The solubility (i.e. the maximum molarity at equilibrium) of N₂ gas in blood at 37^oC under a nitrogen partial pressure of 0.80 atm is 5.6 x 10^-4 mol.L^-1. When swimming at large depth in the ocean, a diver breathes compressed air with a partial pressure of N₂ equal to 4.0 atm. Henry’s law indicates that the solubility of N₂ gas increases with pressure. Assume that the total volume of blood in the body is 5.0 L. Calculate the amount of N₂ gas in the diver’s blood before diving. Calculate the amount of N₂ gas in the diver’s blood as he is breathing compressed air with a partial pressure of N₂ equal to 4.0 atm. Calculate the amount of nitrogen gas (in liters) that must be released when the diver returns to the surface of water, where the partial pressure of N₂ is 0.80 atm.

What are the drift speeds of Li+, Na+, and K+ in water when a potential difference of 10 V is applied across a 1.00 cm conductivity cell? How long would it take an ion to move from one electrode to the other? In conductivity measurements it is normal to use alternating current: what are the displacements of the ions in centimeters during a half cycle of 1.0 kHz applied potential.

The experiment is: analyzing food products for vitamin C. "Determine the amount of vitamin C (ascorbic acid) in different food products by oxidation- reduction titrimetry."

A student performed the experiment described in this module. She first standardized her DCP solution by preparing an ascorbic acid solution containing 46mg of reagent-grade ascorbic acid. Three 10.00mL samples of the ascorbic acid solution required an average of 25.7mL of titrant for the complete reaction.

1)calculate the mean molartity of the DCP solution.

The student titrated three 25-mL samples of a commercial orange "drink". These samples required an average of 14.2 mL of the DCP solution for a complete reaction.

2.) calculate the mass of ascorbic acid present in 25 mL of the orange drink

3.) calculate the number of milligrams of ascorbic acid present in 1 L of the orange drink.

Finally, the student used DCP titration to analyze the extract from the 4.00 g of fresh spinach. The titration required 23.2 mL of DCP solution

4) calculate the mass of ascorbic acid in 4.00 g of spinach assuming that all of the ascorbic acid in the spinach was contained in the extract

5.) which would supply more vitamin C a fresh spinach salad containing 100 g of spinach or a 4 oz glass of orange drink described above? one ounce equals approximately 30 mL

6.) would you expect the ascorbic acid content of spinach increase, descrease, or remain the same after the spinach has been steamed, prior to serving? briefly explain

Use the following data for water at 25 degrees C to answer this question. DeltaHfm(H2O)(l) = -285.830 kj/mol, DeltaHfm(H2O)(g) = -241.818 kJ/mol, DeltaGfm(H2O)(l) = -237.129kJ/mol, DeltaGfm(H2O)(g) = -228.572 kJ/mol

A) calculate the vapor pressure of water at 25 degrees celcius (hint: calculate the equilibrium constant for the "reaction" H2O(l) to H2O(g))
B) calculate the normal boiling point of water (pH2O)= 1 atm
C) why does the answer to part b differ from 100 degrees C, the correct normal boiling point of water?

Complete the following: ( NOTE: Formulas should be entered like the following example: potassium sulfate - K2SO4 , another example: zinc nitrate - Zn(NO3)2 )

Compound              Ionic or Covalent                  Formula

sodium oxide                                                

iron(III) bromide                                           

sodium carbonate                                          

carbon tetrachloride                                       

nitrogen tribromide                                        

Consider the titration of 50.00 mL of 0.200 M thioglycolic acid, H2SC2H2O2 (Ka1 = 2.3 x 10 -4 and Ka2 = 2.5 x 10 -11) with 0.500 M NaOH and calculate the pH after the following volumes of NaOH have been added. a) 0.00 mL b) 7.00 mL c) 20.00 mL d) 32.00 mL e) 40.00 mL f) 43.00 mL

1. Construct the titration curve, for the titration of 50.0 mL of 0.125 M trimethylamine with 0.175 M HCl (aq).

A. Calculate the initial pH of the solution in the flask.

B. Calculate the pH after 15 mL of titrant is added.

C. Calculate the pH at the equivalence volume.

D. Calculate the pH after 45 mL of titrant is added.

E. Calculate the pH after 60 mL of titrant is added.

Please make sure to include the titration curve and show your work!

