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11 Nov 2019

What is atmospheric pressure and what are itâs units?

What does Boyleâs Law relate? Write the formula with units

What is Charlesâs Law? What happens to the temperature if the volume increases?

Write the formula for Avogadroâs law?

What is the ideal gas formula? What are the units

What is the combined gas law?

How can one calculate density of a gas from the ideal gas law?

How can one calculate molar mass of an ideal gas?

What is mole fraction? Dlatonâs Law?

What is the formula for root mean square speed?

Write the formula with units for Grahamâs law of diffusion?

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Related questions

Boyles Law

a) A10.0 L sample of a gas at 25oC and 1.5 atm iscompressed at constant temperature to a volume of 1.0 L. What isthe new pressure?

b) A3.5 L sample of a gas at 1.0 atm is expanded at constanttemperature until the pressure is 0.10atm. What is the volume of the gas?

Charless Law

a) A2.5 L sample of gas at 25oC is heated to50oC at constant pressure. What is the finalvolume?

b) Whattemperature would be required to increase the volume from 2.5 L to6.0 L?

Avogadros Law

a) Assumingno change in temperature and pressure, how many moles of methane(CH₄) need to be added to 0.50 moles of methane todouble the volume?

b) 50g of solid carbon dioxide evaporates to carbon dioxide gas atstandard temperature and pressure. What isthe volume of carbon dioxide gas?

Combined Gas Laws

Calculate the temperature when a 0.50 L sample of gas at 1.0 atmand 25oC is compressed to 0.05 L of gas at 5.0atm.

Ideal Gas Law

a) Whatis the volume of gas occupied by 10.0 g CH4 at37oC and 4 atm?

b) Whatis the mass of N2 required to occupy 5.0 L at80oC and 560 mmHg?

Molar Density of Gases

a) Whatis the density of He at STP?

b) Whatis the density of carbon dioxide at 120^oC and 1.5atm?

Application of Gas Laws:

a) How many grams ofNO₂, nitrogen dioxide, are contained in 0.500 L of thegas at STP?

b) Calculate thedensity of NO₂ gas, in grams per liter, at 110C and 12atm.

c) Calculate the molarmass of a gas if 0.125 g of the gas occupies 93.3 mL at STP.

d) On a spring morning(15C) you fill your tires to a pressure of 2.25 atmospheres. As youride along, the tire heats up to 45C from the friction on the road.What is the pressure in your tires now?

e) What volume ofH₂ is formed at STP when 6.0 g of Al is treated withexcess NaOH?

2NaOH+ 2Al + 6H₂O 2NaAl(OH)₄ +3H₂(g)

Application of Gas Law

a) Whatis the effect on the volume of an ideal gas when the temperature isdecreased from 700K to 350K at constant pressure?

b) Whatis the effect on the volume of an ideal gas when both the pressureand temperature are reduced by half?

c) Whatis the effect on the volume of an ideal gas when the pressure ischanged from 722 torr to 0.950 atm, and the temperature is changedfrom 5^oC to 273 K?

Stoichiometric Relationships

a) Howmany grams of phosphorus react with 35.5 L of O₂ at STPto form tetraphosphorus oxide, according to the following reactionequation?

P₄ (s) + 5 O₂ (g)P₄O₁₀ (s)

b) Ammonia decomposes to nitrogen and hydrogen when in thepresence of heated steel wool. What is thefinal volume of the gas when 45 g of ammonia decomposes at150^oC and 1 atm pressure. Writea balanced equation before you start your calculations!

Daltons Law of Partial Pressures

a) A sample of a natural gas contains 8.24 moles of methane(CH₄), 0.421 mole of ethane(C₂H₆), and 0.116 mole of propane(C₃H₈). If the totalpressure of the gases is 1.37 atm, what are the partial pressuresof the gases?

b) Earths atmosphere consist of 78% N₂and 20%O₂, and other gases. What is the partial pressure ofN₂ and O₂intorr, when the atmospheric pressure is 1 atm?

c) Ammonia is completely decomposed to nitrogen and hydrogen, asin question 9b). At the end of theexperiment the pressure of the gas mixture is 866mmHg. Calculate the partial pressures ofN₂ and H₂.

1) 1.75g of an unknown gas at 31Â°C and 1.05 atm is stores in a 2.55-L flask.

- What is the density of the gas?

______ g/L

- What is the molar mass of the gas?

_____ g/mol

2) If the absolute temperature of a gas is tripled, what happens to the root- mean- square speed of the molecules? (nothing,the new rms speed is 9 times the original rms speed, the new rms speed is 3 times the original rms speed, the new rms speed is 1.732 times the original rms speed, the new rms speed is 1/3 the orginal rms speed)

3) Calculate the average translational kinetic energy (sometimes just called average kinetic energy)...

- for one mole of gas at 723 K.

Ek= ________ J/mol

- for a single gas molecule at 723 K

Ek= ________ J/molecule

4) If He(g) has an average kinetic ebergy of 8890 J/mol inder certain conditions, what is the root mean square speed of F2(g) molecules under the same conditions?

- ___________ m/s

5) Use the van der Waals equation os state to calculate the pressure of 2.70 mol of H2O at 477 K in a 5.10-L vessel.

- P= _________ atm

- use the ideal gas equation to calculate the oressure under the same conditions.

P= _______ atm

1. How many grams of NaCl are required to prepare 500. ml of 1.20M NaCl solution?

2. ) Write the balanced equation for the reaction that occurs when sulfuric acid, H2SO4 is titrated with the base, sodium hydroxide, NaOH. Sodium sulfate, Na2SO4 is the salt produced.

3. SO2 gas is in a 2.0L flask at STP (0 o C, 1 atm).

A. Using the Ideal Gas Law, determine the concentration of the gas in moles/L

B. Calculate the density of the gas in g/L.

4. You burn 150.0g C4H10O in 320.0g O2. The unbalanced equation for the reaction is :

C4H10 + O2 --> CO2 + H2O

A. Balance the equation

B. How many moles of each reactant are you starting with?

C. How many moles of CO2 may actually be produced? Note: determine the limiting reactant?

D. After the reaction is run, it is determined that 220.0g CO2 are actually produced. What is your percent yield?

5. A 1.00M solution of Ba(OH)2 is used to titrate a solution of H3PO4 of unknown concentration. At the end of the titration itâs found that 42.00 ml of Ba(OH)2 and 40.00 ml of H3PO4 were used to reach the endpoint.

The balanced equation for the reaction is: 3Ba(OH)2 + 2H3PO4 --> 6H2O + Ba(PO4)2

A. How many moles of Ba(OH)2 were used?

B. How many moles of H3PO4 are required to react with that much Ba(OH)2?

C. What is the concentration of the H3PO4 in moles/L?

6. GIven the unbalanced equation : PbO2 --> PbO + O2

A. Balance the equation

B. How many liters of O2 gas at 27o C and 1.00 atm can be made from the decomposition of 478.4g PbO2? The molar mass of PbO2 is 239.2g/mole, for O2 itâs 32.00g/mole and for PbO itâs 223.2g/mole. Hint: do the stoichiometry first. Determine how much O2 gas may be produced from 478.4g PbO2. Then determine the volume of the gas.

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