CHE-1102 Lecture Notes - Lecture 2: Aircraft Maintenance Checks, Torr, Ideal Gas Law

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19 Aug 2020

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Gas laws: boyle"s law: pressure and volume are inversely proportional. As pressure increases, volume decrease: equation: p1v1=p2v2, equation: v1n1=v2n2, equation: v1t1=v2t2. Solving calculations: avogadro"s law: volume and number of moles are directly proportional. As volume increases, the number of moles increase: charles" law: volume and temperature are directly proportional. As volume increases, temperature also increases: follow risc, r- read the problem. What is it asking for: i identify the law needed. What equation is needed: s solve for the missing variable, c check proportionality. Example 1: a sample of oxygen gas occupies a volume 2. 97 l at 1. 34 atm. Assume temperature and number of gas molecules present remains unchanged. Example 2: a helium balloon has a volume of 2. 5 ft3 at room temperature. What is the volume of the balloon at 5 of the pressure and number of molecules. A helium balloon contains 1. 25 mol of gas with a volume of 2. 2 l at room temperature and standard pressure.

Related Questions

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 120^oC 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 5^oC 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 at150^oC 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.

WHICH OF THE FOLLOWING IS NOT AN ARRHENIUS BASE? KOH NH3 LiOH Sr(OH)2 Mg(OH)2 WHICH OF THE FOLLOWING IS A STRONG ACID IN AQUEOUS SOLUTION? HC2H3O2 HC1 HC1O2 H2S HC1O WHICH OF THE FOLLOWING REACTIONS IS NOT AN ACID-BASE REACTION? CaO + SiO2 rightarrow CaSiO3 CH3CHO + H2 rightarrow CH3CH2OH PO4^3- + H2O rightarrow HPO4^2- + OH- Na2O + SO3 rightarrow Na2SO4 BF3 + NH3 rightarrow F3BNH3 ALL OF THE FOLLOWING ARE OXIDATION-REDUCTION REACTIONS EXCEPT: H2(G) + F2 rightarrow 2HF(G) Ca(S) + H2(G) rightarrow CAH2(S) 2K(S) + 2H2O(L) rightarrow 2KOH(AQ) H2(G) 6Li(S) + N2(G) rightarrow 2Li3N(S) Mg3N2(S) + 6H2O(L) rightarrow 3Mg(OH)2(S) + 2NH3(G) WHICH OF THE FOLLOWING IS BEST DESCRIBED AS AN OXIDATION-REDUCTION REACTION? SO2(G) + H20(L) rightarrow H2SO3(AQ) 2C1(G) rightarrow C12(G) 3O2(G) rightarrow 2O3(G) 2NO2(G) rightarrow N2O4(G) SO2(G) + O2(G) rightarrow SO3 WHICH OF THE FOLLOWING REACTIONS INVOLVES NEITHER OXIDATION NOR REDUCTION? N2 + 3H2 rightarrow 2NH3 NH4NO2 rightarrow N2 + 2H2O Cu + 2Ag+ rightarrow Cu^2+ + 2Ag 2CrO4^2- + 2H+ rightarrow Cr2O7^2- + H20 C2H4 + H2 rightarrow C2H6 ASSIGN OXIDATION NUMBERS TO EACH ATOM IN NITROUS ACID. H = +1, N=+5, 0=-l H=+l, N=+5, O=-2 H=+l, N=+3, O=-l H=+l, N=+3, O=0 H=+l, N=+3, O=-2 FOR THE REACTION THAT OCCURS IN A LEAD STORAGE BATTERY, Pb(S) + Pb02(S) + 2H+(AQ) + 2HS04-(AQ) rightarrow 2PbSO4(S) + 2H20(L) THE OXIDIZING AGENT IS HSO4- PbSO4 Pb PbO2 H+ IN THE BALANCED EQUATION 3Na+ + 