Hello! We just had a lab where we took measurements of a water-ethanol mix with a densitometer and got volume of ethanol/(total volume of ethanol and water together) and I am stuck on how to convert that to mole fraction of ethanol? Thank you so much!

2 NOCl(g) <=> 2 NO(g) + Cl2(g), K= 1.6E-5. Calculate the concentrations when:

a). 6.0 mol of NO and 2.0 mol of Cl2 in a 1.2-L flask

b).  2.2 mol of NOCl, 2.2 mol of NO, and 1.1 mol of Cl₂ in a 1.0-L flask

c).  1.01 mol/L concentration of all three gases

Please show work and don't just solve the top problem. I need all three and I don't know how to correctly solve either of them!!

Which of the following reactions have a positive ?Srxn? Check all that apply.

2A(g) + 2B(g) -->5C(g)

2A(g) +3 B(s) --> 4C(g)

A(s) + 2B(g) --> C(g)

A(s) + B(g) -->2C(g)

Calculate the ∆Hº (on a per mole basis) for the HCl/NaOH neutralization. You may assume that the specific heat and density of the resulting solution to be the same as water. Be sure to use the combined total volumes of HCl and NAOH when calculating the total mass for this reaction. Remember to take into account the moles of limiting reagent when calculating the ∆Hº on a per mole basis.

Exact Concentrations: HCl = .9637 NaOH = 1.016

Trial 1 : temp of HCl = 19 degrees C Temp of NaOH = 19 degrees C constant temp of HCl & NaOH = 24.5 degrees C

Trial 2 : temp of HCl = 20 degrees C Temp of NaOH = 20 degrees C constant temp of HCl & NaOH = 24 degrees C

synthesis of Ethanol by fermentation

(a) Calculate the atom economy and reaction efficiency of your ethanol synthesis. (b) Describe some green features of your synthesis, and any that aren't so green.

In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods: the half-reaction method or the oxidation number method. The half-reaction method balances the electrons lost in the oxidation half-reaction with the electrons gained in the reduction half-reaction. In either method H2O(l), OH?(aq), and H+(aq) may be added to complete the mass balance. Which substances are used depends on the reaction conditions.

Acidic solution

In acidic solution, the nitrate ion can be used to react with a number of metal ions. One such reaction is

NO3?(aq)+Sn2+(aq)?NO2(aq)+Sn4+(aq)

Since this reaction takes place in acidic solution, H2O(l) and H+(aq) will be involved in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:

NO3?(aq)+Sn2+(aq)+     ????NO2(aq)+Sn4+(aq)+     ???

Part A

What are the coefficients of the reactants and products in the balanced equation above? Remember to include H2O(l) and H+(aq) in the appropriate blanks. Your answer should have six terms.

Enter the equation coefficients in order separated by commas (e.g., 2,2,1,4,4,3). Include coefficients of 1, as required, for grading purposes.

Basic solution

Potassium permanganate, KMnO4, is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the reaction conditions used. In basic solution, the following equation represents the reaction of this ion with a solution containing sodium iodide:

MnO4?(aq)+I?(aq)?MnO2(s)+I2(aq)

Since this reaction takes place in basic solution, H2O(l) and OH?(aq) will be shown in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation: MnO4?(aq)+I?(aq)+     ????MnO2(s)+I2(aq)+     ???

Part B

What are the coefficients of the reactants and products in the balanced equation above? Remember to include H2O(l) and OH?(aq) in the blanks where appropriate. Your answer should have six terms.

Enter the equation coefficients in order separated by commas (e.g., 2,2,1,4,4,3). Include coefficients of 1, as required, for grading purposes.

What is the pH of a solution containing 10 g of HCOOH, formic acid dissolved in enough water to make 250 mL of solution?