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CHE-1102 Study Guide - Quiz Guide: Hydrogen Cyanide, Sulfur Oxide, Mole Fraction

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School
App State
Department
Chemistry
Course
CHE-1102
Professor
Jennifer Cecile

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Document Summary

The states of matter are solid, liquid, and gas. Temperature and volume affect the spontaneity of gas. Gases have no definite shape of volume, so they expand to fill their containers. Common gases include hydrogen cyanide (hcn), hydrogen sulfide (h2s), carbon monoxide (co), carbon dioxide (co2), methane (ch4), ethene (c2h4), propane (c3h8), nitrous oxide (n2o), nitrogen dioxide (no2), ammonia (nh3), and sulfur oxide (so4). The variables that affect gas include volume, the number of moles of the gas, the temperature, and the pressure applied to the gas. Temperature is measured in kelvin for all use kelvin for all calculations involving gases. Absolute zero is -273. 15 and standard temperature is 0 , which can also be shown as. Pressure is the force placed onto something and it is calculated by p=forcearea . Atmospheric pressure is the pressure of the air calculated by dividing the weight of air by the area. Pressure is measured in mm hg, torr, or atm.

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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 120oC 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 5oC 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 at150oC 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.

All volume answers should be in the units of Pascals or kiloPascals, all volumes should be in Liters, all temperatures should be in Kelvin, all masses in grams, all densities in g/L, molar masses in g/mol, etc.

1) If I have 5.6 L of a gas in a piston with a pressure of 1.5 atm and compress the gas to 4.8 L, what is the new piston pressure?

2) I have 15 L of air in a balloon at sea level. If I take it to Denver where the air pressure is 85% of sea level, what volume will the air in the balloon take?

3) I have a car with an internal volume of 12000 L. If it goes underwater, it will implode because the air pressure will change from 1.0 atm to 1.4 atm. What would the new volume of the air in the car be?

6) If I have 45 L of helium at 25 °C and increase the temperature to 55 °C what is the new volume?

7) Calcium carbonate decomposes at 1200 °C to form carbon dioxide and calcium oxide. If you collect 25 L of carbon dioxide at 1200 °C, what is the volume of this gas at 25°C.

11) The gas in a can of hairspray has a temp of 27 °C and 30 lbs/in2 of pressure. If the gas reaches a pressure of 90 lbs/in2 the can will explode. What temperature would make that happen?

16) 500 mL of gas at STP. The volume increased to 560 mL and 20 °C, what is the pressure?

17) 400 mL of a gas at 300 mmHg and 0 °C is increased to 10 °C and 140 mmHg, what is the new volume?

18) A balloon has a pressure of 1.05 atm and 5.0 L. If the balloon is released at 20.0 °C but rises to a pressure of 0.65 atm and -15 °C, what is the new volume?

21) What is the partial pressure of carbon dioxide in a container of 5 moles of carbon dioxide, 3 moles of nitrogen gas, and 1 mole of hydrogen gas with a total pressure of 1.05 atm.

26) If neon travels at 400 m/s, what is the velocity of C4H10 at the same temperature?

27) Hydrogen sulfide smells of rotten eggs. C8H8O3 smells of wintergreen. C7H6O smells of almonds. If they are mixed into a container and the container is opened across the room from you, which smell will hit you first?

31) A 50 L container holds 45 moles at 200 °C. What is the pressure?

32) If a 1 L canister holds 2 moles of gas and is thrown into a 1400 °C fire, what is the new pressure in the canister?

36) Calcium carbonate degrades to form carbon dioxide and calcium oxide. How many grams of calcium carbonate are needed to form 3.45 L of carbon dioxide?

37) How many liters of water vapor are formed by combusting 1.25 L of ethene?

41) A gas has a density of 0.53 g/L at 225 K and 108.8 kPa. What is the density at 345 K and 68.3 kPa?

42) 250 mL of a gas at STP weighs 0.291 grams. The composition of the gas is 92.24 % carbon, and 7.76 % hydrogen. What is the gas?

45) The average molar mass of the gases on Titan (a moon of Saturn) is 28.6 g/mol and rests at 95 K and 1.6 atm. What is the density of the gases of Titan?