Practice 10 questions on CHM101 - CHM 101 at University of North Carolina, Chapel Hill. Free AI-generated quiz on uNotes — track your score, retake anytime.
1The atmospheric pressure at a mountain summit is 581 mm Hg. Calculate this pressure in atmospheres (atm).
2A gas sample occupies 900.0 mL at a temperature of 27.0 °C. At what temperature, in Celsius, will the gas occupy a volume of 1220 mL if pressure remains constant?
3According to the Kinetic Molecular Theory of gases, which of the following statements is INCORRECT?
4What mass of sodium nitrate (NaNO₃, FW = 85.0 g/mol) is required to prepare 2.0 liters of a 1.5 M solution?
5A gaseous mixture contains partial pressures of H₂ (0.01887 atm), N₂ (0.3105 atm), and Ar (1.027 atm). What is the mole fraction of Argon in this mixture?
6Which of the following intermolecular forces must be overcome to boil liquid methanol (CH₃OH)?
7In a phase diagram, the point where the solid, liquid, and gas phases coexist in equilibrium is known as the:
8How many grams of CaC₂ (FW = 64.1 g/mol) are needed to produce 20.0 L of C₂H₂ gas at 1.00 atm and 25.0 °C based on the reaction: CaC₂(s) + 2 H₂O(l) → C₂H₂(g) + Ca(OH)₂(s)?
9Calculate the molarity of a solution prepared by dissolving 1.6 g of NaOH (FW = 40.0 g/mol) in enough water to make 125 mL of solution.
10If the volume of a piston containing liquid and vapor in equilibrium is increased (raised) at constant temperature, what happens to achieve a new equilibrium?
