂(aq)

I would appreciate any help with this,

thanks :)

Suppose you carried out the catalyst trial. Could you calculate, from your data, the value of Ea
for the reaction catalyzed by copper? If not, what additional experimental data would you
require in order to be able to do this? Would the value of Ea be greater or less than that
obtained for the uncatalyzed reaction? Explain. Please type your answers.

Calculate the pH after 0.17 mole of NaOH is added to 1.06 L of a solution that is 0.54 M HCO2H and 1.16 M HCO2Na, and calculate the pH after 0.34 mole of HCl is added to 1.06 L of the same solution of HCO2H and HCO2Na.

0.17 mole of NaOH

0.34 mole of HCl

the vapore pressure of ethanel ( C2 H5 OH) at 20 degree C is 44mmHg and the vaper pressure of methol ( CH3 OH) at hte same tempature is 94mmHg. a mixture of 26.9g of methanol and 49.7g of ethanol is prepared and can be asumed to behave as an ideal solution.

calculate the vapor pressure of methanol and ethanol above this solution at 20 degree C?

calculate the mole fraction of methanol and ethanol in the vapor above this solution at 20 degree .C?

In a laboratory experiment, students synthesized a new compound and found that when 11.77 grams of the compound were dissolved to make 253.3 mL of a benzene solution, the osmotic pressure generated was 3.94 atm at 298 K. The compound was also found to be nonvolatile and a non-electrolyte.  


What is the molecular weight they determined for this compound?

b) Methoxide ion, CH3O , and amide ion, NH2 , are very strong bases commonly used in organic solvents. However, both bases are

1) What volume of 17.4 M acetic acid should be used to produce 0.100 L of 3.00 M acetic acid solution?

2) Given the following thermochemical equation, how much total energy is released when 1.50 kg of CH₄ is combusted?:
CH₄ (g) + 2O₂ (g) -----> CO₂(g) + 2H₂O (l)

Thank you!!

Starting with the 0.1250M Cu(NH3)+2 as the stock (concentration) calculate the following concentrations of the dilute solutions showing work:

15mL stock diluted to 20mL

10.0mL of stock solution diluted to 20.0mL

5.0mL of the stock solution diluted to 20.0mL

Demonstrate by a “microstate analysis” that four electrons in a degenerate set of three p‐orbitals gives rise to the same electronic state

113 “terms” as two electrons do (i.e. ¹D, ¹S and ³P)

2.5 grams of a metallic sample containing an unknown amount of zinc is dissolved in 500 ml of acidic water, releasing the zinc into the water as Zn²⁺ ions. A 10.00 ml aliquot of this solution is extracted with 10 ml of CCl₄ containing an excess of 8-hydroxy quinoline. The CCl₄ and aqueous phases separate and 8-hydroxy quinoline forms a fluorescent complex with Zn²⁺ ions that partitions entirely into the CCl₄ phase. The CCl₄ phase is separated and then diluted to 25 ml. This solution gives a fluorescence intensity of 155 (arbitrary units). A similar procedure is done with 10.00 ml of the unknown zinc solution plus 8.00 ml of an aqueous 2.50 ppm Zn²⁺ solution, and the final fluorescence intensity is 247. Calculate the Zn²⁺ concentration in the original 500 ml solution and the amount of zinc in the original solid.