In the kinetic theory of gases, explain the concept of the velocity distribution function of particles in space.

Methanol, CH3OH, is produced industrially by the following reaction: CO(g)+2H2(g)coppercatalyst300C,300atmCH3OH(g) Assuming that the gases behave as ideal gases, find the ratio of the total volume of the reactants to the final volume.

The graph below shows the probability of molecular velocities for sulfur hexafluoride gas (SF6) at some fixed temperature.  Use the data to determine the temperature of the SF6 gas in degrees Celsius.

7. The average kinetic energy of the molecules of an ideal gas is directly proportional to the (1) number of moles present (2) volume occupied by individual gas molecules (3) temperature measured on the Kelvin scale (4) pressure at standard temperature

if .500 moles of zinc metal completely react with hydrochloric acid, how many liters of hydrogen gas will be made at standard temperature and pressure? (273 kelvin and 1.0atm

This relationship is known as Graham’s Law of Effusion. Since both gases are at the same temperature, they must have the same average kinetic energy (½ mv2), where m is mass and v is velocity (like speed). Since both gases have the same average kinetic energy, you can state that ½ mLvL2 = ½ mHvH2. Multiplying both sides by 2 gives you mLvL2 = mHvH2. Rearranging the equation to get both masses on the same side of the equation will give you mL/mH = VH2/VL2. In 3a and 3b, you probably noticed that the heavy gas particles took twice as long to diffuse as the light gas particles. This means that the light gas particles are moving twice as fast, VH/VL = ½. Therefore, VH2/VL2 = ¼. If the light gas was Ne, what would be a reasonable identity for the heavy gas? Explain.

One of the assumptions of the KMT of gases is that the particles have negligible volume. Is this assumption valid or invalid for a real gas?

The kinetic molecular theory assumes that the particles of an ideal gas...

Carbon dioxide molecules have an average speed of 25.0 m/s at a given temperature and pressure. What is the average speed of carbon monoxide molecules at the same condition.

The graph below shows the probability of molecular velocities for sulfur hexafluoride gas (SF6) at some fixed temperature.  Use the data to determine the temperature of the SF6 gas in degrees Celsius.