Boyles law states: P=c/V where P is pressure, c is some constant, and V is volume. It can more applicably express as PV=c by simple algebraic method.
If C is to remain constant than anything that happens to P has to be undone by a reaction in V. So if P doubles, V has to fall by half.
If the pressure is halved from 500 kPa to 250 kPa (a decrease), we can expect the volume to double if the temperature remains constant. This means the new volume would be 400 mL when starting with an initial volume of 200 mL.
Increasing the pressure would increase the yield of sulfur trioxide because the reaction involves a decrease in volume. Decreasing the pressure would decrease the yield of sulfur trioxide because the reaction volume would increase.
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.
If the temperature increases, then the volume of the gases cannot stay the same. The pressure will keep building until it overcomes the integrity of the container its contained in and causes an explosion.
The volume of gas at a depth of 100 feet would depend on the pressure and temperature at that depth. As pressure increases with depth, gas volume decreases. To calculate the exact volume, you would need to know the specific pressure and temperature conditions at that depth.
If the pressure is doubled according to the ideal gas equation (PV = nRT), and the other variables remain constant, then the volume would be halved. This is because pressure and volume are inversely proportional when the other variables are constant in an ideal gas.
If the volume is halved from 20.00 ml to 10 ml, according to Boyle's Law, the pressure would double assuming the temperature remains constant. This inverse relationship between pressure and volume is described by Boyle's Law: P1V1 = P2V2.
If the pressure is halved from 500 kPa to 250 kPa (a decrease), we can expect the volume to double if the temperature remains constant. This means the new volume would be 400 mL when starting with an initial volume of 200 mL.
Pressure and volume are inversely proportional at any given temperature and quantity of molecules. Thus, a mole of gas squeezed into half the volume would have double the pressure if all other things remain equal. Conversely, a mole of gas whose pressure was halved would occupy double the volume, all other things remaining equal.
circumference would be halved, area would be one fourth of original , andvolume would be one eighth of original.
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 temperature and volume is fixed,pressure reduces.
Pressure is halved when ONLY volume is doubled (n and T are constant).Remember the General Gas Law:p.V = n.R.T(in which R=general gas constant)
The volume is reduced by 7/8. for example - if you had a cube measuring 4 cm each side - the volume would be 4x4x4=64cm3. Halving each side to 2cm would result in the sum 2x2x2=8cm3. 8 is one-eighth of 64.
Pressure and volume are inversely proportional at any given temperature and quantity of molecules. Thus, a mole of gas squeezed into half the volume would have double the pressure if all other things remain equal. Conversely, a mole of gas whose pressure was halved would occupy double the volume, all other things remaining equal.
Increasing the pressure would increase the yield of sulfur trioxide because the reaction involves a decrease in volume. Decreasing the pressure would decrease the yield of sulfur trioxide because the reaction volume would increase.
since there were no enough water and salts reabsored, there woulnd't be enough blood volume, and blood pressure will be decreased.