.. then
EITHER the pressure is halved for the same amount (moles) of gas,
OR
the amount (moles) of gas is doubled at the same pressure,
OR
any valid combination of these possibillities.
The temperature will increase, if the gas is ideal or nearly so. For an ideal gas, the product of pressure and volume equals a constant times the absolute temperature. If each of the temperature and pressure of the gas is doubled, the product of pressure and volume increases by a factor of 4, and the absolute temperature must increase by the same ratio.
When the volume of a gas is doubled with the temperature of the gas held constant, the pressure exerted by the gas reduces. This can be explained lucidly using the kinetic theory; when the gas is kept in a container closed by a movable piston, the gas molecules collide frequently as they are compressed by the piston but if the volume is increased by raising the the piston, the gas molecules are now more spaced out and thus the number of collision per second of the gas molecules decreases and pressure being the rate of collision decreases.Therefore as seen from the above explanation, when the volume of a gas is doubled, the pressure of the gas is consequently halved. This is in accordance to Boyle's law which states that " the volume(V) of a given mass of gas is inversely proportional to the pressure(P) provided the temperature remains constant"mathematically,V=k/P where K is a constant. (There is also the Boyle's,Charle's and the gas laws involved in this.)
if the pressure is decreased to half value the volume becomes doubled at constant temperature.
If the pressure doubles, the volume will be halved. This is according to Boyles Law when the temperature is constant (and the number of moles is constant). Thus, P1V1 = P2V2.
It is reduced by one half.
is reduced by one-half
The pressure increases
A sample of gas occupies 1.55L at STP. What will the volume be if the pressure is increased to 50 atm while the temperature remains constant?
The pressure will increase, proportionally to the decrease in volume. The Gas Law is PV=RT; then PdV + VdP = 0 if the Temperature stays constant.
Charles's law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its absolute temperature. For fixed mass of an Ideal Gas at constant pressure the volume it occupies is directly proportional to its absolute temperature. So, if you double the absolute temperature of a gas while holding its pressure constant, the volume has to double. There is no such thing as an Ideal Gas. So, doubling the temperature of a real gas will not exactly double its volume. However, the general principle hold true. If you increase the temperature of any gas at constant pressure the volume it occupies will increase.
volume decreases until the gas condenses to a liquid,
The pressure is reduced four times.
The volume is doubled.
A sample of gas occupies 1.55L at STP. What will the volume be if the pressure is increased to 50 atm while the temperature remains constant?
volume decreases considering the pressure is constant
The pressure will increase, proportionally to the decrease in volume. The Gas Law is PV=RT; then PdV + VdP = 0 if the Temperature stays constant.
It is halved. coz voltage=current * resistance
Charles's law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its absolute temperature. For fixed mass of an Ideal Gas at constant pressure the volume it occupies is directly proportional to its absolute temperature. So, if you double the absolute temperature of a gas while holding its pressure constant, the volume has to double. There is no such thing as an Ideal Gas. So, doubling the temperature of a real gas will not exactly double its volume. However, the general principle hold true. If you increase the temperature of any gas at constant pressure the volume it occupies will increase.
volume decreases until the gas condenses to a liquid,
The pressure is reduced four times.
The universal gas equation is PV = nRT (Pressure x Volume = Number of moles x Universal Gas Constant x Temperature in Kelvin/Rankin). So - if Pressure is constant, the number of moles is constant, but the temperature increases from 25C (298 K) to 125C (398K) - a 34% increase, a similar 34% increase in volume will occur.
increases by a factor of eight
increases by a factor of eight
The gas pressure increases by a factor of 8. The relevant equation is pV = nRT. Since nothing on the right side of this equation changes, the product on the left side must remain constant. The volume is stated to decrease by a factor of 4/0.5 or 8; therefore the pressure must increase by the same factor.