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Pressure will decrease with (because it is inversely proportianal to) volume, if (and only if!) temperature is held constant.
Charles's Law states that (Volume)/(Temperature) is constant, assuming constant pressure and moles of gas. This means that (V1)/(T1) = (V2)/(T2). So if the volume of the gas increases, V2 is bigger than V1; to keep the ratio constant, T2 must also increase, which represents an increase in temperature.
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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 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.
Charles's Law states that (Volume)/(Temperature) is constant, assuming constant pressure and moles of gas. This means that (V1)/(T1) = (V2)/(T2). So if the volume of the gas increases, V2 is bigger than V1; to keep the ratio constant, T2 must also increase, which represents an increase in temperature.
Yes. If the temperature increases, the gas expands (assuming the pressure remains constant).
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).
As the pressure increases, the volume wil decrease.
assuming the balloon is closed, the air pressure would double
Temperature increases as pressure increases.
As pressure increases, if temperature is constant, the gas will decrease in volume.