chem hw

Name:__________________________________________ Points:+___/10

Extra Credit Assignment: Due 07/07/2022 by 11:59:00pm

1. Place your final answers on a on this sheet of paper.

2. Attach ALL your work for every problem on a separate sheet of paper (handwritten).

3. There should be a page just for your answers (this page), and a page just for your work. Please separate them for easy grading.

4. Submit your answers and the work together by the due date above in the designated blackboard link.

5. I am not a resource to use to help with this assignment.

Late submissions will not be accepted.

1. Change the following numbers from scientific notation to regular notation.

a) 6.022 x 1013 _____________ b) 3.1494 x 104 _____________ f) 1.131 x 108 _____________ g) 6.87 x 10-10 _____________ h) 3.978 x 10-4 _____________

2.

3. Express the following numbers in scientific notation, making sure there is only one nonzero digit to the left of the decimal place. Do not discard any nonzero digits.

a) 33700000 _____________ b) 0.006110 _____________ f) 410.00 _____________ g) 41007 _____________ h) 0.0000033201 _____________

4.

5. For each of the following quantities, underline the zeroes that are significant figures.

a) 13300.0120 c) 0.041120 d) 700120000

6. Give the number of significant figures in the following numbers:

a) 4.301x105 ____ b) 6.33x10-7 ____ e) 5400.00 ____ f) 0.000041 ____

7.

8. Round off the following numbers using five significant figures in your answer.

a) 306719 ___________ b) 607378 ___________ c) 807999 ___________

9. Perform the following operations and give the answers with the correct number of significant figures and include units on your answers.

a) 83.197g - 41.8g = ___________ c) = ___________

PART C. DIMENSION ANALYSIS

10. Complete the following conversions:

307.7 ft = ________________m

4.08 pints =_________________ L

8.83 km = _________________ yds

784.11 m = _________________in

11. A small crystal has a mass of 7.03 mg and is shaped like a cylinder with a height of 5.17 in and a radius of 34.8 mm. What is the density of the solid in g/cm3?

12. If the price of gasoline is $2.03 dollars/gal, what is its price in Euros per liter, given the exchange rate is $1.20 per Euro.

13. Convert 316.25 K into oC. Convert 14.7 oC into oF.

14. Provide the names for the following compounds

15.

a. NaF

b. N2O4

c. KNO3

d. MgSO4

e. NH3

f. Cr(NO2)

16. Provide formulas for the following compounds

a.

b. Calcium iodide

c. Aluminum sulfide

d. Lithium carbonate

e. Lead (II) oxide

f. Manganese (II) dichromate

17. Name These Acids:

a. H2S b. HF c. H2CO3 d. HNO2

18. Write formulas for the following acids:

a. Hydroiodic acid b. Hydrophosphoric acid c. Nitric acid d. Chromic acid

19. How many neon atoms are there in 2.585 mol of neon?

20. What is the mass in grams of 0.2338 mol of Titanium?

21. How many moles of barium are there in 42.9g of barium?

22. Molar mass of Copper (II) Nitrate = ___________________g/mole

23. Balancing Equations

a) ____ Na3PO4 + ____ Ba(OH)2 ____ NaOH + ____ Ba3(PO4)2 b) ____ CaF2 + ____ Li2CO3 ____ CaCO3 + ____ LiF c) ____ Ba3N2 + ____ PtF2 ____ BaF2 + ____ Pt3N2

24. Write chemical equations for the following reactions. a) Rubidium reacts with bromine to form Rubidium bromide.

b) Iron (II) sulfide and water vapor are formed when hydrogen sulfide and iron (II) hydroxide react. c) Calcium reacts violently with water to produce calcium hydroxide and hydrogen.

25. Stoichiometry

a) If 2.98 moles of C are reacted with an excess of Cu2O, what mass of CO would be produced?

b) If 43.6 g of Co(NO3)3 are reacted with an excess of (NH4)2S, how many moles of NH4NO3 would be produced?

c) If 19.6g of FeS is added to 44.8g of HCl and allowed to react, what is the theoretical yield of H2S? If 6.20 g of H2S were obtained in the lab, what is the percent yield?

d) 0.947 g of chromium (III) chloride combined with 1.13 g of copper (II) sulfate to produce 0.154 g of copper (II) chloride. What is the percent yield of this reaction?

26. Solutions and Solubility

Label the following compounds as soluble or insoluble in water:

a)

b) NaCl

c) CaSO4

d) AgNO3

e) PbCl2

f) Li2S

g) MgCO3

27. Calculate the molar concentration, M, of a solution of a sample with 0.271 moles in 55.0 L or solution.

28. Calculate the pH of a 0.543M HCl solution.

29. Write the net ionic equations for the following reactions. Be sure to show all physical states for reactants and products for each equation type:

1. ___KBr + ___Pb(NO3)2 ___PbBr2 + ___KNO3

1. ___Fe(C2H3O2)2 + ___Li2SO4 ___FeSO4 + ___LiC2H3O2