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# Gas Laws

### Ideal Gas Law of Hydrogen

How do I determine liters of hydrogen gas collected over water at 18 C and 725 mmHg when 0.79 g lithium reacts with water? (Aqueous lithium hydroxide also forms).

### (MM) of a volatile liquid using th ideal gas law (PV=nRT) in the following form:

(MM) of a volatile liquid using th 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 275 ml, the pressure is 775 torr., calculate the following: 1. The density of the vapo

### 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?

### Grams of oxygen are required to fill a chamber

How many grams of oxygen are required to fill a 3.00 x 10 to the 3rd power, liter chamber at a pressure of 250 cm Hg and 68 degree F? If the same quantity of oxygen was pumped back into a gas cylinder at a pressure of 200atm. and at 75K, what would be the volume be?

### 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

### Final volume of the helium balloon

A balloon of helium whose volume is 2.20 L at 25 degrees C is cooled by pouring liquid N2 over it. The final temperature of the balloon is -196 C. What is the final volume, in L? A. 0.57 B. 8.5 C. -17 D. 0.28 E. 2.2

### Molecules

How many molecules are present in 475 mL of CO2 at STP? a. 2.86 x 10 to the power of 23 molecules of CO2 b. 0.0212 molecules of CO2 c. 6.50 x 10 to the power of 21 molecules of CO2 d. 1.28 x 10 to the power of 22 molecules of CO2 e. 1.28 x 10 to the power of 25 molecules of CO2

### Temperature of Gas in Kelvin

A sample of gas occupies 234 mL at 3.56 atm and 79.0 degrees C. The volume change to 438 mL and the pressure is changed to 2.92 atm. What is the new temperature in Kelvin? A. 28.0 B. 0.00824 C. 541 D. -273 E. 0.00436

### Total Pressure of the Helium and Oxygen Mixture

Mixtures of helium and oxygen are used in scuba diving. What is the total pressure of a mixture of 1.96 g He and 6.08 g O2 confined in a 5-L tank at 25 C? A. 0.279 atm B. 4.26 atm C. 39.3 atm D. 16.6 atm E. 3.33 atm

### Partial Pressure of Oxygen Gas

What is the partial pressure of oxygen gas produced if 8.42 g of hydrogen peroxide decomposes at 22 degrees C into a container with a fixed volume of 3.78 L (assuming no oxygen is initially present)? 2H2O2 --> 2 H2O +O2

### 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

### Problem involving the application of ideal gas law

Mole and Mass relationship in chemical equation: 1. What mass of ammonia, in grams, can be made from 440g of H2? N2+3H2-2NH3 The combined Gas Law: 1.If the gas present in 4.65L at STP is changed to a temperature of 15C and pressure of 756mmHg, what will be new volume? The Ideal Gas Law: 1. Calculate the

### 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

### It is found that 250 ml of gas at STP has a 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. Calculate the numbe

### 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

### Limiting reactant, application of ideal gas equation, mole

See the attachment.

### Application of ideal gas equation, mole and mass calculation.

See the attachment. 6. In the reaction of copper with concentrated nitric acid, the products are copper (II) nitrate, water and nitrogen monoxide, sometimes called nitric oxide. If 150 ml of nitric oxide were collected over mercury at 42C and under a pressure of 74.5 cm of mercury, how many grams of copper had reacted?

### Solubility, Molar conc., Molarity, Application of ideal gas equation.

3. The solubility of laughing gas, dinitrogen monoxide, in water is 7.50 mg per cent by mass at 760 Torr and 25C. If the density of the resulting solution is 1.01 grams per milliliter, what is the morality of the resulting solution? What is the % of the volume?

### Partial pressure, pressure conversion, application of ideal gas

Any number of green plants can photosynthesize glucose (C6H12O6) in the presence of carbon dioxide and water, and producing oxygen as the remaining product. 250 ml of oxygen was produced. The oxygen was collected over water at 27C and at a pressure of 755 Torr. The vapor pressure of water at 27C is approximately 26mm Hg. What

### Pressure conversion, mole, use of ideal gas equation

1. How many grams of oxygen are required to fill a 4.5 x 103 liter hyperbaric chamber at a pressure of 225 cm Hg and 62 F?

### Ideal gas equation, moles and temperature conversion

Ideal gas equation, mole, temperature conversion, pressure conversion, % weight.

### Production of ethyne, ideal gas equation application

Production of ethyne, ideal gas equation's application, Temperature conversion: Celcius to Kelvin, Pressure conversion: mm Hg to Pascal, mole and volume calculation.

### 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)