Which statement correctly describes the relationship between the volume of a gas and its temperature, in Kelvin, assuming pressure is held constant?(1 point)
The relationship is inversely 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 directly proportional; as temperature increases, volume decreases in the same way.
The relationship is directly proportional; as temperature increases, volume increases in the same way.
Technically I don't like any of them. D comes the closest to being correct if it left off that part about being "in the same way". V goes up when T goes up and V goes down when T goes down. And the amount of increase or decrease is function of the kelvin temperature.
The correct statement that describes the relationship between the volume of a gas and its temperature, assuming pressure is held constant, is: "The relationship is directly proportional; as temperature increases, volume increases in the same way."
The correct statement that describes the relationship between the volume of a gas and its temperature, assuming pressure is constant, is: "The relationship is directly proportional; as temperature increases, volume increases in the same way."
To understand why this is the correct statement, we can refer to the ideal gas law: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
When the pressure is constant, this equation can be simplified to V = kT, where k is a constant.
According to this equation, temperature (T) and volume (V) have a direct proportional relationship. If the temperature increases, the volume also increases, and if the temperature decreases, the volume also decreases.
So, the correct statement is that as the temperature increases, the volume of a gas also increases in the same way.