3OH- + P4 + 2H2O rightarrow 3Na+ + 3H2OP2- + PH3 WHAT IS THE REDUCING AGENT? OH- Na+ H2O P4 PH3 ALL OF THE FOLLOWING REACTIONS ARE CALLED COMBINATION REACTIONS EXCEPT BaO(S) + SO2(G) rightarrow BaSO3(S) C6H10(L) + Br2(L) rightarrow C6H10Br2(L) Br2(L) + H20(L) rightarrow HOBr(AQ) + HBr(AQ) CaC12(S) + 6H2O(L) rightarrow CaC12 * 6H2O(S) 3H2(G) + N2(G) rightarrow 2NH3(G) A 12.0 SAMPLE OF NaOH IS DISSOLVED IN WATER, AND THE SOLUTION IS DILUTED TO GIVE A FINAL VOLUME OF 1.80 L. THE MOLARITY OF THE FINAL SOLUTION IS 6.67 M 0.167 M 0.300 M 0.150 M 1.85 M HOW MANY GRAMS OF LITHIUM NITRATE, LiN03 (68.9 G/MOL), ARE REQUIRED TO PREPARE 511.5 mL OF A 0.101 M LiN03 SOLUTION? 0.000750 G 3.56 G 0.281 G 349 G 0.0735 G WHICH SUBSTANCE WOULD PRODUCE 2 MOL OF PARTICLES PER MOLE OF SOLUTE WHEN DISSOLVED IN WATER? NH4CH3COO CH2O CO2 SO2 A1(NO3)3 WHAT MASS OF H3PO4 (98 G/MOL) IS PRESENT IN 59.7 L OF A 0.0438 M SOLUTION OF H3P)4? 0.0267 G 0.00390 G 2.56 Times 10^2 G 1.34 Times 10^5 G 13.9 G WHICH OF THE FOLLOWING IS A CORRECT STATEMENT OF CHARLE'S LAW, V/T = k THE VOLUME OF A GAS VARIES PROPORTIONALLY WITH THE PRESSURE THE VOLUME OF A GAS SAMPLE VARIES DIRECTLY WITH THE ABSOLUTE TEMPERATURE ALL GAS SAMPLES OF THE SAME VOLUME OF STP CONTAIN THE SAME NUMBER OF ATOMS THE PRESSURE OF A GAS SAMPLE VARIES INVERSELY WITH THE VOLUME. ALL GAS SAMPLES OF THE SAME VOLUME AT STP CONTAIN THE SAME NUMBER OF MOLECULES. THE DENSITY OF A GAS IS 3.48 G/L AT STP. WHAT IS ITS MOLAR MASS? 115.7 G/MOL 104.7 G/MOL 6.4 G/MOL 22.4 G/MOL 78.0 G/MOL WHAT VOLUME OF AMMONIA GAS, MEASURED AT 455.9 MM HG AND 57.4 DEG C, IS REQUIRED TO PRODUCE 2.78 G OF AMMONIUM SULFATE ACCORDING TO THE FOLLOWING BALANCED CHEMICAL EQUATION? 2NH3(G) + H2SO4(AQ) rightarrow (NH4)2SO4(S) 0.0002233 L 0.000931 L 0.476 L 7.38 L 1.90 L CALCIUM NITRATE WILL REACT WITH AMMONIUM CHLORIDE AT SLIGHTLY ELEVATED TEMPERATURES, AS REPRESENTED IN THE EQUATION Ca(NO3)2(S) + 2NH4C1(S) rightarrow 2N2O(G) + CaC12(S) + 4H2O(G) WHAT IS THE MAXIMUM VOLUME OF N20 AT STP THAT COULD BE PRODUCED USING A 2.40-MOL SAMPLE OF EACH REACTANT? 6.55 Times 10^2 L 108 L 1.86 Times 10^-2 L 53.8 L 22.4 L WHAT IS THE PARTIAL PRESSURE OF CARBON DIOXIDE IN A CONTAINER THAT CONTAINS 7.64 MOL OF OXYGEN, 1.68 MOL OF NITROGEN, AND 1.42 MOL OF CARBON DIOXIDE WITH A TOTAL PRESSURE OF 529 MM HP? 376 MMHG 80.6 MMHG 82.7 MMHG 69.9 MMHG 529 MMHG A SAMPLE OF HYDROGEN IS COLLECTED BY WATER DISPLACEMENT AT 23.0 DEG C AND AN ATMOSPHERIC PRESSURE OF 735 MMHG. ITS VOLUME IS 568 ML. AFTER WATER VAPOR IS REMOVED, WHAT VOLUME WOULD THE HYDROGEN OCCUPY AT THE SAME CONDITIONS OF PRESSURE AND TEMPERATRE? (THE VAPOR PRESSURE OF WATER AT 23.0 DEG C IS 21 MMHG)509 mL 539 mL 552 mL 568 mL 585 mL

CHE-1102 Lecture Notes - Lecture 2: Aircraft Maintenance Checks, Torr, Ideal Gas Law

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Related Questions

Boyles Law

Charless Law

Combined Gas Laws