Question1. In the area of nano-chemistry, particles defined as nanoparticles r

1. In the area of nano-chemistry, particles defined as nanoparticles range in size from 1-2500 nm. 1 nm is equivalent to 1 × 10–9 m. A wavelength of red light is measured at 655 nm. What is this measurement in centimeters?

 

 

 

a.

 

6.55 cm

 

 

 

b.

 

0.00655 cm

 

 

 

c.

 

6.55 x 10−5 cm

 

 

 

d.

 

6.55 x 10−7 cm

 

 

 

e.

 

6.55 x 10−9 cm

 

2. The liquid 1,2-ethanedithiol is insoluble in water. If a 75.5-g sample of 1,2-ethanedithiol has a volume of 61.2 mL, what is its density, and would it float or sink if poured into a beaker containing water?

 

 

 

a.

 

1.23 g/mL and it would sink in water

 

 

 

b.

 

1.23 g/mL and it would float on water

 

 

 

c.

 

0.811 g/mL and it would sink in water

 

 

 

d.

 

0.811 g/mL and it would float on water

 

3. A general chemistry student found a chunk of metal in the basement of a friend’s house. She measured the mass of the metal to be 238.7 g. Then she dropped the metal into a graduated cylinder containing 35.0 mL of water, and the water level rose to 47.3mL. Of the following metals, which one did she use?

 

 

 

a.

 

Aluminum, d = 2.72 g/mL

 

 

 

b.

 

Silver, d = 10.50 g/mL

 

 

 

c.

 

Lead, d = 11.34 g/mL

 

 

 

d.

 

Tungsten, d = 19.38 g/mL

 

 

 

e.

 

Platinum, d = 21.46 g/mL

 

4. An empty Erlenmeyer flask weighs 241.3 g. When filled with water (density = 0.997 g/mL), the flask and its contents weigh 489.1 g. What volume of water does the flask hold?

 

 

 

a.

 

246. mL

 

 

 

b.

 

247. mL

 

 

 

c.

 

248. mL

 

 

 

d.

 

249. mL

 

 

 

e.

 

241. mL

 

5. What is the correct answer to the expression below?

 

=

 

 

 

a.

 

8.63 cm

 

 

 

b.

 

8.6369 cm

 

 

 

c.

 

8.6 cm

 

 

 

d.

 

8.636 cm

 

 

 

e.

 

8 cm

 

6. The specific heat of ice is 0.492 cal/(g × °C). How many calories of heat are required to raise 100.0 g of ice from -20.0 °C to -0.5 °C?

 

a. 2.52 cal

 

b. 10.4 cal

 

c. 49.2 cal

 

d. 959 cal

 

e. 3960 cal

 

7. An Indy race car can travel 111 m/s. What is the speed of the car in miles per hour? (Given: 1 mi = 1.61 km, and 1 h = 3600 s)

 

a. 111 mi/h

 

b. 178 mi/h

 

c. 248 mi/h

 

d. 400 mi/h

 

e. 643 mi/h

 

8. Calculate the length of a copper wire having a diameter of 0.200 cm and a mass of 15.620 g. The density of copper is 8.92 g/cm3. (Given: volume = πd2 L/4, where π = 3.14, d = diameter, and L = length)

 

a. 1.80 × 10-4 cm

 

b. 4.00 × 10-4 cm

 

c. 5.50 × 10-2 cm

 

d. 1.75 cm

 

e. 55.8 cm

 

9. At which of the following temperatures is it most economical to fill a gas tank?

 

a. 50 °C

 

b. 40 °C

 

c. 30 °C

 

d. 20 °C

 

e. 10 °C

 

10. Element Y has two natural isotopes: Y-63 (62.940 amu) and Y-65 (64.928 amu). Calculate the atomic mass of element Y given the abundance of Y-63 is 69.17%.

 

a. 63.55 amu

 

b. 64.00 amu

 

c. 64.32 amu

 

d. 107.85 amu

 

e. 108.46 amu

 

11. For the following reaction, 4.57 g of silver nitrate (Molar Mass = 169.88 g/mol) are mixed with excess copper. The reaction yields 2.29 g of copper(II) nitrate (Molar Mass = 187.57 g/mol). What is the percent yield for this reaction?

 

2 AgNO3(aq) + Cu(s) ? Cu(NO3)2 (aq) + 2 Ag(s)

 

 

 

a.

 

45.3%

 

 

 

b.

 

50.1%

 

 

 

c.

 

67.8%

 

 

 

d.

 

73.8%

 

 

 

e.

 

90.9%

 

12. How many grams of nickel are present in 3.89 g of nickel(II) iodide?

 

 

 

a.

 

0.138 g Ni

 

 

 

b.

 

0.731 g Ni

 

 

 

c.

 

1.23 g Ni

 

 

 

d.

 

1.30 g Ni

 

 

 

e.

 

2.07 g Ni

 

13. How many grams of silver will be formed when 27.9 g of copper reacts with

 

excess silver nitrate, according to the balanced equation below?

 

2AgNO3 + Cu ? Cu(NO3)2 + 2Ag

 

 

 

a.

 

8.22 g

 

 

 

b.

 

23.7 g

 

 

 

c.

 

32.9 g

 

 

 

d.

 

47.4 g

 

 

 

e.

 

94.7 g

 

14. What is the maximum amount of carbon dioxide which can be formed if 15.2 g of glucose, C6H12O6 (molar mass = 180.18 g/mol) is allowed to react with 22.5 g of oxygen, O2?

 

C6H12O6 + 6O2 ? 6CO2 + 6H2O

 

 

 

a.

 

19.2 g

 

 

 

b.

 

20.6 g

 

 

 

c.

 

22.3 g

 

 

 

d.

 

26.4 g

 

 

 

e.

 

30.9 g

 

15. 61.8 g of potassium hydroxide is allowed to react with 33.8 g of phosphoric acid, according to the following reaction:

 

3 KOH(aq) + H3PO4(aq) ? K3PO4(aq) + 3 H2O(l)

 

What is the theoretical yield of potassium phosphate for this reaction?

 

 

 

a.

 

15.6 g

 

 

 

b.

 

16.3 g

 

 

 

c.

 

73.2 g

 

 

 

d.

 

77.9 g

 

 

 

e.

 

233.8 g

 

16. An oxide of nitrogen contains 74.1% oxygen and has a molar mass of 108 g/mol. What is the molecular formula for this compound?

 

 

 

a.

 

N2O5

 

 

 

b.

 

N2O3

 

 

 

c.

 

N2O4

 

 

 

d.

 

N2O0

 

 

 

e.

 

N2O2

 

17. Butyric acid, found in rancid butter, has a molar mass of 88 g/mol. If butyric acid is 54.5% C, 9.09% H and 36.4% O, what is the molecular formula?

 

 

 

a.

 

C4H8O2

 

 

 

b.

 

C8H12O4

 

 

 

c.

 

C2H4O

 

 

 

d.

 

C12H6O

 

 

 

e.

 

CHO2

 

18. When 2.34 g of pure iron is allowed to react with an excess of oxygen, 3.35 g of the final compound is produced. Determine the formula of the compound.

 

 

 

a.

 

Fe2O3

 

 

 

b.

 

FeO2

 

 

 

c.

 

FeO4

 

 

 

d.

 

FeO3

 

 

 

e.

 

FeO

 

19. You need to make an aqueous solution of 0.139 M aluminum nitrate, Al(NO3)3, for an experiment in the lab, using a 300. mL volumetric flask. How much solid aluminum nitrate (Molar Mass = 213.012 g/mol) should you add?

 

 

 

a.

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