Ideal gas law
28.1 g sample of Xe is in a 552.4 mL container. What is the pressure of this gas in kilopascals at 1087.2 K?
3500 kPa
What is the defenition of a limiting reactant in a chemical reaction?
The limiting reactant is the substance that is completely consumed first, limiting the amount of product formed in a chemical reaction.
What type of classification best characterizes the following reaction?
2HBr (g) → H2 (g) + Br2 (g)
A) combination reaction
B) combustion reaction
C) decomposition reaction
D) single replacement reaction
E) none of the above
C) Decomposition
MATCH
A) Boyle's Law
B) Charles' Law
C) Avogadro's Law
1. The volume of a gas is directly proportional to its temperature when pressure and the number of gas particles are constant.
Answer: B) Charles' Law
2. The volume of a gas is inversely proportional to its pressure when temperature and the number of gas particles are constant.
Answer: A) Boyle's Law
3. The volume of a gas is directly proportional to the number of moles of gas when pressure and temperature are constant.
Answer: C) Avogadro's Law
NaCl can be classified as a ________.
A) gas
B) liquid
C) weak electrolyte
D) strong electrolyte
E) nonelectrolyte
D) nonelectrolyte
1.889 × 1023 particles sample of I2 is in a 8862.4 mL container. What is the pressure of this gas in atmospheres at 817.2 °C?
3.168 atm
In a reaction between 2 moles of hydrogen gas (H₂) and 1 mole of oxygen gas (O₂) to form water (H₂O), which reactant is limiting if you have 3 moles of H₂ and 1 mole of O₂?
Oxygen (O₂) is the limiting reactant because it will be completely consumed first, leaving excess hydrogen (H₂).
A gas mixture contains O2 and Ne. If O2 has a partial pressure of 766 torr and Ne has a partial pressure of 0.88 atm, what is the total pressure of this mixture in atm?
A) 767 atm
B) 563 atm
C) 1.00 atm
D) 1.48 atm
E) 1.89 atm
E) 1.89 atm
Which of the following is not a property predicted based on the Kinetic Molecular Theory?
A) It explains the low density of gases in comparison to solids and liquids.
B) It predicts a gasʹs tendency to assume the shape and volume of the container.
C) It explains why gases are compressible.
D) It predicts a gasʹs tendency to have high melting and boiling points.
E) It explains how the molecules slow down as temperature is decreased.
It predicts a gasʹs tendency to have high melting and boiling points.
Methanol, CH3OH, can be classified as a ________.
A) gas
B) solid
C) weak electrolyte
D) strong electrolyte
E) nonelectrolyte
E) nonelectrolyte
7.77 g of ClF3 is held at 0.647 atm and 925.9 °C. What is the volume of its container in milliliters?
128,000 mL ClF3
How do you calculate the limiting reactant in a reaction involving two reactants?
To calculate the limiting reactant, convert the moles of each reactant to moles of product using stoichiometric ratios. The reactant that produces the least amount of product is the limiting reactant.
Which of the statements below best describes Ni (s) in the following reaction?
Ni (s) → Ni2+ (aq) + 2e-
A) Ni (s) is oxidized
B) Ni (s) is neither oxidized nor reduced
C) Ni (s) is both oxidized and reduced
D) Ni (s) is reduced
A) Ni (s) is oxidized
If the pressure of a constant amount of gas at constant temperature is increased by threefold, what happens to its volume?
A) The volume increases by six-fold.
B) The volume will not change.
C) The volume triples.
D) The volume increases by nine-fold.
E) The volume is one-third of the original volume.
E) The volume is one-third of the original volume.
The solubility of KI is 50 g in 100 g of H2O at 20 °C. If 110 grams of KI are added to 200 grams of H2O,
A) all of the KI will dissolve.
B) the solution will freeze.
C) the solution will start boiling.
D) a saturated solution will form.
E) the solution will be unsaturated.
D) a saturated solution will form.
44.39 g of AsH3 is held at 384.25 kPa and 608 °C. What is the volume of its container in milliliters?
10,900 mL AsH3
In a reaction where 4.0 moles of nitrogen (N₂) react with 12.0 moles of hydrogen (H₂) to form ammonia (NH₃), how do you determine which reactant is limiting and how many moles of NH₃ will be produced?
To determine the limiting reactant, use the balanced chemical equation:
N₂ + 3H₂ → 2NH₃
What volume (mL) of a 10.5 M solution of sodium hydorxide (NaOH) must be diluted to
prepare a 200. mL solution of 1.75 M sodium hydroxide ?
A) 101 mL
B) 1200 mL
C) 33.3 mL
D) 56.9 mL
E) 0.0919 mL
C) 33.3 mL
A quantity of Ne gas that was originally held at 3.80 atm pressure in a 1.00 L container at 26.0
°C is transferred to a 10.0 L container at 20.0 °C. What is the pressure (in atm) of Ne in the
new container ?
A) 0.372 atm
B) 3.80 atm
C) 1.35 atm
D) 0.292 atm
E) 5.56 atm
A) 0.372 atm
Which compound below becomes a strong electrolyte when dissolved in water?
A) C12H22O11 (sucrose)
B) SCl6
C) CH3CH2OH
D) KOH
E) Cl2
D) KOH
The pressure of a 46.7 g sample of ClF5 in a 28.45 L container is measured to be 5.18 atm. What is the temperature of this gas in kelvins?
5,020 K
Provide a real-life application of the limiting reactant concept in industrial chemistry.
In the production of ammonia through the Haber process, nitrogen and hydrogen are reacted together. To optimize efficiency and minimize waste, the limiting reactant must be carefully managed to ensure that the maximum amount of ammonia is produced with minimal leftover reactants, thereby saving both resources and costs.
According to the reaction given below, how many grams of solid Fe(OH)2 is formed when 175 mL of 2.27 M aqueous LiOH reacts with excess aqueous FeCl2? (Note: Molar Mass of Fe(OH)2 is 89.859 g/mol)
FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq)
A) 34.7 g
B) 35.7 g
C) 17.8 g
D) 51.0 g
E) 25.5 g
C) 17.8 g
gas exerts a pressure of 685 mmHg and has a temperature of 245 K. What is the new
pressure of this gas, in mmHg, if the temperature is increased to 655 K? Volume and the
amount of the gas stay constant.
A) 933 mmHg
B) 556 mmHg
C) 256 mmHg
D) 1830 mmHg
E) 442 mmHg
D) 1830 mmHg
Which pair of compounds will form a solution?
A) Na2SO4 and benzene (C6H6)
B) H2O and CCl4
C) Benzene (C6H6) and hexane (C6H14)
D) NaCl and hexane (C6H14)
E) More than one of the combinations will form solutions.
C) Benzene (C₆H₆) and hexane (C₆H₁₄)