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Chem exam 1

front 1

1. A molecule is found to contain 47.35% by mass C, 10.60% by mass H, and 42.05% by mass O. What is the empirical formula for this molecule?

back 1

C3H8O2

front 2

2.Which element is most likely to form a 2– ion?

K, S, Mg, P, Br

back 2

S

front 3

3. You have 6.23 moles of each of the following elements: Li, Ca, Fe, S and Cu. Which sample contains the largest mass in grams?

back 3

Cu

front 4

4. How many hydrogen atoms are present in 1.89 g of NH3?

back 4

2.00E+23

front 5

5. How many protons, neutrons, and electrons are in a silver atom with a mass number of 108?

back 5

47 P

61 N

47 E

front 6

6. Which one of the following substances is classified as an element?

C6H12O6, I2, NO, CO, KCl

back 6

I2

front 7

7. The density of ice at 0 °C is 0.917 g/mL. What is the volume of 322 g of ice?

back 7

351mL

front 8

8. What is the percent yield if 15.5 g SF6 is isolated from the reaction of 14.5 g S8 and 58.6 g F2?

S8(s) + 24 F2(g) → 8 SF6(g)

back 8

23.5%

front 9

9. Which of the following observations is/are examples of chemical change?
1.Iron (Fe) rusts, forming Fe2O3.

2.The density of water increases when it changes from a solid to a liquid.

3.Sodium chloride melts at 801 °C

back 9

1 only

front 10

10. Two electronic balances are tested using a standard weight. The true mass of the standard is 5.0000 g. The results of 5 individual measurements on each balance are recorded below.

A: 5.2895, 5.1077, 4.6407, 4.8947, 5.0672

B: 5.0001, 4.9998, 4.9999, 5.0002, 4.9999
Which statement best describes the results?

back 10

A: poor precision and good accuracy

B: good precision and accuracy

front 11

11. How many protons, neutrons and electrons are present in one ion of 31P3–?

back 11

protons = 15, neutrons = 16, electrons = 18

front 12

12. How many moles of sodium bromide can be produced from the reaction of 5.82 moles of sodium with 3.04 moles of bromine gas?

2 Na(s) + Br2(g) → 2 NaBr(s)

back 12

5.82 mol

front 13

13. Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas.

2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g)

What mass of H2(g) is produced from the reaction of 0.743 g Al(s) with excess hydrochloric acid?

back 13

8.34E-2 g

front 14

14. Which of the following compounds are named correctly?

1. BaI2, barium(I) iodide
2. CoO, cobalt(II) oxide
3. FeBr3, iron(II) bromide

back 14

2 only

front 15

15. Write the balanced chemical equation for the reaction below and indicate the smallest whole number coefficient for each substance.

__iron(III) carbonate(s) + __hydrochloric acid(aq) __iron(III) chloride + __H2O(l) + __CO2(g)

back 15

1 6 2 3 3

front 16

16. Calculate the number of moles of aluminum oxide in 8.25 g Al2O3.

back 16

8.09E-2 mol

front 17

17. Rubidium has two naturally occurring isotopes. The average mass of Rb is 85.4678 u. If 72.15% of Rb is found as Rb-85 (84.9117 u), what is the mass of the other isotope?

back 17

86.91u

front 18

18. Which of the following is the smallest mass?

2.12e-5g

1.74e+7ng

2.52e+9pg

0.154mg

2.71e+6ng

back 18

2.12e-5g

front 19

19. Round 0.00763521 to 3 significant figures.

back 19

0.00764

front 20

20. Which of the following compounds are named correctly?

1. NO2, nitrogen oxide
2. PCl5, phosphorous pentachloride
3. NH4I, ammonium monoiodide

back 20

2 & 3

front 21

21. What is the correct answer to the following expression: (201.83 – 146.00) ÷ 7.109?

back 21

7.853

front 22

22. Identify the ions present in Na2SO4.

back 22

Na+ and SO4 2–

front 23

23. Which two of the atoms below have the same number of neutrons?
(mass/atomic number)

S34/16

S32/16

Cl35/17

Ar38/18

back 23

S34/16 and Cl35/17

front 24

24. What is the percent by weight of hydrogen in propane, C3H8?

back 24

18.32

front 25

25. How many grams of fluorine are present in 3.56 moles of boron trifluoride?

back 25

203