CHEM 101 Lecture Notes - Lecture 8: Ideal Gas, Ideal Gas Law, Molar Volume

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21 Mar 2016

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Avogodro"s law: volume and amount: experimental observations: Constant temperature and pressure: v1/n1 = v2/n2. Interdependence is perfectly linear (changes in equal proportions) and based on pressure definition: consequence of avogodro"s law: Identical gas volumes contain the same number of molecules when temperature and pressure is the same. The ratio of volumes is the same as the mole ratio from the balanced equation. Avogodro"s law: v/n: stp (standard temperature and pressure) At stp one mole of an ideal gas occupies 22. 414l. = standard molar volume: 1l = 1dm3 = 1000cm3 = 1000ml. Gas mixtures and partial pressures: dalton"s law of partial pressures. The total pressure exerted by a mixture of gases is the sum of the partial pressures of each gas in the mixture. Pa/ptotal = na(rt/v)/ntotal(rt/v) = na/ntotal = xa. Mole fraction -> ration of moles of component to total moles (always some value between 0 and 1) Molecular theory for ideal gases: molecules much smaller than the intermolecular distance.

Related Questions

The ideal gas law (PV=nRT) describes the relationship amongpressure P, volume V, temperature T, and molar amount n. When someof these variables are constant, the ideal gas law can berearranged in different ways to take the following forms where k isa constant: Name Expression Constant Boyle's law PV=nRT=k n and TCharles's law VT=nRP=k n and P Avogadro's law Vn=RTP=k T and P

Part A

A certain amount of chlorine gas was placed inside a cylinderwith a movable piston at one end. The initial volume was 3.00 L andthe initial pressure of chlorine was 1.80atm . The piston waspushed down to change the volume to 1.00 L. Calculate the finalpressure of the gas if the temperature and number of moles ofchlorine remain constant.. (Figure 1) Express your answer with theappropriate units. Pfinal =

Part B

In an air-conditioned room at 19.0 âC, a spherical balloon hadthe diameter of 50.0 cm. When taken outside on a hot summer day,the balloon expanded to 51.0cm in diameter. What was thetemperature outside? Assume that the balloon is a perfect sphereand that the pressure and number of moles of air molecules remainsthe same. Express your answer with the appropriate units. outsidetemperature =

Part C

A cylinder with a movable piston contains 2.00 g of helium, He,at room temperature. More helium was added to the cylinder and thevolume was adjusted so that the gas pressure remained the same. Howmany grams of helium were added to the cylinder if the volume waschanged from 2.00 L to 4.50L ? (The temperature was held constant.)Express your answer with the appropriate units. mass of heliumadded =

Â± Changes in Volume

The ideal gas law (PV=nRT) describes the relationship among pressure P, volume V, temperature T, and molar amount n. When some of these variables are constant, the ideal gas law can be rearranged in different ways to take the following forms where k is a constant:

Name	Expression	Constant
Boyle's law	PV=nRT=k	n and T
Charles's law	VT=nRP=k	n and P
Avogadro's law	Vn=RTP=k	T and P

Part A

A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00 L and the initial pressure of chlorine was 1.15 atm . The piston was pushed down to change the volume to 1.00 L. Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant.. (Figure 1)

Express your answer with the appropriate units.

Pfinal =

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Part B

In an air-conditioned room at 19.0 âC, a spherical balloon had the diameter of 50.0 cm. When taken outside on a hot summer day, the balloon expanded to 51.0 cm in diameter. What was the temperature outside in degrees Celsius? Assume that the balloon is a perfect sphere and that the pressure and number of moles of air molecules remains the same.

Express your answer with the appropriate units.

outside temperature =

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Part C

A cylinder with a movable piston contains 2.00 g of helium, He, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00 L to 4.10 L ? (The temperature was held constant.)

Express your answer with the appropriate units.

mass of helium added =

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The ideal gas law

PV=nRT

relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08206 L?atm/(K?mol) or 8.3145 J/(K?mol). The equation can be rearranged as follows to solve for n:

n=PV/RT

This equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios.

Part A

When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction

CaCO3(s)?CaO(s)+CO2(g)

What is the mass of calcium carbonate needed to produce 29.0L of carbon dioxide at STP?

Part B

Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is

2C4H10(g)+13O2(g)?8CO2(g)+10H2O(l)

At 1.00 atm and 23 ?C, what is the volume of carbon dioxide formed by the combustion of 2.00g of butane?

-Stoichiometric relationships w/ gases-

CHEM 101 Lecture Notes - Lecture 8: Ideal Gas, Ideal Gas Law, Molar Volume

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