If you know other factors, you could use PV=nRT, where P is pressure, V is volume, n is the number of moles of the gas, R is the gas constant (typically 0.0821, but it depends on the units of the other factors), and T is temperature.
However, if you don't know those other factors, or have no need for them, Boyle's law will suffice: P1V1=P2V2.
Pressure will decrease with (because it is inversely proportianal to) volume, if (and only if!) temperature is held constant.
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"Constant pressure" means the pressure must not change.
Temperature is really just the amount of kinetic energy in the molecules of a substance. If you add more energy by heating the substance then the molecules dash about faster and faster. This increases the pressure if the substance is constrained, like gas in a jar or in a bomb.
Assuming the temperature stays constant and there is no leakage of gas, then if the container decreases in size then the pressure will increase.
Assuming the volume is kept constant, the pressure will also decrease in this case.
Pressure will decrease with (because it is inversely proportianal to) volume, if (and only if!) temperature is held constant.
Yes. If the temperature increases, the gas expands (assuming the pressure remains constant).
Assuming no change in temperature and pressure, calculate the volume of O2 (in liters) required for the complete combustion of 14.9 L of butane (C4H10):
Assuming that pressure and the amount of matter are constant (meaning they do not change), volume will increase as temperature increases.
Liquids. By assuming that temperature and pressure are constant so that volume does not change.
Boyles Law deals with conditions of constant temperature. Charles' Law deals with conditions of constant pressure. From the ideal gas law of PV = nRT, when temperature is constant (Boyles Law), this can be rearranged to P1V1 = P2V2 (assuming constant number of moles of gas). When pressure is constant, it can be rearranged to V1/T1 = V2/T2 (assuming constant number of moles of gas).
Boyles Law deals with conditions of constant temperature. Charles' Law deals with conditions of constant pressure. From the ideal gas law of PV = nRT, when temperature is constant (Boyles Law), this can be rearranged to P1V1 = P2V2 (assuming constant number of moles of gas). When pressure is constant, it can be rearranged to V1/T1 = V2/T2 (assuming constant number of moles of gas).
You can calculate pressure and temperature for a constant volume process using the combined gas law.
As the pressure increases, the volume wil decrease.
assuming the balloon is closed, the air pressure would double
Temperature increases as pressure increases.