What will happen to the volume of the gas if the number of moles is doubled?

Volume will become double since V ∝ n according to Avogadro’s law.

What will happen to the volume of a gas if the pressure will be reduced at constant temperature?

The combined gas law states that the pressure of a gas is inversely related to the volume and directly related to the temperature. If temperature is held constant, the equation is reduced to Boyle’s law. Therefore, if you decrease the pressure of a fixed amount of gas, its volume will increase.

What happened to the volume when the temperature decreases?

These examples of the effect of temperature on the volume of a given amount of a confined gas at constant pressure are true in general: The volume increases as the temperature increases, and decreases as the temperature decreases.

What happens to the volume of the gas being measured when the temperature or pressure changes during the experiment?

If the number of gas molecules and the temperature remain constant, then the pressure is inversely proportional to the volume. If the temperature changes and the number of gas molecules is kept constant, then either pressure of volume will change in direct proportion to the temperature.

What happens to the volume of a gas when the number of moles of gas is doubled while keeping the temperature and pressure constant?

According to the Avogadro’s Law : The volumes of the same number of moles of all gases measured at constant pressure and temperature are the same. Therefore,volume will be doubled if number of moles are doubled.

What will happen to the pressure of a gas if its volume triples increases by a factor of three as the amount of gas and the temperature are held constant?

Explanation: Boyle’s law states that the pressure of a gas and the volume it occupies are inversely proportional. Therefore, if the pressure increases by a factor of 3 (tripled), then at constant temperature, we expect the volume to decrease by a factor of 13 (“cut in third”).

What happens to the volume the gas occupies?

Decreasing the volume of a gas increases the pressure of the gas. An example of this is when a gas is trapped in a cylinder by a piston. If the piston is pushed in, the gas particles will have less room to move as the volume the gas occupies has been decreased.

What happens to the volume the gas occupies when the pressure on a gas increases it decreases it increases it has no effect on it?

The Relationship between Pressure and Volume: Boyle’s Law. As the pressure on a gas increases, the volume of the gas decreases because the gas particles are forced closer together. Conversely, as the pressure on a gas decreases, the gas volume increases because the gas particles can now move farther apart.

What is the volume of nitrogen gas at STP?

According to Avogadro’s Law a gas will always have a volume of 22.4 L mol at Standard Temperature and Pressure (STP). To determine the volume of 2.3 kg of nitrogen gas we would need to convert the mass of nitrogen to moles and then covert moles to liters at STP. We begin be converting the mass to moles. 2.3 kg of nitrogen is 2300 g.

Why does NO2 undergo dimerisation to form N2O4?

NO2 contains odd number of valence electrons. That valence electron behaves as an odd electron molecule and therefore,undergoes dimerisation to form stable N2O4 molecule with even number of electrons. In NO2, the oxidation state of Nitrogen is +4, hence it always makes an effort to reduce it’s state to +1 or better to 0. Therefore, it combines with

What happens to the unpaired electron in NO2 at low temperature?

The unpaired electron on N in NO2 gets dimeirsed with another NO2 to form N2O4 at low temperature as bond formation takes place with lowering of energy. Since it is exothermic it takes place at low temperature. Why doesn’t NO dimerise while NO2 does?

What is the bond type of nitrogen in N2?

In the nitrogen molecule (N2, which is found in air in the free state), the two nitrogen atoms are bonded by triple-bonds. A double-bond is stronger than a single-bond, and a triple-bond is even stronger than a double-bond.