According to Boyle's Law, if the volume of a gas is increased while the temperature remains constant, the pressure of the gas will decrease. This is because the gas molecules have more space to move around, resulting in fewer collisions with the walls of the container, which leads to lower pressure. Conversely, if the volume decreases, the pressure would increase.
If the pressure of a gas in a closed system increases, the volume of the gas would decrease, following Boyle's Law. This is because there is an inverse relationship between pressure and volume when temperature is constant.
If the volume of the tank was effectivelly constant, and the tank was sealed to prevent gas escaping, the pressure of the gas would increase.
Assuming all other conditions remain constant (temperature and amount of gas), Boyle's law states that the volume of a gas is inversely proportional to its pressure. Therefore, if the pressure is increased to 40 kPa, the volume of the gas would decrease proportionally.
Volume & pressure are inversely proportionate, if temperature stays constant volume would decrease at a factor proporionate to the increase in pressure.
The volume of the container is increased.
Reducing the volume that a gas occupies will increase the pressure because it reduces the surface area that the gas has to impact against. Likewise increasing the temperature will increase pressure by increasing the kinetic energy of the gas molecules.
the volume would get bigger, and the solid itself would just get bigger.
If temperature and volume is fixed,pressure reduces.
It's Pressure would rise.
The ideal gas law states that pressure (P) is directly proportional to temperature (T) at constant volume. So if the temperature is increased to 3T, the pressure would also increase by a factor of 3.
Since the stroke volume increased then the cardiac out put would increase, pumping out more blood with the same amount of heart beats.
Its volume would increase (apex)