What acts as the cathode (negative end) in this experiment

• The metal
• The solution
• The copper wire
• The buret
• The buret clamp
• The hydrogen ions
• The hydrogen gas

The copper wire

What property of the metal is measured in this experiment?

• Gain of mass by the metal
• Conductivity of the metal
• Resistivity of the metal
• Loss of mass of the metal

Loss of mass of the metal

The purpose of this experiment is to

• find the molar mass of a metal using moles of hydrogen produced when the metal is oxidized.
• find the molar mass of hydrogen using moles of metal lost when the metal is oxidized.
• find the molar mass of hydrogen using moles of metal lost when the metal is reduced.
• find the molar mass of a metal using moles of hydrogen produced when the metal is reduced.
• find the molar mass of hydrogen using moles of metal gained when the metal is reduced.
• find the molar mass of hydrogen using moles of metal gained when the metal is oxidized.

find the molar mass of a metal using moles of hydrogen produced when the metal is oxidized.

The H⁺ in this experiment is

• oxidized to H₂ gas.
• reduced to H₂ gas.

reduced to H₂ gas.

The barometric pressure of a room at 26 degrees C is found to be 752.0 mm Hg. The vapor pressure of water at this temperature is 25.2 mm Hg. What is the partial pressure of H₂ in a buret in this room during a similar experiment to this one?

• 777.2 mm Hg
• 752.0 mm Hg
• 25.2 mm Hg
• 726.8 mm Hg

726.8 mm Hg

How many moles of H₂ gas are present if the partial pressure of H₂ gas is 0.956 atm, its volume is 0.09500 L, and the temperature is 299 K. (Use R = 0.08206 L atm/K/mol).

HINT : Use PV = nRT

• 0.00370 moles
• 270. moles
• 362 moles
• 0.00276 moles

0.00370 moles