Chemistry 1302A/B Chapter Notes - Chapter 1: Ideal Gas Law, Ideal Gas, Inverse Relation

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19 Apr 2017

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States of matter: solid liquid gas (vaporization) Ideal gas law: describes relationship between moles of gas, pressure, volume, and temperate, but o(cid:374)ly t(cid:396)ue u(cid:374)de(cid:396) (cid:862)ideal(cid:863) (cid:272)o(cid:374)ditio(cid:374)s. Pv = nrt: pressure not too high, temperature not close to the condensation temperature, attractive forces come into factor, assume no interaction or volume. Boyle"s la(cid:449: for a fixed amount (# of moles is constant) of gas at fixed temperature. If the volume of a gas sample is increased, then the number of collisions of gas molecules against the wall decreases. Cha(cid:396)les"s la(cid:449: for a fixed amount of gas at fixed pressure. V1/t1 = v2/t2: no, you cannot maintain the pressure of a gas (1 mole) sample and increase the temperature in a fixed container. If you heat the container, the pressure will increase until the container cannot take it anymore (explosion). Co(cid:373)(cid:271)i(cid:374)i(cid:374)g cha(cid:396)les"s a(cid:374)d boyle"s la(cid:449)s: p x v / t = constant, p1v1 / t1 = p2v2 / t2.

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 =

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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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Chemistry 1302A/B Chapter Notes - Chapter 1: Ideal Gas Law, Ideal Gas, Inverse Relation

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