Adv CHEM Unit 9 Days 1-3 Review

Consider the two samples of helium gas pictured.  The gases are in a flexible container. Which of the following best explains the differences in volume of the two samples?  Justify your answer. 

• The Kelvin temperature of container B is triple the Kelvin temperature of container A.  According to the equation PV=nRT, volume and Kelvin temperature are INVERSELY related.  If the Kelvin temp is tripled under constant pressure and number of moles conditions, the volume must triple as well.
• The Kelvin temperature of container A is triple the Kelvin temperature of container B.  According to the equation PV=nRT, volume and Kelvin temperature are DIRECTLY related.  If the Kelvin temp is tripled under constant pressure and number of moles conditions, the volume must triple as well.
• The Kelvin temperature of container B is triple the Kelvin temperature of container A.  According to the equation PV=nRT, volume and Kelvin temperature are DIRECTLY related.  If the Kelvin temp is tripled under constant pressure and number of moles conditions, the volume must triple as well.
• The Kelvin temperature of container A is triple the Kelvin temperature of container B.  According to the equation PV=nRT, volume and Kelvin temperature are INVERSELY related.  If the Kelvin temp is tripled under constant pressure and number of moles conditions, the volume must triple as well.

Consider the two samples of helium gas pictured.  The gases are in a flexible container. Which of the following best explains the differences in pressure of the two samples?  Justify your answer. 

• The volume of container B is double the volume of container A.  According to the equation PV=nRT, pressure and volume are DIRECTLY related.  If the volume is doubled under constant temperature and number of moles conditions, pressure will be halved.
• The volume of container B is double the volume of container A.  According to the equation PV=nRT, pressure and volume are INVERSELY related.  If the volume is doubled under constant temperature and number of moles conditions, pressure will be halved.
• The volume of container A is double the volume of container B.  According to the equation PV=nRT, pressure and volume are INVERSELY related.  If the volume is doubled under constant temperature and number of moles conditions, pressure will be halved.
• The volume of container A is double the volume of container B.  According to the equation PV=nRT, pressure and volume are DIRECTLY related.  If the volume is doubled under constant temperature and number of moles conditions, pressure will be halved.

Consider the two samples of helium gas pictured.  The samples are in a rigid container.  Which of the following best explains the differences in pressure of the two samples?  Justify your answer. 

• The number of moles of He in container B is double the number of moles of container A.  According to the equation PV=nRT, pressure and number of moles are DIRECTLY related. If the pressure is doubled under constant temperature and volume conditions, the number of moles will double as well. 
• The number of moles of He in container B is double the number of moles of container A.  According to the equation PV=nRT, pressure and number of moles are INVERSELY related. If the pressure is doubled under constant temperature and volume conditions, the number of moles will double as well. 
• The number of moles of He in container A is double the number of moles of container B.  According to the equation PV=nRT, pressure and number of moles are DIRECTLY related. If the pressure is doubled under constant temperature and volume conditions, the number of moles will double as well. 
• The number of moles of He in container A is double the number of moles of container B.  According to the equation PV=nRT, pressure and number of moles are INVERSELY related. If the pressure is doubled under constant temperature and volume conditions, the number of moles will double as well. 

Tags

NGSS.HS-PS1-7

How does the average kinetic energy of the helium atoms in Container A compare to the average kinetic energy of the helium atoms in Container B?

• The average kinetic energy of helium atoms in Container A is half the average kinetic energy of helium atoms in Container B because the pressure in Container A is half the  pressure in Container B. Average kinetic energy is directly related to pressure.
• The average kinetic energy of helium atoms in Container A is half the average kinetic energy of helium atoms in Container B because the number of moles in Container A is half the number of moles in Container B. Average kinetic energy is directly related to number of moles.
• The average kinetic energy of helium atoms in Container A is the same as the average kinetic energy of helium atoms in Container B because the volumes of the containers are the same. Average kinetic energy is directly related to volume. 
• The average kinetic energy of helium atoms in Container A is the same as the average kinetic energy of helium atoms in Container B because the temperatures of the gases in the containers are the same. Average kinetic energy is directly related to temperature.

Consider the mixture of gases pictured.  
Helium has the _________ AVERAGE KINETIC ENERGY as neon because it has _____________.

• SAME:
  THE SAME TEMPERATURE
• SAME:
  THE SAME PRESSURE
• HIGHER:
  THE LOWER MOLAR MASS
• LOWER:
  THE HIGHER MOLAR MASS

Tags

NGSS.HS-PS3-2

Consider the mixture of gases pictured.  
Which of the gases occupy a larger volume?

• Helium because it has a smaller molar mass. 
• Neon because it has a larger molar mass. 
• The both occupy the same volume because they are in the same container. 
• It is impossible to tell without knowing the number of moles of each gas.

Consider the mixture of gases pictured.  
Helium has the _________ VELOCITY as neon because it has _____________.

• SAME:
  THE SAME TEMPERATURE
• SAME:
  THE SAME PRESSURE
• HIGHER:
  THE LOWER MOLAR MASS
• LOWER:
  THE HIGHER MOLAR MASS

Tags

NGSS.HS-PS3-2

The following plot is for an ideal gas. Consider the ideal gas equation, PV=nRT, and identify what state function(s) could be represented by x for this plot.

• P, T, or n
• P, or T
• P, or n
• T, or n

A rigid vessel is connected to four separate 2.00 liter gas cylinders. Each cylinder contains a separate, diatomic gas at room temperature. When the gases are combined and held at room temperature, which of the following most accurately describes what happens in the reaction vessel?

• All of the gases immediately diffuse at the same rate, causing the kinetic energy of the substances to increase.
• The heavier diatomic gases diffuse slower than the lighter diatomic gases, causing a heterogeneous mixture in the new system.
• The rate of diffusion differs for each gas, but the overall kinetic energy of the system remains constant.
• The lightest mass gas is unable to diffuse into the new system due to the increased pressure by the heavier gases causing only three of the four gases to mix in the new container.

The N₂ gas particles in  the container shown is initially at 27°C.  The lengths of the arrows represents the speeds of the particles.  Which of the following diagrams best represents the particles when the vessel is heated to 127°C?

• A
• B
• C
• D

Tags

NGSS.HS-PS1-5