For each of the quantities listed below, explain which of the following properties (mass of the molecule, density of the gas sample, temperature of the gas sample, size of the molecule, and number of moles of gas) must be known to calculate the quantity. average number of collisions per second with other gas molecules

For each of the quantities listed below, explain which of the following properties (mass of the molecule, density of the gas sample, temperature of the gas sample, size of the molecule, and number of moles of gas) must be known to calculate the quantity. average force of each impact with the wall of the container

For each of the quantities listed below, explain which of the following properties (mass of the molecule, density of the gas sample, temperature of the gas sample, size of the molecule, and number of moles of gas) must be known to calculate the quantity. distance between collisions

You have two containers each with 1 mole of xenon gas at $15^{\circ} \mathrm{C}.$ Container A has a volume of 3.0 L, and container B has a volume of 1.0 L. Explain how the following quantities compare between the two containers. the pressure of the Xe sample

Graph each function in over the indicated interval. $N=\frac{200}{1+3 e^{-t}} ;[0,5]$

You have two containers each with 1 mole of xenon gas at 15$^{\circ}$C. Container A has a volume of 3.0 L, and container B has a volume of 1.0 L. Explain how the gas density compare between the two containers.

Consider two gases, A and B, each in a 1.0−L container with both gases at the same temperature and pressure. The mass of gas A in the container is 0.34 g, and the mass of gas B in the container is 0.48 g. Which gas sample has the largest average kinetic energy? Explain.

You have two containers each with 1 mole of xenon gas at 15$^{\circ}$C. Container A has a volume of 3.0 L, and container B has a volume of 1.0 L. Explain how the collision frequency of the Xe atoms (with other atoms) compare between the two containers.

You have two containers each with 1 mole of xenon gas at 15$^{\circ}$C. Container A has a volume of 3.0 L, and container B has a volume of 1.0 L. Explain how the root mean square velocity of the Xe atoms compare between the two containers.

You have two containers each with 1 mole of xenon gas at 15$^{\circ}$C. Container A has a volume of 3.0 L, and container B has a volume of 1.0 L. Explain how the pressure of the Xe sample compare between the two containers.

You have two containers each with 1 mole of xenon gas at $15 ^ { \circ } \mathrm { C }.$ Container A has a volume of 3.0 L, and container B has a volume of 1.0 L. Explain how the following quantities compare between the two containers. a. the average kinetic energy of the Xe atoms, b. the force with which the Xe atoms collide with the container walls, c. the root mean square velocity of the Xe atoms, d. the collision frequency of the Xe atoms (with other atoms), e. the pressure of the Xe sample.

For each of the quantities listed below, explain which of the following properties (mass of the molecule, density of the gas sample, temperature of the gas sample, size of the molecule, and number of moles of gas) must be known to calculate the quantity. average number of collisions with a given area of the container

Explain the following seeming contradiction: You have two gases, A and B, in two separate containers of equal volume and at equal pressure and temperature. Therefore, you must have the same number of moles of each gas. Because the two temperatures are equal, the average kinetic energies of the two samples are equal. Therefore, since the energy of such a system corresponds to translational motion, the root mean square velocities of the two are equal, and thus the particles in each sample move, on average, with the same relative speed. Since A and B are different gases, each must have a different molar mass. If A has a higher molar mass than B, the particles of A must be hitting the sides of the container with more force. Thus the pressure in the container of gas A must be higher than that in the container with gas B. However, one of our initial assumptions was that the pressures were equal. Explain.

How does Dalton’s law of partial pressures help us with our model of ideal gases? That is, what postulates of the kinetic molecular theory does it support?