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23 Nov 2019

4. A mixture of CS2 (g) and excess O2 (g) is contained in a10.0-liter reaction vessel at 100.0°C; the total
pressure of the mixture is 3.00 atm. A spark causes the CS2 toignite, and it burns completely according to
the following equation: CS2(g) + 3O2(g)?CO2(g) + 2SO2(g)
The vessel and contents are returned to 100°C and the mixture ofproduct gases (CO2, SO2, and unreacted O2) has a total pressure of2.40 atm. Determine the partial pressure of each of these gases inthe final product mixture. (Show all your work)

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Reid Wolff
Reid WolffLv2
15 Oct 2019

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Related questions

Problem 9.128

An empty 4.25 L steel vessel is filled with 1.15 atm of CH4(g) and 4.60 atm of O2(g) at 300 ∘C. A spark causes the CH4 to burn completely, according to the equation:
CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔH∘ = -802kJ

Part A

What mass of CO2(g) is produced in the reaction?

mCO2=4.57

Part B

What is the final temperature inside the vessel after combustion, assuming that the steel vessel has a mass of 12.475 kg , the mixture of gases has an average molar heat capacity of 21J/(mol⋠∘C), and the heat capacity of steel is 0.499J/(g⋠∘C)?

Part C

What is the partial pressure of CO2(g) in the vessel after combustion?
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.

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