The initial pressure is halved. Use Boyle's law that relates pressure & volume at a constant temperature.
P1V1 = P2V2
In this case the V1(initial volume) is doubled so V2 = 2V1
P2 = P1V1/V2 = P1V1/2V1
P2 = (1/2)*P1
.. thenEITHER the pressure is halved for the same amount (moles) of gas,ORthe amount (moles) of gas is doubled at the same pressure,ORany valid combination of these possibillities.
When the volume is doubled at constant temperature, the total pressure of the system remains constant. Therefore, the partial pressures of N2O4 and NO2 will adjust accordingly to maintain the total pressure. Use the ideal gas law to calculate the new equilibrium partial pressures.
When pressure is increased on a fixed mass of gas at constant temperature, the volume of the gas will decrease. This is known as Boyle's Law, which states that pressure and volume are inversely proportional when temperature is held constant.
Using the combined gas law (P1/T1 = P2/T2), we can calculate the new temperature at the safe limit pressure: (388 kPa / 273 K) = (825 kPa / T2) T2 = 273 K * (825 kPa / 388 kPa) T2 = 578 K Therefore, the gas will reach a pressure of 825 kPa at a temperature of 578 K.
the temperature is constant. This means that as the pressure of a gas increases, its volume decreases, and vice versa, as long as the temperature remains the same. The relationship between pressure and volume can be described by the equation PV = k, where P is pressure, V is volume, and k is a constant.
To change from 380 torr and 546 K to standard temperature and pressure (STP: 1 atm and 273 K), the pressure decreases from 380 torr to 1 atm, and the temperature decreases from 546 K to 273 K. This change can be calculated using the ideal gas law and the principles of gas behavior.
Increasing the the pressure the volume decrease.The law of Boyle and Mariotte: P.V= k
Increasing the the pressure the volume decrease.The law of Boyle and Mariotte: P.V= k
Increasing the the pressure the volume decrease.The law of Boyle and Mariotte: P.V= k
If the pressure on a confined gas is doubled (assuming temperature remains constant), the volume of the gas will be reduced by half. This is known as Boyle's Law, which states that pressure and volume are inversely proportional when temperature is constant.
The ideal Gas Law states the following: pV=nRT p=pressure [pa] V=volume [m³] n=number of moles R=constant T=temperature [K] So, if you multiply the number of moles by 2, and all the other variables are not changed, your volume will also be multiplied by 2.
.. thenEITHER the pressure is halved for the same amount (moles) of gas,ORthe amount (moles) of gas is doubled at the same pressure,ORany valid combination of these possibillities.
At stp or standard temperature and pressure, we have pressure = 100kPa and temperature=273.15 K
When the volume is doubled at constant temperature, the total pressure of the system remains constant. Therefore, the partial pressures of N2O4 and NO2 will adjust accordingly to maintain the total pressure. Use the ideal gas law to calculate the new equilibrium partial pressures.
60kpa
It becomes double as K=Q/t×L/A(T2-T1) so if the thickness (L) of an object is doubled the thermal conductivity will be doubled as thermal conductivity is directly proportional to the thickness/L of the object K=L K=2L,K=2 two times
When pressure is increased on a fixed mass of gas at constant temperature, the volume of the gas will decrease. This is known as Boyle's Law, which states that pressure and volume are inversely proportional when temperature is held constant.