Part 1. What do we call a gas which fulfills all five of these assumptions ? Ide
ID: 635967 • Letter: P
Question
Part 1.
What do we call a gas which fulfills all five of these assumptions ?
Ideal gas
Inert gas
Noble gas
Diatomic gas
Part 2.
Which assumption is incorrect for non-spherical gas molecules ?
Gases consist of particles (molecules or atoms) that are in constant random motion.
Gas particles are constantly colliding with each other and the walls of their container. These collisions are elastic; that is, there is no net loss of energy from the collisions.
Gas particles are small and the total volume occupied by gas molecules is negligible relative to the total volume of their container.
There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.
The average kinetic energy of gas particles is proportional to the absolute temperature of the gas, and all gases at the same temperature have the same average kinetic energy.
Part 3.
Which assumption is incorrect for gas molecules at high pressure (packed tightly together) ?
Gases consist of particles (molecules or atoms) that are in constant random motion.
Gas particles are constantly colliding with each other and the walls of their container. These collisions are elastic; that is, there is no net loss of energy from the collisions.
Gas particles are small and the total volume occupied by gas molecules is negligible relative to the total volume of their container.
There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.
The average kinetic energy of gas particles is proportional to the absolute temperature of the gas, and all gases at the same temperature have the same average kinetic energy.
Part 4.
Which assumption is incorrect for gas molecules at a temperature low enough to be liquid or solid ?
Gases consist of particles (molecules or atoms) that are in constant random motion.
Gas particles are constantly colliding with each other and the walls of their container. These collisions are elastic; that is, there is no net loss of energy from the collisions.
Gas particles are small and the total volume occupied by gas molecules is negligible relative to the total volume of their container.
There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.
The average kinetic energy of gas particles is proportional to the absolute temperature of the gas, and all gases at the same temperature have the same average kinetic energy.
Part 5.
Which assumption is incorrect for gas molecules which are highly polar (have electrostatic forces between molecules) ?
Gases consist of particles (molecules or atoms) that are in constant random motion.
Gas particles are constantly colliding with each other and the walls of their container. These collisions are elastic; that is, there is no net loss of energy from the collisions.
Gas particles are small and the total volume occupied by gas molecules is negligible relative to the total volume of their container.
There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.
The average kinetic energy of gas particles is proportional to the absolute temperature of the gas, and all gases at the same temperature have the same average kinetic energy.
Part 6.
Which of the following laws went into deriving the Ideal Gas Law,
P V = n R T ?
Boyles
Charles
Guy-lussacs
Avogadros law
All the above
Part 7.
When a gas sample is held at constant temperature, which of the simple gas laws is the result ?
Boyle’s
Charles’s
Guy-Lussac’s
Avagadro’s law
All the above.
Part 8
When a gas sample is held at constant Pressure, which of the simple gas laws is the result ?
Boyle’s
Charles’s
Guy-Lussac’s
Avagadro’s law
All the above.
Part 9.
When a gas sample is held at constant volume, which of the simple gas laws is the result ?
Boyle’s
Charles’s
Guy-Lussac’s
Avagadro’s law
All the above.
Part 10.
When there is a tiny leak in a balloon, which gas law explains the result ?
Boyle’s
Charles’s
Guy-Lussac’s
Avagadro’s law
All the above.
Part 11
The percentages in tables of the various gases in air are a form of mole fraction calculations.
True or false?
Part 12
A scientist sets up a gas experiment with a container holding 5.00 moles of oxygen gas, 2.00 moles of hydrogen gas, and 3.00 moles of argon gas. The mole fraction of hydrogen gas is
0.200
0.500
0.400
0.300
Part 13
A scientist sets up a gas experiment with a container holding 5.00 moles of oxygen gas, 2.00 moles of hydrogen gas, and 3.00 moles of argon gas. If the gas mixture is at STP, what is the volume of the container ?
44.8L
112 L
22.4 L
2.24 L
Part 14.
A scientist sets up a gas experiment with a container holding 5.00 moles of oxygen gas, 2.00 moles of hydrogen gas, and 3.00 moles of argon gas. If the gas mixture is at STP, what is the partial pressure of the hydrogen gas ?
Part 15
A scientist sets up a gas experiment with a container holding 5.00 moles of oxygen gas, 2.00 moles of hydrogen gas, and 3.00 moles of argon gas. If the gas is compressed until the pressure is at 10 atm at 0oC, what will the volume be ?
Explanation / Answer
Part 1.
What do we call a gas which fulfills all five of these assumptions ?
Answer :Ideal gas
Part 2.
Which assumption is incorrect for non-spherical gas molecules ?
Answer : Gas particles are small and the total volume occupied by gas molecules is negligible relative to the total volume of their container.
Part 3.
Which assumption is incorrect for gas molecules at high pressure (packed tightly together) ?
Answer : There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.
Part 4.
Which assumption is incorrect for gas molecules at a temperature low enough to be liquid or solid ?
Answer : There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.
Part 5.
Which assumption is incorrect for gas molecules which are highly polar (have electrostatic forces between molecules) ?
Answer : There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.
Part 6.
Which of the following laws went into deriving the Ideal Gas Law,
P V = n R T ?
Answer : Boyles, Charles and Avogadros law.
Part 7.
When a gas sample is held at constant temperature, which of the simple gas laws is the result ?
Answer : Boyle’s law
Part 8
When a gas sample is held at constant Pressure, which of the simple gas laws is the result ?
Answer : Charles’s law
Part 9.
When a gas sample is held at constant volume, which of the simple gas laws is the result ?
Answer : Guy-Lussac’s law
Part 10.
When there is a tiny leak in a balloon, which gas law explains the result ?
Answer : Boyle’s law
Part 11
The percentages in tables of the various gases in air are a form of mole fraction calculations.
Answer : True
Part 12
A scientist sets up a gas experiment with a container holding 5.00 moles of oxygen gas, 2.00 moles of hydrogen gas, and 3.00 moles of argon gas. The mole fraction of hydrogen gas is
Molefraction = (moles of single gas) /(moles of all the gasesin the mixture)
molefraction of Hydrogen gas = moles of Hydrogen gas/( sum of the moles of all gases)
= (2.00)/(5.00+2.00+3.00)
= 0.200