If you put a higher amount of gas into a container with a constant volume and temperature, several things will happen:
Increase in Pressure: According to Boyle's Law, which states that at constant temperature, the pressure and volume of a gas are inversely proportional, the increased amount of gas will lead to an increase in pressure. Since the volume remains constant, the gas particles will have less space to move around, resulting in more frequent collisions with the container walls, thus increasing the pressure exerted by the gas.
Increased Density: With a higher amount of gas in the same volume, the gas density will increase. Density is defined as mass per unit volume, so as the amount of gas (mass) increases while the volume remains constant, the gas particles will become more closely packed together, resulting in a higher density.
Unchanged Temperature: Since the container's temperature is constant, the average kinetic energy of the gas particles will remain the same. The increased number of gas particles will lead to more frequent collisions, but the average speed and temperature of the gas will remain constant.
It's important to note that these observations hold true under the assumption that the gas behaves ideally, meaning that it follows the ideal gas law. The ideal gas law states that at constant temperature and volume, the pressure of a gas is directly proportional to the amount of gas (measured in moles) present. However, if the gas is non-ideal or exhibits deviations from ideal gas behavior, additional factors such as intermolecular forces may come into play, and the behavior of the gas may deviate from what is described above.