Respuesta :
C. Both A. and B.
Explanation:
Statement A. Reducing the volume is true because of Boyle's law, which states that for a gas at fixed temperature, the pressure p and the volume V are inversely proportional:
[tex]pV=const.[/tex]
Therefore, when the volume V is reduced, the pressure p increases.
Statement B. Adding more gas is also true: in fact, if we add gas into the container, we will have more molecules of the gas hitting the wall of the container. But the pressure of a gas is exactly given by this: by the collision of the molecules against the wall of the container, so the more the molecules of gas, the greater the pressure.
The pressure in the gas container is increased by reducing the volume of the gas and also by adding more gas to the container.
Further Explanation:
The pressure of the gas is given by the Boyle’s law. It states that at constant temperature, the pressure of the gas is inversely proportional to the volume of the gas. The expression for the Boyle’s law is written as.
[tex]\begin{gathered}p\propto \frac{1}{v} \\\Rightarrow pv = {\text{constant}} \\\end{gathered}[/tex]
Therefore, if the volume of the gas container is reduced, it will lead to the increase in the pressure of the gas inside the container.
On the other hand, if the amount of gas inside the container is increased, the number of molecules hitting the per unit area of the wall will be increased and this will also lead to the increase in the pressure of the gas inside the container.
Thus, the pressure of the gas inside the container is increased by decreasing the volume of the gas and also by increasing the amount of gas inside the container.
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Answer Details:
Grade: High School
Chapter: Gas Laws
Subject: Physics
Keywords: Charles’s law, Boyle’s law, increase in pressure, closed container, reducing the volume, adding more gas, number of molecules, volume of gas.
