If i were to get the amount of heat transfer using constant pressure calorimetery, can I get the amount for the constant volume calorimetery using that value? Or vice versa?

A solution contains 0.003Mof sodium phenobarbital together with a buffer consisting of 0.20 M sodium acetate and 0.30 M acetic acid. Acetic acid is a weak electrolyte; its degree, or fraction, of dissociation, α, at this concentration is 0.008 and the undissociated species do not contribute to the ionic strength. What is the ionic strength of the solution?

pka for acetic acid = 4.8

At 85oC, the vapor pressure of pure o-xylene is 55 Torr and the vapor pressure of pure p-xylene is 85 Torr. When liquid o-xylene is mixed with liquid p-xylene, the solution formed is ideal at all compositions.

(a) Calculate ∆G, ∆H, and ∆S of mixing when liquid o-xylene and liquid p-xylene are mixed at 85oC, given that the mole fraction of p-xylene is 0.30 and the solution contains a total of 4.0 mol of material.

(b) What are the mole fractions of o-xylene and p-xylene in the vapor at equilibrium with this solution?

A 115.0 −mL sample of a solution that is 2.6×10⁻³ M in AgNO3 is mixed with a 230.0 −mL sample of a solution that is 0.14 M in NaCN .

After the solution reaches equilibrium, what concentration of Ag+(aq) remains?

Could you give me some tips on how to know how to identify chiral centers in a large molecule?

I know that a chiral center is surrounded by 4 different groups...but I'm finding it a little bit hard to recognize multiple chiral center in large structures.

If the dissolution of KCl (74.55 g/mol) is expected to absorb 17.2 kJ of energy per mole of KCl dissolved, then what is the expected change in temperature (in oC) if 2.11 grams of KCl are dissolved in 10.00 mL of water (density of 1.00 g/mL and specific heat capacity of 4.184 J/g•oC)? (Give answer as the absolute value of the temperature change; do NOT include negative sign if temperature decreases.)

The average human body contains 5.70 L of blood with a Fe2+ concentration of 2.10×10⁻⁵M . If a person ingests 10.0 mL of 25.0 mM NaCN, what percentage of iron(II) in the blood would be sequestered by the cyanide ion?

Express the percentage numerically.

An analytical chemist is titrating 60.3 mL of a 0.5500 M solution of nitrous acid (HNO2) with a 0.6400 M solution of KOH. The pKa of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 22.2 mL of the KOH solution to it. Please round your answer to 2 decimal places

At a temperature other than 25^oC, Cd(OH)₂ solubility is 5.5 x 10^-4 . Calculate it's Ksp at this temperature.

[ACCORDING TO MY TEXT, Ksp of Cd(OH)₂ = 2.5 x 10¹⁴ @ 25 C]

A.1.7 x 10^-10

B.6.7 x 10^-10

C.2.5 x 10^-14

1.   An electrode of solid chromium is immersed in a 1M solution of Cr³⁺; In a second beaker, a tin electrode is immersed in a 1 M solution of Sn²⁺. The two electrodes are connected by a wire through a voltmeter, and the two beakers are connected via a salt bridge. The entire system is maintained at a T = 298K. When the connection is made between the two cells, what is the E^o for the cell, in volts, if the reduction potential for Cr(III) to Cr(0) is -0.74 V and the reduction potential for Sn(II) to Sn(0) is -0.14V? (a) –0.78V (b) 0.78V (c) –0.60V (d) 0.60V (e) none of these

2.   Using the data in the table provided, calculate the approximate standard state Gibbs free energy change at 298 K for the reaction Al₂O_3(s) + 3H_2(g) => 2Al_(s) + 3H₂O_(g)

   (a) 236 (b) 886 (c) –344 (d) –1021 (e) none of these

3. The K_sp for lead (II) fluoride in water is 3.6 x 10^-8. What is its solubility in g/L? (a) 3.3 x 10^-3 (b) 1.3 x 10^-4 (c) 0.051 (d) 2.1 (e) none of these

4. The lower the vapor pressure of a liquid, the (a) higher the boiling point (b) the lower the boiling point (c) the higher the melting point (d) the lower the melting point (e) none of these relationships are true.

5. Elemental phosphorous, which exists as P₄ molecules, has the following solubility properties: Water – insoluble; CCl₄ – soluble. What may be ascertained about the type of intermolecular forces which are operative when P₄ forms solutions? (a) they are ion-dipole in nature (b) they are dipole-dipole in nature (c) they are London force in nature (d) they are ionic in nature (e) they are covalent in nature

6. What is the order of the reaction in NO? (a) -1 (b) 0 (c) 1 (d) 2 (e) none of these

7. What is the order of the reaction in H₂? (a) -1 (b) 0 (c) 1 (d) 2 (e) none of these

Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO and 0.135 M H2O. What is the equilibrium concentration of [CO], [H2O], [CO2], and [H2]

compare the values of the enthalpy of neutralization for the three acids( H3CCOH, Na2S2O3, HCl). explain any similarities and/or differences

Find the pH of a 0.14M CH3COOH solution. Ka= 1.8x 10^-5

Fill in the blanks using (fatty acids, glycerol, sphingolipids, steriods, glycolipids, glycerophospholipid, triacylglycerols.)

Compounds that contain a fused ring system are called __________. These have three 6-membered rings and one 5-membered ring. Some of these compounds are found in biological membranes. _________ are the building blocks for many lipids, and they generally contain an even number of carbon atoms and an unbranched hydrocarbon chain. ________ are formed when a carbohydrate is glycosidically linked to a hydroxyl group of a lipid. Examples include gangliosides and cerebrosides. These are found in biological membranes. ________ are the storage form of lipids, accumulating in adipose tissue, and they can be used as metabolic fuel. These compounds have a polar part, made of three ester groups, and a nonpolar fatty acid tail. They behave as all nonpolar. ________ are made up of a long-chain amino alcohol joined, either by a glycosidic linkage and a phosphodiester linkage, to a fatty acid. These do not contain ______. They are abundant in the nervous system. When glycerol is esterfied to two fatty acids and a phosphoric acid molecule a _____ is formed. These are found in biological membranes.

Hydrogen and chlorine gas are placed in a 10.0 L container and allowed to react. The initial density of the mixture is 5.01 x10-3 gm/ml. The vessel is at 300K and the initial pressure is 6.52 atm. After the reaction is complete , the pressure is 6.52 atm. The gas is bubbled into 1.00 liter of deionized water. In another part of the universe, a grey haired chemistry instructor prepares an acetic acid/ acetate buffer. The buffer was prepared by adding acetic acid and sodium acetate to 2.50 L of deionized water. Now, as universes collide, our hero adds 107 ml of the HCl solution to 405 ml of the buffer. The pH is measured and is 4.35 after the HCl addition. A drop of phenolphthalein is added and the solution is titrated to equivalence with 657 ml of 0.920 M NaOH. Calculate the original molarities of the weak acid and conjugate base in the 2.50 L solution?