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The ideal gas law is represented by PV = RT. As volume is held constant and the temperature increases, how would the

pressure be expected to change? (1 point)

11 answers

According to the ideal gas law, expressed as \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles of gas, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin, we can analyze the scenario where volume is held constant.

If the volume (\( V \)) is constant and the temperature (\( T \)) increases, we can rearrange the equation to isolate pressure:

\[ P = \frac{nRT}{V} \]

Since \( n \) (the number of moles) and \( R \) (the ideal gas constant) are both constants in this scenario, an increase in temperature (\( T \)) will lead to a proportional increase in pressure (\( P \)). Thus, as the temperature increases at constant volume, the pressure will also increase.

In summary, if the temperature increases while the volume is held constant, the pressure is expected to increase.

When the pressure of a gas decreases, which quantity will increase, assuming all other variables are held constant? (1 point)

According to Boyle's Law, which states that \( P \propto \frac{1}{V} \) when the temperature and the amount of gas are held constant, if the pressure (\( P \)) of a gas decreases, the volume (\( V \)) of the gas will increase, assuming all other variables remain constant.

So, when the pressure of a gas decreases (while holding temperature and the amount of gas constant), the volume will increase.

V
R
n
T

It seems you are asking for the relationship between pressure, volume, moles of gas, and temperature in the context of the ideal gas law \( PV = nRT \).

To clarify further based on your question:

  • \( V \) (Volume): When pressure \( P \) decreases and all other variables are held constant (i.e., \( n \) and \( T \)), the volume \( V \) will increase.

  • \( R \) (Ideal gas constant): This is a constant value and does not change with pressure.

  • \( n \) (Number of moles of gas): Assuming the amount of gas does not change, \( n \) remains constant.

  • \( T \) (Temperature): If pressure decreases but temperature remains constant, then temperature itself does not change.

Given your question about which quantity will increase when the pressure of a gas decreases (holding all other variables constant), the correct answer is Volume \( V \) will increase.

If you meant something else by providing the letters (V, R, n, T), please specify, and I would be happy to assist you further!

Two balloons hold two different gases. The gases are held at the same pressure, volume, and temperature. Which quantity can differ between the two gases? (1 point)

When two balloons hold two different gases at the same pressure, volume, and temperature, the quantity that can differ between the two gases is the number of moles (\( n \)) of the gases.

According to the ideal gas law \( PV = nRT \), if pressure (\( P \)), volume (\( V \)), and temperature (\( T \)) are the same, the number of moles of gas (\( n \)) can vary, leading to different gases having different masses or molecular identities, despite the other conditions being identical. Thus, the quantity that can differ is \( n \).

• the number of moles of each gas
• the mass of each gas
© the molar volume of each gas
• the gas constant of each gas

Given that two balloons hold two different gases at the same pressure, volume, and temperature, let’s analyze the quantities listed:

  1. The number of moles of each gas: This can differ between the two gases if they have different molar masses.

  2. The mass of each gas: This can also differ because mass is the product of the number of moles and molar mass (\( \text{mass} = n \times \text{molar mass} \)). If the gases have different molar masses or different moles, their masses will differ.

  3. The molar volume of each gas: At a given temperature and pressure, all ideal gases occupy the same molar volume (approximately 22.4 L/mol at STP). However, real gases may not always behave ideally, but under the stated conditions, molar volume would typically be consistent for ideal gases regardless of the type.

  4. The gas constant of each gas: The gas constant \( R \) is the same for all ideal gases and does not depend on the type of gas. It is a universal constant.

Based on the analysis, the quantities that can differ between the two gases are:

  • The number of moles of each gas
  • The mass of each gas

If you're looking for a single selection based on typical question patterns, usually, the first two options (number of moles and mass) are the most directly different characteristics under the conditions indicated.

Choose one please

The quantity that can differ between the two gases is the number of moles of each gas.