CHM 1311 Lecture Notes - Lecture 7: Ideal Gas, Molar Concentration, Molar Volume

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29 Sep 2016

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Gases have three characteristics we need use in any theory of gases: Uniformly fill any container, mix completely with any other gas, exert pressure on its surroundings. Pressure pressure = force/area standard atmospheric pressure = 1 bar. Gas can be characterized by volume (v), temperature (t), and amount (n), but is highly sensitive to pressure (p) Units of pressure: standard atmosphere (atm) is the pressure that will support a column of mercury. 760mm in height unit of mm hg, aka torr. 1 bar = 100 kpa (kilopascal) = 100 000 n/m2 = 750. 06 torr. 1 atm = 1. 01326 bar = 101 325 pa (101. 325kpa) = 760 torr. 1 torr = 1mm hg = 133. 3 pa. Atmospheric pressure pushes down on mercury causing it to rise from 760mm. P gas > p atm + phg (in the bulb version) Variations in gas volume volume changes with conditions (based on kelvin for temp) Boyle - increase pressure = decrease in volume.

Related Questions

Question 11 pts

Which general statement about gases is NOT correct?

The molecules of a pure gas are distributed evenly throughout the container.

Gases are much less dense than liquids or solids

Molecules in a gas mixture can form layers according to their densities

Gases can be compressed, even to the point of liquefaction

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Question 21 pts

Which example is the greatest pressure?

1.00 atm

101 kPa

760 mm Hg (= 760 torr)

All of the above pressures are equal.

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Question 31 pts

Which example is the greatest pressure?

850 mm Hg (= 850 torr)

1.5 atm

All of the above pressures are equal.

96 kPa

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Question 41 pts

Assuming all other variables are held constant, a graph of which of the following will NOT yield a straight line?

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Question 51 pts

A sealed vessel contains 0.250 mol of oxygen gas. Which of the following will result in a decrease in the pressure of the oxygen gas?

increasing the number of moles of oxygen

increasing the temperature of the vessel

increasing the volume of the vessel

adding some helium to the vessel

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Question 61 pts

According to Charlesâs law, which change will cause the pressure of a gas to double? Pressure and amount of gas are constant.

The temperature decreases from 650 K to 325 K.

The temperature of the sample decreases fromï¿½88 Â°C to 44 Â°C.

The temperature of the sample increases fromï¿½22 Â°C to 44 Â°C.

The temperature of the sample increases fromï¿½250 K to 500 K.

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Question 71 pts

Which set of units for P, V, and T can be used for combined gas law calculations?

torr, L, and Kelvins

tm, g/L, and Kelvins

atm, mL, and degrees Celsius

inches of mercury, g/mL, and degrees Celsius

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Question 81 pts

The vapor pressure of a gas is

the atmospheric pressure at which the boiling point is determined.

the pressure at a Kelvin temperature exactly two times the boiling point.

impossible to determine experimentally without knowing the temperature and volume.

the pressure above a gas sample when evaporation and condensation are balanced.

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Question 91 pts

In a chemistry experiment where CO2 is collected over water, the atmospheric pressure is 755 mm. The partial pressure of water at the temperature in the lab is 24.2 mm. What is the pressure of the CO2?

779 mm

731 mm

More information is needed to answer this question

755 mm

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Question 101 pts

Which statement is NOT true according to the kinetic molecular theory of gases?

Molecules undergo elastic collisions

Molecules move in straight-line paths.

Molecules of different gases have differentï¿½kinetic energies at the same temperature

Molecules occupy a negligible volume.

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