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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

### 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

### Applying Ideal Gas Law

A 9.15-L container holds a mixture of two gases at 37 degrees C. The partial pressures of gas A and gas B, respectively, are 0.443 atm and 0.707 atm. If 0.150 mol a third gas is added with no change in volume or temperature, what will the total pressure become?

### Gas laws and examples of how to solve them

This is a review of Boyle's law, Charles's law, Gay-Lussac's law, the combined gas law, and the ideal gas law equations with examples.

### 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

### Volume of oxygen required for the combustion of octane

Combustion Reactions Combustion reactions are classified as rapid reactions that produce a flame. Usually, a combustion reaction refers to the reaction of a substance with O2. A very important class of reactions is the combustion of hydrocarbons (compounds containing hydrogen and oxygen) to form CO2 and H2O. All of the

### 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

### Combined Gas Law and Molarity: Example Questions

Given STP conditions as initial start with 4.00 moles of N2 gas, what is the new temperature with an increase of pressure to 1502 torr and a decrease in volume to 53.5L? a. Calculate molarity of 7.5%(m/v) solution of NaCl? b. How many grams need to be added to make a 7.5%(m/v) solution of NaCl in 694Ml of water?

Consider a vehicle powered by hydrogen gas. a. About 2.7 kg of H2 is required for a vehicle to have a 500 km range. Assume ideal gas behavior and a storage tank of 60 L (a comparable size to conventional gasoline vehicles). What tank pressure( atm) might one expect at 25 degrees celsius? b. Since their discovery in 1991,

### Boyle's Law and Charles's Law

A fixed quantity of gas at 23C degree exhibits a pressure of 735 torr and occupies a volume of 4.32L . Use Boyle's law to calculate the volume the gas will occupy if the pressure is increased to 1.86 atm while the temperature is held constant. Use Charles's law to calculate the volume the gas will occupy if the temperature

### Calculating Kc and Kp of Reverse Reaction

The equilibrium constant Kc for the reaction shown below is 3.8 x 10-5 at 727°C. I2(g) = 2 I(g) Calculate Kc and Kp for the following equilibrium at the same temperature. 2 I(g)= I2(g) Since they give us first rxn Kc do I first take the inverse (to get the Kc for the second rxn)and then figure the Kp? Is this r

### 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

### Mole percent of methane

An evacuated glass bulb has a mass of 27.9214 g. Filled with dry air (80% nitrogen gas, 20% oxygen gas by mass) at 1 atm and 25 degrees Celsius it has a mass of 28.0529 g. Filled with a mixture of methane and ethane it has a mass of 28.0140 g. What is the mole percent of methane in the mixture?

### Pressure from Water Vapor

A 25.0 L stainless steel container was charged with 3.00 atm of hydrogen gas and 4.00 atm of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at a constant temperature of 25°C? atm What is the pressure in the tank, starting with the same pressures of gases, at a constant temperat

### Ideal Gas equation: Increase in air pressure.

A bicycle tire is filled with air to a pressure of 107 psi at a temperature of 19°C. Riding the bike on asphalt on a hot day increases the temperature of the tire to 58°C. The volume of the tire increases by 4.4%. What is the new pressure in the bicycle tire?

### The Molar Mass (g/mole) of the Compound

A white solid has a mass of 3.45 g was vaporized at 148°C in a 517.5 mL container with a pressure reading at the end of the vaporization process of 985 mmHg. What is the molar mass (g/mole) of this compound?

### Finding the Volume of a Balloon

A helium balloon with a volume of 2.4 L contains 0.10 moles of gas at 25 degrees C and 1 atm of pressure. The balloon leaks 0.02 moles of gas until someone manages to seal the hole. What is the new volume of the balloon?

### O2 produced during potassium chlorate decomposition

When heated, potassium chlorate decomposes by the reaction: 2KClO3 --> 2KCl + 3O2 How many liters of O2 gas result when 75.0 grams of KClO3 react at 30.0 degree Celsius and 1.10 atm?

### the factor by that the catalyst speeds up the reaction

The activation energy of an uncatalyzed reaction is Ea^1 = 92 kJ/mol, with a catalyst present it decreases to Ea^2 = 70 kJ/mol. Compute the factor by that the catalyst speeds up the reaction at 306 K: (If the catalyzed reaction were two times faster, the factor would be 2.)

### Under what conditions of temperature and pressure do you think that the gas laws would work best?

Under what conditions of temperature and pressure do you think that the gas laws would work best? Please be specific. ii) What is the total pressure of a gas mixture that contains hydrogen at 0.45 atm, nitrogen at 0.25 atm, and argon at 0.60 atm? iii) How much volume in liters will 100.0 g of oxygen occupy at 100 0C and 1

### Temperatures and Pressures for Gas Laws

I) Under what conditions of temperature and pressure do you think that the gas laws would work best? Please be specific. ii) What is the total pressure of a gas mixture that contains hydrogen at 0.45 atm, nitrogen at 0.25 atm, and argon at 0.60atm? iii) How much volume in liters will 100.0 g of oxygen occupy at 100 0C and

### Evaporation of Methanol

If you place 10.0 L of methanol (CH4O) in a sealed room that is 3 m long, 1.75 m wide, and 2.5 m high, will all the methanol evaporate? If some liquid remains, how much will there be? The vapor pressure of methanol is 127 torr at 25 degrees C, and the density of the liquid at this temperature is 0.791 g/mL.

### 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

### Find the Compound Formula Based on the Molecular Mass

Please show all work, I think all the conversions are messing me up, thanks A 255 mL round bottom flask is weighted and found to have a mass of 114.85g. A few milliliters of an easily vaporized liquid are added to the flask and the flask is immersed in a boiling water bath. All of the liquid vaporizes at the boiling point of

### Gas - A 255 mL round bottom flask is weighted

A 255 mL round bottom flask is weighted and found to have a mass of 114.85g. A few milliliters of an easily vaporized liquid are added to the flask and the flask is immersed in a boiling water bath. All of the liquid vaporizes at the boiling point of water, filling the flask with vapor at 101,325 Pa. When all the liquid has vapo

### Determine Formula

A 255 mL round bottom flask is weighted and found to have a mass of 114.85g. A few milliliters of an easily vaporized liquid are added to the flask and the flask is immersed in a boiling water bath. All of the liquid vaporizes at the boiling point of water, filling the flask with vapor at 101,325 Pa. When all the liquid has vapo

### Determining Oxygen Produced by Decomposition

H2O2(aq) > 2H2 (l) + O2 (g) What volume of O2 (g), collected at 27 degrees celsius and 746 torr, would be generated by decomposition of 125g of a 50% by mass hydrogen peroxide solution? Ignore any water vapor present.

### Volume of H2 Gas

A sample of H2 gas ( 12.28 g) occupies 100.0 L at 400 degree Kelvin and 2.00 atm. A sample weighing 9.49 gram would occupy how many L at 353 Kelvin and 2.00 atm?

### Partial Pressure and Total Pressure

CO (5.0g) and CO2 ( 5.0g) were placed in a 750 mL container at 50 degrees celsius. What was the partial pressure on the CO2 in the container _____atm? What was the total pressure in___atm in the container?

### 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

### Celsius and External Pressure

What is the celsius temperature of 100.0g of chlorine gas in a 40.0L container at 800mm Hg? Calculate the work, w, done on the surroundings when a gas expands from 15L to 35L against a constant external pressure of 1.5 atm.[1L=101J].