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13 Dec 2019

1: A 30.66 gram sample of glycerin, C3H8O3 was dissolved in 323grams of water. Calculate the boiling and freezing points of thesolution


2: A solution is prepared by dissolving 5.00 mg of apolysaccharide (a polymer made of sugar molecules) in enough waterto give a final volume of 1.00 mL of solution. The osmotic pressureis measured and found to be 1.91E-3 atm at 25 degrees C. Calculatethe molar mass of the polysaccharide.

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Nelly Stracke
Nelly StrackeLv2
17 Dec 2019

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Related questions

Need help with number three

1.) Indicate which aqueous solution has the lowest vapor pressure:

a. 0.2 M MgCl2 b. 0.1 M MgCl2 c. 0.2 M NaCl d. 0.1 M KCl e. 0.1 M Na2CO3

2.) Indicate which aqueous solution has the fastest evaporation rate.

a. 0.2 M MgCl2 b. 0.1 M MgCl2 c. 0.2 M NaCl d. 0.1 M KCl e. 0.1 M Na2CO3

3.) What is the molarity of a sucrose (C12H22O11) solution that produces an osmotic pressure of 2.65 atm at 25°C?

a. 0.0349 M b. 0.108 M c. 0.127 M d. 0.398 M e. 0.0127 M

4.) The pressure of carbon dioxide in a beer bottle is about 2 atm. At this pressure about 0.15 g of carbon dioxide dissolves in 100 mL of beer. How much carbon dioxide remains dissolved in 100 mL after the bottle is opened? The partial pressure of carbon dioxide is 2.0 ´ 10-4 atm. a. 3.8 ´ 10-3 g b. 0.15 g c. 6.0 ´ 10-5 g d. 1.5 ´ 10-5 g e. 3.0 ´ 10-4 g

5.) Caryophyllene, a nonelectrolyte, is one of the compounds responsible for the flavor of cloves. A 207 mg sample of caryophyllene was dissolved in 1.00 g of chloroform (Kb = 3.63°C/m), increasing the boiling point of chloroform by 3.68°C. What is the molar mass of caryophyllene? a. 164 g/mol b. 219 g/mol c. 193 g/mol d. 204 g/mol e. 156 g/mol

6.) Which of the following would be most effective in melting ice on a sidewalk?

a. 1 kg KCl b. 1 kg CaCl2 c. 1 kg NaCl d. 1 kg MgCl2 e. 1 kg CuCl

7.) Given the same number of moles of each of the following substances, which one would be most effective in melting ice on a sidewalk?

a. KCl b. CaCl2 c. MgCl2 d. (NH4)3PO4 e. NaCl

8.) If water contains about 42 mg of oxygen per liter at 20°C and 1.0 atm, what would be the value of Henry's law constant for oxygen dissolving in water? The mole fraction of oxygen in air is 0.21.

a. 1.9 ´ 10-2 mol/(L atm) b. 6.3 ´ 10-3 mol/(L atm) c. 0.25 mol/(L atm) d. 0.010 mol/(L atm) e. 1.3 ´ 10-3 mol/(L atm)

9.) What is the molarity of a solution of 10% by mass cadmium sulfate, CdSO4 (molar mass = 208.46 g/mol) by mass? The density of the solution is 1.10 g/mL. a. 0.048 M b. 0.528 M c. 0.479 M d. 0.436 M e. 22.9 M

10.) Determine the molal concentration of a sugar solution in water that has a freezing point of -2.1°C. Kf = 1.86°C/m for water.

a. -1.13 m b. -3.91 m c. 1.13 m d. 0.113 m e. 3.91 m

11.) Eugenol is a nonelectrolyte that contributes to the flavor of spices such as clove, nutmeg, cinnamon, and basil. A 328 mg sample of eugenol was dissolved in 10.0 g of chloroform
(Kb = 3.63°C/m), increasing the boiling point of the chloroform by 0.726°C. What is the molar
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1. Consider the unbalanced equation for the reaction of solid lead with a silver nitrate solution.

_____Pb (s) + ______AgNO3 (ac) → ______Pb(NO3)2 (ac) + _______Ag (s)

a. Balance the equation.

b. How many moles of silver nitrate are required to react completely with 9.3 mol of lead?

c. How many moles of silver, Ag, are formed by the complete reaction of 28.4 mol of Pb?

2. For the following reaction: _____CaO (s) + _____CO2 (g) → _____CaCO3 (s), Calculate how many grams of CaCO3, are formed when 2.4 g of CaO Do they react completely with CO2?

3. For the following reaction: 2 Li (s) + F2 (g) → 2 LiF (s), find the reagent limiting with the amounts of 1.0 mol of Li and 1.0 mol of F2.

4. For the next reaction, determine the limiting reagent, calculate the yield Theoretical product in grams with 5.5 g of Al and 19.8 g of Cl2.

2 Al (s) + 3 Cl2 (g) → 2 AlCl3 (s)

5. Consider the reaction between NiS2 and O2:

2 NiS2 (s) + 5 O2 (g) → 2 NiO (s) + 4 SO2 (g)

When 11.2 g of NiS2 react with 5.43 g of O2, 4.86 g of NiO are obtained. Determine the limiting reagent, the theoretical yield of NiO and the% yield for the reaction.

6. How many atoms of mercury are in 5.8 mol of mercury?

7. Complete the following table:

Element Moles Mass Number of molecules

8. How many grams of sodium are there in 1.00 g of each of the following compounds?

a. Na3PO4

b. NaC7H5O2

c. Na2C6H6O7

9. A sample of 4.78 g of aluminum reacts completely with oxygen to form 6.67 g of aluminum oxide. Use the data to calculate the percent of composition by mass.

10. Citric acid, the compound responsible for the bitter taste in lemons, has the following composition: C - 37.51%

H - 4.40%

O - 58.29%

Calculate the empirical formula.

11. A compound containing phosphorus and oxygen has a molar mass of 219.9 g / mol and an empirical formula of P2O3. Find the molecular formula of compound.

12. It is a term used in chemistry, to describe a system in which a

or more substances, are mixed or dissolved homogeneously in another

substance.

a. Mixture

b. Solution

c. Compound

d. None of the above

13. It is the component that is in a solution, in smaller quantity.

a. Solution

b. Solvent

c. Solvent

d. Soluto

14. It is the component that is in a solution in greater quantity.

a. Solution

b. Solvent

c. Solvent

d. The answers b and c are correct.

15. The quantitative expression of the dissolved amount of solute in a quantity determined solvent is known as:

a. Solution

b. Volume

c. Concentration

d. Stoichiometry

16.Express the moles of solute among the liters of solution

a. Molality

b. Molarity

c. % weight by volume

d. % weight by weight

17.Express the moles of solute between kg of solvent

a. Molarity

b. ppm

c. ppt

d. Molality

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a. 10.3 M

b. 5.6 M

c. 6.5 M

d. 2.03 M

19. How many grams of sodium chloride, NaCl are needed to prepare 125 mL of 0.037 M NaCl solution

a. 1.021 M

b. 0.268 M

c. 0.201 M

d. 0.500 M

20. Calculate the molality of a solution containing 12.5 g of ethylene glycol (C2H6O2) dissolved in 135 g of water.

21. A solution of ethylene glycol contains 21.2 g of ethylene glycol (C2H6O2) in 85.4 mL of water. Calculate the freezing point and the boiling point of the solution. (Assume the water density is 1.00 g / mL)

22. At what volume should you dilute 75 mL of a 10.0 M solution of H2SO4 to obtain a 1.75 M solution of H2SO4.

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