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A gas at 250 K and 15 atm has a molar volume 12% smaller thanthat calculated from the ideal gas law. Calculate the molar volumeand compression factor of the gas. Are attractive or repulsionforces dominating?



B) Which gas would be most non-ideal (largest values of Van DerWaal's coefficients) at 350K? Neon, Ethane, or Acetone?

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Related questions

The molar volume of the gas calculated from ideal gas equationis 12 % larger than measured experimentally at 250 K and 15 atm.Calculate (a) the compressibility factor (Z) under these conditionsand (b) the molar volume of the gas. Which are dominating in thesample, the attractive or the repulsive forces?

(consider implicit solution)

The van der Waals equation of state (Equation 5.3-7) is to be used to estimate the specific molar volume V̂ (L/mol) of air at specified values of T (K) and P (atm). The van der Waals constants for air are a = 1.33 atm  L2/mol2 and b = 0.0366 L/mol.

a) Show why the wan der Walls equation is classified as a cubic equation of state by expressing it in the form:

f(V̂)=c3V̂3+c2V̂2+c1V̂ +c0=0

where the coefficients c3, c2, c1, and c0 involve P, R, T, a, and b. Calculate the values of these coefficients for air at 223 K and 50.0 atm. (Include the units when giving the values.)

b) What would the value of V̂ be if the ideal-gas equation of state were used for the calculation? Use this value as an initial estimate of V̂ for air at 223 K and 50.0 atm and solve the wan der Waals equation using Goal Seek or Solver in Excel. What percentage error results from the use of the ideal-gas equation of state, taking the van der Waals estimate to be correct?

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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