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Gas Laws

Gas Laws describe the behavior of gases through examining the relationships between their physical properties. Despite the wide differences in chemical properties of all gases, they more or less obey the gas laws. For example, although both H2 and O2 are very different gases, with molecular weights of 2 g/mol and 32 g/mol respectively, they will behave similarly to a change in any physical property.

Gas is one of the four fundamental states of matter, found between the liquid and plasma states, where their particles are widely separated and have very weak intermolecular bonds between the atoms. Gases are the only states of matter that can be compressed or even expand to fill a very large space. It is these properties which makes them subject to behave differently with respect to changing physical properties such as pressure, volume, temperature and amount.

The main gas laws include Avogadro’s Law, Boyle’s Law, Charles’ Law, Fick’s Law of Diffusion, Gay-Lussac’s Law and Henry’s Law. All of these examining the relationship between physical properties to help predict the overall behavior of that gas. Thus, understanding the gas laws and when to apply them is crucial to help predict how a gas will react to varying conditions.

Categories within Gas Laws

Avogadro’s Law

Postings: 2

Avogadro’s Law describes the relationship between the volume of gas and the amount of gas present.

Boyle’s Law

Postings: 7

Boyle’s Law describes the relationship between the change in pressure and volume of a gas.

Charles’ Law

Postings: 3

Charles’ Law describes the relationship between the change in volume and the temperature of a gas.

Fick’s Law of Diffusion

Postings: 2

Fick’s Law of Diffusion relates diffusion flux to the diffusion coefficient, change in concentration and change in position.

Henry’s Law

Postings: 7

Henry’s Law describes the relationship of the solubility of a gas in a liquid and the partial pressure of that gas when it is in equilibrium with the liquid.

Heat Of Formation & Gas Laws

Please solve and show all calculations. 1. An ideal gas at 300K and 2.00 atm pressure in a 400 cm^3 container has its pressure increased to 5.00 atm and its volume increased to 6000 cm^3. What is the final temperature? 2. The vapor pressure of water at 23 degrees celcius is 21.07 torr. Find the vapor pressure at 23 degre

Gas Laws Experiment

Hi, Based on your Chemistry knowledge, please estimate the temperatures, plug them on the data table on the last page and answers the other questions. Thank you for the help! Gas Laws Under ordinary conditions of pressure and temperature, matter exists in either the solid liquid or gaseous state. In a solid, the pa

Molar Volume of an Ideal Gas

Add 0.25g of zinc to the Erlenmeyer flask and close the flask with an air-tight stopper. Take a thermometer and pressure gauge and record the initial temperature and pressure.(my answer: 21C, 1 atm). Add 10 mL of 6M HCl solution to the flask. Record all of the indications that the reaction has occurred (my answer: temperature

Decomposition of NaHCO3

At 125°C, Kp = 0.25 for the following reaction. 2 NaHCO3(s)<---> Na2CO3(s) + CO2(g) + H2O(g) A 1.00 L flask containing 11.1 g NaHCO3 is evacuated and heated to 125°C. (a) Calculate the partial pressures of CO2 and H2O after equilibrium is established. PCO2 atm PH2O atm (b) Calculate the masses of NaHCO3 a

application of ideal gas law

Convert the following pressure into atmospheres. 781 torr 781 mm Hg A 1.04-L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.24 L. What will be the pressure in the expnaded gas sample at a constant temperature. At conditions of constant temperature and pressure, the volume of a sample of ideal gas i

General Chemistry

(Problem 1) A person accidentally swallows a drop of liquid oxygen, O2(l), which has a density of 1.149 g/mL. Assuming the drop has a volume of 0.050 mL, what volume of gas will be produced in the person's stomach at body temperature (37 C) and a pressure of 1.0 atm? (Problem 2 ) The density of N2O at 1.53 atm and 45.2 degree

Volume of a Balloon

Weather balloon is filled with 4.0 liters of helium at 27 degree C and 1.0atm. What volume does the balloon have when it has risen to a point in the atmosphere where the pressure is 200 Torr and the temperature is minus -45 degree C?

