CHEM 06100 Lecture Notes - Lecture 3: Molar Mass, Unified Atomic Mass Unit, Stoichiometry

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tanpanda642

31 Oct 2017

School

Rowan University

Department

Chemical Engineering Biochemistry

Course

CHEM 06100

Professor

Grinias

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Document Summary

Stoichiometry and chemical reactions: stoichiometry- to determine how much mass, moles, and the making of product. The mole (mol) if we take 12 grams of carbon 12 we have 1 mol. An atom: na= 1 x m of na = 22. 99g/ mol (amu) O2= 2 x m of o = 2 x 16. 00 g/mol = 32. 00g/mol (amu) H2o= 2 m of h= 2. 00+ 1 mo= 16. 00=18. 00g/mol. An ion (particle)= ci= 1 x < =35. 45 g/mol. A formula unit nacl= 1 x m of na = 22. 99+1 x m of ci = 35. 45 g/mol = 58. 44g/mol: need a transfer electron and electronegativity to make ion. [ atoms of x in formula] x [ atomic mass of x (amu)] [moles of x in formula]x [ molar mass of x(/mol 0] Mass fraction and the mass of an element. Mass of compound x mass of element in 1 mol of compound.

Related Questions

A matching question the letters and answers mash together when I submit question.

1. Avogrado constant A. formula mass

2. CO2 B. ideal gas law

3. R C. study that relates mass to number of particles

4. 2g of H2 E D. percent yield

5. u E. one molecule or one mole

6. 58.5 u of NACl F. 6.02x1023

7. NaCl G. 0.1 mole

8. 22.4L H. molar mass

9. PV=nRT I. molar volume

10. Ratio of mass of product J. 0.25 mole

obtained to mass expected

11. Stoichiometry K. 8.31 kPa * L/mol * K

12. 24.5g of H2SO4 L. atomic mass unit

13. 2.24L of a gas at STP M. empirical formula

1. Consider the unbalanced equation for the reaction of solid lead with a silver nitrate solution.

_____Pb (s) + ______AgNO3 (ac) â ______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) â _____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) â 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) â 2 AlCl3 (s)

5. Consider the reaction between NiS2 and O2:

2 NiS2 (s) + 5 O2 (g) â 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

18. What is the molarity of a solution prepared by dissolving 7.50 g of nitrate of magnesium, Mg (NO3) 2 in enough water to prepare 25.0 mL of solution?

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.

CHEM 06100 Lecture Notes - Lecture 3: Molar Mass, Unified Atomic Mass Unit, Stoichiometry

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