Question 1

The speed of light is $$3.0 	imes 10^8$ m/s. What is this speed in nm/ms?

Accepted Answer

$$3.0 	imes 10$$^{14}$$ nm/ms

Question 2

A palladium nanoparticle has a density of $$12.0 g/cm$^3. $$What is the mass of a nanoparticle with a volume of $$1.84 	imes 10$$^{-21}$$ cm^3$?

Accepted Answer

$$2.21 	imes 10$$^{-20}$$ g

Question 3

Which of the following compounds contains a +1 ion?

Accepted Answer

KCl

Question 4

What is the energy of a photon with a wavelength of $$656 nm$$? (Use $$h = 6.62 	imes 10$$^{-34}$$ J·s, c = 2.998$$ 	imes $$10^8 m/s)$$

Accepted Answer

$$3.03 	imes 10$$^{-19}$$ J

Question 5

Which set of quantum numbers is correct and consistent with $$n=4$$?

Accepted Answer

$$l=3$$, $$m_l=-3$$, $$m_s=+\frac{1}{2}$$

Question 6

Which of these atoms will be the smallest?

Accepted Answer

P ($$Z=15)$$

Question 7

A single molecule of a certain compound has a mass of $$3.4 	imes 10$$^{-22}$$ g. Which value comes closest to the mass of a mole of this compound?

Accepted Answer

200 g/mol

Question 8

A 10 gram sample of which substance contains the greatest number of hydrogen atoms?

Accepted Answer

10 grams of H$$_2$$

Question 9

What is the mass percent of oxygen in $$\mathrm{Fe_2$(SO_4$)_3}$$? (Molar mass: Fe = 55.85 g/mol, S = 32.07 g/mol, O = 16.00 g/mol)

Accepted Answer

48.01%

Question 10

How many moles of $$\mathrm{Ba_3N_2}$$ are necessary to react completely with $$1.5$$ mol of water? $$\mathrm{Ba_3N_2} + 6 \mathrm{H_2O} \rightarrow 3 \mathrm{Ba(OH)_2} + 2 \mathrm{NH_3$}$$

Accepted Answer

0.25 mol

Question 11

What is the percent yield when $$1.72 g of$$ $$\mathrm{H_2O_2}$$ decomposes and produces $$375 mL of$$ $$\mathrm{O_2$}$$ gas measured at $$42^\circC $$and $$1.52$$ atm? (Molar mass of $$\mathrm{H_2O_2} is$$ $$34.02 g/$$mol, $$R = 0.0821 L$$·atm·mol$$^{-1}$$·K$$^{-1})$$

Accepted Answer

87.2%

Question 12

If a system's internal energy increases by $$250 kJ $$after the addition of $$375 kJ of $$energy as heat, what was the value of the work in the process?

Accepted Answer

$$-125 kJ$$

Question 13

Calculate the enthalpy of combustion of ethylene, $$\mathrm{C_2H_4}$$, at $$25^\circC $$and one atmosphere of pressure. $$\mathrm{C_2H_4(g) + 3 O_2$(g) \rightarrow 2 CO_2$(g) + 2 H_2O(l)} ($$Use $$\Delta H_f^\circ$$ values: $$\mathrm{C_2H_4(g)} = 52.3 kJ/$$mol, $$\mathrm{CO_2$(g)} = -393.5 kJ/$$mol, $$\mathrm{H_2O(l)} = -285.8 kJ/$$mol)

Accepted Answer

$$-1411 kJ/$$mol

Question 14

Which molecule contains carbon with a negative formal charge?

Accepted Answer

CO

Question 15

A 14.0 g sample of $$\mathrm{N_2$} (g) $$occupies what volume at $$0^\circC $$and $$1.00$$ atm? (Molar mass $$\mathrm{N_2$} = 28.0 g/$$mol, $$R = 0.0821 L$$·atm·mol$$^{-1}$$·K$$^{-1})$$

Accepted Answer

11.2 L

Question 16

According to kinetic-molecular theory, why does pressure increase as the temperature of an ideal gas increases?

Accepted Answer

Both I and II

Question 17

Why is the boiling point of $$\mathrm{Br_2$}$$ higher than that of $$\mathrm{Cl_2$}$$?

Accepted Answer

$$\mathrm{Br_2$} is $$more polarizable and therefore has greater London dispersion forces.

Question 18

Which substance has the lowest boiling point?

Accepted Answer

CH$$_4$$

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