0
What else can I help you with?
How does reducing the volume of gas affect its pressure if the temperature of the gas and the number of particles are constant?
The pressure is now higher.
How are pressure and the number of the particle related?
PV = NkT P: pressure V: volume N: number of particles in gas k: Boltzmann's constant T: absolute temperature More particles in a constant volume, constant temperature space means more pressure.
How does pressure temperature and the number of particles affect the behavior of a gas?
The combined gas equation is used to calculate the behaviour of gas under different temperature, pressure and number of particles. PV = nRT Where P is pressure V is volume n is the number of moles T is the temperature in Kelvin and R is the Ideal Gas Constant. If P is in kPa and V is in dm3 then R = 8.31.
What are the effects of temperature and volume of gas samples at constant pressure?
If the volume is constant, the density does not change with temperature. With increasing temperature there is still the same number of molecules confined to the same volume of space, so no difference in density.
Why does vapor pressure increase with an increase in temperature?
PV=nRT where P=pressure, V=volume, n=no. of moles, R=gas constant, T=temperature(K) since volume and the number of moles remain constant, they can be ignored and we can assume:- that P is proportional to T and thus if temperature is increased, pressure will also increase.
What happens to the temperature increase the number of particles what happens to the pressure?
Increasing the temperature the number of particles remain constant and the pressure increase.
Why does pressure increase with an increase in temperature?
PV=nRT where P=pressure, V=volume, n=no. of moles, R=gas constant, T=temperature(K) since volume and the number of moles remain constant, they can be ignored and we can assume:- that P is proportional to T and thus if temperature is increased, pressure will also increase.
How does the volume of an ideal gas at constant temperature and pressure change as the number of molecules increases?
The volume of an ideal gas will increase as the number of molecules increases at constant temperature and pressure. This relationship is described by Avogadro's law, which states that the volume of a gas is directly proportional to the number of molecules present, assuming constant temperature and pressure.
How does reducing the volume of gas affect its pressure if the temperature of the gas and the number of particles are constant?
The pressure is now higher.
When temperature and number of particles of a gas are constant what is also constant?
When temperature and number of particles of a gas are constant, the pressure of the gas remains constant as well if the volume is fixed. This is known as Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when temperature and quantity of gas are held constant.
What would the effect on temperature and volume be if you changed the number of moles of gas in a container?
In a container the volume remain constant but the pressure increase.
What When the volume and number of particles of a gas are constant is also constant?
The temperature and pressure.
When the volume and number of particles of a gas are constant is also constant?
The temperature and pressure.
How are pressure and the number of the particle related?
PV = NkT P: pressure V: volume N: number of particles in gas k: Boltzmann's constant T: absolute temperature More particles in a constant volume, constant temperature space means more pressure.
How does pressure temperature and the number of particles affect the behavior of a gas?
The combined gas equation is used to calculate the behaviour of gas under different temperature, pressure and number of particles. PV = nRT Where P is pressure V is volume n is the number of moles T is the temperature in Kelvin and R is the Ideal Gas Constant. If P is in kPa and V is in dm3 then R = 8.31.
Does an increase in pressure at constant temperature increase the rate constant of a reversible reaction in both directions?
The rate constant is unaffected, as demonstrated by Arrhenius equation: k = Ae^(-E/RT) where A is the pre-exponential factor (constant for a particular reaction) E is the activation energy R is the molar gas constant T is the thermodynamic temperature However, when pressure is increased at constant temperature for a gaseous reversible reaction, the concentrations of every reactant and product increase by the SAME factor. Since Kp (pressure equilibrium constant) is to remain constant, it means that the position of equilibrium will shift in such a way so as to decrease the total number of moles of gaseous species. Note: This answer can be improved by proving the last statement using a general example which, due to lack of time, I skipped. (Although some people might get the logic!!!)
If you wanted to predict how temperature will effect the volume of a gas what factors must be held constant?
If temperature increases, then pressure increases. Temperature measures the average speed of particles, so if the temperature is high, then the particles are moving quickly and are colliding with other particles more forcefully. Pressure is defined as the force and number of collisions the particles have with the wall of its container. So if the high temperature causes the particles to move quickly, they are going to collide more often with the container, increasing the pressure. This remains true as long as the number of moles (n) remains constant.
