Question 1

Which of the following molecules has more than one valid Lewis structure (i.e., exhibits resonance)?

Accepted Answer

$$\mathrm{NO_3$^-}$$

Question 2

Which of the following best explains why water ($$\mathrm{H_2O}) $$has a higher boiling point than methane ($$\mathrm{CH_4$}$$)?

Accepted Answer

Water forms hydrogen bonds, which are stronger than the dispersion forces in methane.

Question 3

A sample of gas occupies $$2.50\ \mathrm{L} at$$ $$1.00\ \mathrm{atm}. If $$the pressure is increased to $$2.00\ \mathrm{atm} at $$constant temperature, what is the new volume?

Accepted Answer

$$1.25\ \mathrm{L}$$

Question 4

Which of the following molecules is nonpolar, despite having polar bonds?

Accepted Answer

$$\mathrm{CO_2$}$$

Question 5

A $$10.0\ \mathrm{g}$$ sample of ice at $$0^\circ\mathrm{C}$$ absorbs $$3.34\$$times10^2$$\ \mathrm{J} of $$heat. What mass of ice melts? (Heat of fusion of ice = $$334\ \mathrm{J/g})$$

Accepted Answer

$$1.00\ \mathrm{g}$$

Question 6

Which of the following statements about the Kinetic Molecular Theory is correct?

Accepted Answer

Gas particles are in constant, random motion and collisions are elastic.

Question 7

A $$5.00\ \mathrm{L}$$ sample of gas at $$300\ \mathrm{K}$$ and $$2.00\ \mathrm{atm} is $$heated to $$600\ \mathrm{K} at $$constant pressure. What is the final volume?

Accepted Answer

$$10.0\ \mathrm{L}$$

Question 8

Which of the following molecules can form hydrogen bonds with itself?

Accepted Answer

$$\mathrm{NH_3$}$$

Question 9

A $$0.500\ \mathrm{mol}$$ sample of an ideal gas occupies $$12.0\ \mathrm{L} at$$ $$300\ \mathrm{K}. $$What is the pressure? $$(R = 0.0821\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$1.02\ \mathrm{atm}$$

Question 10

Which of the following best describes the molecular geometry of $$\mathrm{BF_3$}$$ according to VSEPR theory?

Accepted Answer

Trigonal planar

Question 11

A mixture contains $$2.0\ \mathrm{mol} of$$ $$\mathrm{N_2$}$$ and $$3.0\ \mathrm{mol} of$$ $$\mathrm{O_2$} at a $$total pressure of $$5.0\ \mathrm{atm}. $$What is the partial pressure of $$\mathrm{O_2$}$$?

Accepted Answer

$$3.0\ \mathrm{atm}$$

Question 12

Which of the following changes will increase the boiling point of a liquid?

Accepted Answer

Increasing atmospheric pressure

Question 13

A gas is collected over water at $$25^\circ\mathrm{C}$$ and a total pressure of $$760\ \mathrm{mmHg}. $$The vapor pressure of water at this temperature is $$24\ \mathrm{mmHg}. $$What is the partial pressure of the dry gas?

Accepted Answer

$$736\ \mathrm{mmHg}$$

Question 14

Which of the following best describes the relationship between temperature and pressure for a fixed volume of gas (Gay-Lussac's Law)?

Accepted Answer

Pressure is directly proportional to temperature in Kelvin.

Question 15

Which of the following molecules has the highest electronegativity difference between its atoms?

Accepted Answer

$$\mathrm{HCl}$$

Question 16

A $$2.00\ \mathrm{L}$$ sample of gas at $$27^\circ\mathrm{C} is $$cooled to $$0^\circ\mathrm{C} at $$constant pressure. What is the final volume?

Accepted Answer

$$1.82\ \mathrm{L}$$

Question 17

Which of the following is the best explanation for why $$\mathrm{CO_2$} is a $$gas at room temperature while $$\mathrm{H_2O} is a $$liquid?

Accepted Answer

$$\mathrm{CO_2$}$$ has weaker intermolecular forces than $$\mathrm{H_2O}.$$

Question 18

A $$1.00\ \mathrm{mol}$$ sample of gas at $$1.00\ \mathrm{atm}$$ and $$273\ \mathrm{K} is $$compressed to $$0.500\ \mathrm{L}. $$What is the final pressure? $$(R = 0.0821\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$49.2\ \mathrm{atm}$$

Question 19

Which of the following best describes the effect of increasing the number of moles of gas in a fixed volume at constant temperature?

Accepted Answer

The pressure increases.

Question 20

A reaction produces $$4.48\ \mathrm{L} of$$ $$\mathrm{CO_2$}$$ gas at STP. What mass of $$\mathrm{CO_2$} is $$produced? $$(\mathrm{Molar\ mass\ of\ CO_2$} = 44.0\ \mathrm{g/mol})$$

Accepted Answer

$$8.80\ \mathrm{g}$$

Solids, Liquids, and Gases: Structure, Properties, and Gas Laws

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