Flipbook

Gasses Flipbook

Basic guide to create an awesome presentation

Properties of Gas

4 quantaties are needed to define the state of gas: the quantity (In Moles), the temperature (In Kelvin), the volume,(In Liters) and the pressure of the gas (In Atmospheres). A gas fills any container, is easily compressed and mixes with any gas. The Kinetic Molecular Theory neglects intermolecular forces , while gasses fill their container and are compressible solids and and liquids do not do this easily. Gas Pressure is a measure of the forces that a gas exerts on an container and is measured by a barometer. 1.00 atm = 760.00 mm Hg = 760.00 torr = 29.92 in Hg = 14.7 psi = 101.325 kPa = 10 Pa

Ideal Gas Law

Ideal gases exist in only in ideal conditions: low pressure and high temperature, obey the KMT at all times, doesnt take up volume, has no effect on each other. However, in the real world no gas is truly ideal. The Ideal Gas law: one gas at a set of of conditions that permits you to solve for a number of moles of a contained mass given only on value for each (P, V, or T). (PV=nRT) Ideal Gas Constant= 0.0821 L * atm/mol * k. 62.4 L * lmttg/mol * k, 8.314 L * KPA/ mol * k.

Experimental Gas law

P1V1=P2V2 is one of the easiest of Boyle's laws to memorize. Boyle's Law has been tested fir years but only holds true in low pressures. EX: [ (5.6 * 10^3 Pa)(1.53L)/1.5 * 10^4 Pa] = (1.5 *10^+PA)V2/1.5*10^4Pa = (V2=0.57L) V1T2=V2T1 (The formula for Temerature of Volume for at constantly) (V1/T1=V2/T2[Stay the Same]) Absolute Motion= -273.15 (All KE Motion) 2.58 L/288 K = V2/311 K (2.58 L)(311K)=V2(288K) = (V2=2.79 L) P1T2=P2T1 plot = straight line P1/T1 = P2/T2 Avagrado's Hypothesis: All gasses under the exact same conditions will have the exact same moles. Combined Gas Law: P1V1/n1T1 = P2V2/n2T2

Combined Gas Law

This law combines they previous laws of Boyle, Charles, and Gay-Lussac and can be used to find the equations for all the other laws. The Equation is: P1V1/T1N1=P2V2/T2N2 EX: An Unknown Pressure occupies 0.766 L at a temperature of 298 K was tested under unknown conditions and then has a Pressure of 32.6 kPa, occupies 0.644 L at 303 K. V1- 0.776L V2- 0.644 L T1- 298 K T2- 303 K P1- ? P2- 32.6 kPa P1(0.766 L)/298 K = (32.6 kPa)(0.644 L)/303 K -----> P1(0.766 L)(303 K)/(0.766 L)(303 K) = (298 K) (32.6 kPa) (0.644 L)/(0.766 L) (303 K) = (P1 = 27.0 kPa)

Practice Problems

a) A fixed volume steel tank holds 50.0 L of oxygen gas at 10.0oC and 2.0 atm. What will the pressure in the tank be if it is moved to a room that has a temperature of 25.0oC? b) A helium filled weather balloon has a volume of 25.0 L at 23.0oC and 0.963 atm when it is released from the weather station. In the upper atmosphere at a location where the pressure is 0.584 atm, the balloon increases to 34.7 L. What is the Celsius temperature of the balloon at the higher altitude? c) In a double replacement reaction, 5.00 moles of water vapor are produced at 760 mmHg and 300 K. What volume of water will be collected? d) A cylinder is filled to a volume of 3.50 L at 760 mmHg with chlorine gas. What is the volume if the pressure is changed to 50.0 kPa? e) How many moles argon gas are found when 2.3 L are isolated from a sample of air at STP? How many grams of argon are in the container? f) A gas originally occupies an unknown volume at 27 oC. It currently occupies 40.0 mL at -123oC. What was the original volume? g) Using dimensional analysis: Convert 23 kPa to mmHg and then to atmospheres. h) Covert 100 K to Celsius. Convert 100 oC to Kelvin. i) Using dimensional analysis: Convert 150 mL to liters. Convert 3.00 L to mL. j) At STP, a sample of methane gas (CH4) is combusted to produce 1.2 L carbon dioxide. What volume of oxygen was required for the reaction to occur?