CHEM 130 Chapter Notes - Chapter 5: Mole Fraction, Address Plus Port, Caffeine

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27 Jan 2015

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Avogadro"s law : vm=specific constant (22. 4 l/mol at stp) (depending on t and p but independent of the gas) Ideal gas law: pv=nrt (p pressure, v volume, n moles of gas molecule, r constant, t temperature) Gas density: pmm=drt (p pressure, mm molar mass, d density of gas, r constant, t temperature) Stp: standard temperature and pressure: 0 c and 1 atm (760 mmhg). To use gas laws, temperature also convert to k. whenever you see temperature, change it to. Types of problems: one gas one condition. [example 1] given the following chemical equation, what is the density of ammonia (in g/l) at. Strategy: (1) write down the equations pv=nrt and pmm=drt (2) find the unknown you want to solve, and the information you are given, to choose which equation you will use: Here you are asking to solve density (d) and are given p, t and mm (since you know ammonia is.

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The ideal gas law relates the pressure P, volume V, absolutetemperature T, and amount of gas n. The law is P = nRT/V where R isthe gas constant.

An engineer must design a large natural gas storage tank to beexpandable to maintain the pressure constant at 2.2 atm. InDecember when the temperature is 4 degrees Farenheight (-15 C), thevolume of gas in the tank is 28,500 ft^3. What will the volume ofthe same quantity of gas be in July when the temperature is 88 F(31 C)? (Hint: Use the fact that n, R, and P are constant in theproblem. Note also that K = C + 273.2

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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

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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 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 =

CHEM 130 Chapter Notes - Chapter 5: Mole Fraction, Address Plus Port, Caffeine

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