Which statement correctly describes the relationship between the volume of a gas and it’s temperature, in kelvin, assuming pressure is held constant?
The relationship is directly proportional as temperature increases volume, increases in the same way
The relationship is directly proportional as temperature increases volume, decreases in the same way
The relationship is inversely, proportional as temperature increases volume, increases in the same way
The relationship is inversely proportional as temperature increases volume, decreases in the same way
The correct statement is: The relationship is directly proportional as temperature increases, volume increases in the same way.
Which statement explains the molecular changes that occur in an enclosed gas as the pressure increases, and the temperature is held constant
An increase in pressure causes particles to move, farther apart, decreasing the volume
An increase in pressure causes particles to move closer together, decreasing the volume
An increase in pressure causes particles to move, farther apart, increasing volume
An increase in pressure causes the particles to move closer together, increase your volume
The correct statement is: An increase in pressure causes particles to move closer together, decreasing the volume.
The ideal gas law is represented by PV = nRT. As volume is held constant and the temperature increases. How about the pressure be expected to change.
It would remain constant
It would become zero
It would decrease
It would increase
If the volume is held constant and the temperature increases, according to the ideal gas law (PV = nRT), the pressure is expected to increase.
When did the pressure of a gas decreases, which quantity will increase, assuming all other variables are held constant?
P
n
V
T
When the pressure of a gas decreases, assuming all other variables are held constant, the quantity that will increase is the volume (V).
Two balloons whole two different gases. The gases are held at the same pressure, volume, and temperature. Which quantity can defer between the two gases?
The number of moles, in each gas
The mass of each gas
The molar volume of each gas
The gas, constant of each gas
The quantity that can differ between the two gases is the number of moles in each gas.
The correct statement is:
The relationship is directly proportional as temperature increases, volume increases in the same way.
To understand this relationship, we can refer to the ideal gas law, which states that the product of pressure (P), volume (V), and temperature (T) of a gas is proportional to the number of gas molecules (n) and the universal gas constant (R). Mathematically, this can be represented as:
PV = nRT
With pressure being held constant, we can rearrange the equation to isolate the volume:
V ∝ T
This means that volume is directly proportional to temperature. When the temperature of a gas increases, its volume also increases in the same proportion. Similarly, when the temperature decreases, the volume decreases in the same proportion.
Therefore, the correct statement is that the relationship between the volume of a gas and its temperature, assuming constant pressure, is directly proportional.