The Apparent Molecular Weight of Air

1. Record your data table of temperature vs. volume here. 2. Construct a graph by hand or using a spreadsheet program, plotting the values of temperature on the x-axis and air volume on the y-axis. Initial temp. 21 Deg C, Vol. 100mL Ice -3 Deg C, Vol. 91.84mL Water 100 deg. C, Vol. 126.87mL Gas Piston Removed: Temp. Deg

Chemistry Questions

1. Chlorine gas occupies a volume of 1.20 liters at 725 torr pressure. What volume will it occupy at 1 atm pressure? 2. Fluorine gas exerts a pressure of 975 torr. When the pressure is changed to 1.50 atm, its volume is 250 mL. What was the original volume? 3. Helium occupies a volume of 3.80 Liters at -45 &#61616;C. Wh

Density of an Ideal Gas

A gas mixture was found to have a density of 0.26 g/L at 20 C and 0.245 atm. What was the average molar mass of the molecules?

Gas Laws

1. A diver at a depth of 100 ft (pressure approximately 3 atm) exhales a small bubble of air with a volume equal to 100 mL. What will be the volume of the bubble (assume the same amount of air) at the surface? 2. What would the volume of gas contained in an expandable 1.0 L cylinder at 15 MPa (1MPa = 10^6 Pa) be at 1 atm (assum

Pressure Before & After

One mole of argon gas inside a cylinder fitted with a piston is made to expand very slowly in good thermal contact with its surroundings. During this expansion the volume was doubled and the temperature was constant. The same expansion is performed very rapidly with the cylinder being thermal isolated. The conditions were contro

Final gas pressure

A sample of ammonia gas with a volume of 7.0 mL at a pressure of 1.68 atm is compressed to a final volume of 2.7 mL at constant temperature. Use the ideal gas law to calculate the final pressure. a. 100 atm b. 2.2 atm c. 1 atm d. 4.4 atm

Molar mass

It is found that 250 ml of gas at STP has a mass of 1.00 gram. What is the molar mass? a. 89.6 gram/mol b. 28.0 gram/mol c. 14.0 gram/mol d. 22.4 gram/mol

Gas and Stoichiometry with Avogadro and Dalton's

Please show all work. 1.)(Ideal Gas Law) How many moles of chlorine atoms are there in a container that holds 1.529 kg of XCl5 gas (where X = unknown element) at 600.5°C at a pressure of 1213 torr? The density of the gas is 4.63 g/L. 2.) (Ideal Gas Law) A chemist carries out a reaction and isolates a gaseous product.

The law of Charles & Gay-Lussac

We wish to double the volume of a gas held at constant pressure. To what temperature must we heat it if its original temperature was (a) 0^oC, (b) 100^oC, and (c) 1000^oC? I believe the answer is a) 546 K, b) 746 K and c) 2546 K. I need to see each step and formula to solve this question.

Nitrogen gas pressure problem

A nitrogen container has 100.0 liters of gas at a pressure of 3200 psi ruptures in a room at 28° C and 0.92 atm pressure. What volume will the nitrogen gas occupy in the room after the bottle empties? Please show all steps. 2 A typical vacuum system can obtain a pressure of 1.0 x 10-8 (-8 power) torr. Cal

Finding the volume, PV = nRT

1.86 moles of a gas occupies 245L at 281 degrees C with a pressure of 0.63 ATM. The pressure is increased to 886 ATM with the same temp. What is the volume?

Molar mass and density

In most general chemistry courses, students calculate the molar mass (MM) of a volatile liquid using the ideal gas law (PV = nRT) in the following form: MM = (mass of vapor*R*boiling point in Kelvins)/(pressure in atmospheres*flask volume). If R = 0.0821 liter-atmospheres/mole-degree K, the flask volume is 550 ml, the pressure i

Molecular Mass Calculation

The density of benzene vapor at 100 C* and 650 mmHg is 2.18g/L. Calculate the molecular mass. (Hint D=n(mol. Weight)/vol.=P(mol. Weight)/RT)

Total Volume of Gas Collected

Potassium chlorate, KClO3, decomposes when heated: KClO3 (s) ® KCl (s) + 3/2 O2 (g) 1.00 gram of potassium chlorate is completely decomposed and the oxygen is collected over water at 25°C and 0.99 atm. Calculate the total volume of gas collected. (The vapor pressure of water at 25°C is 23.8 torr).