Ideal Gas Law & Gas Stoichiometry. Avogadro’s Principle Equal volumes of gases contain equal numbers of moles at constant temp & pressure true for any.

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Presentation transcript:

Ideal Gas Law & Gas Stoichiometry

Avogadro’s Principle Equal volumes of gases contain equal numbers of moles at constant temp & pressure true for any gas V n

I. Ideal Gas Law Merge the Combined Gas Law with Avogadro’s Principle: PV nT = R UNIVERSAL GAS CONSTANT R= L  atm/mol  K R=8.315 dm 3  kPa/mol  K

Equation: PV = nRT New variables: n = AMOUNT of gas in MOLES R = UNIVERSAL GAS CONSTANT * PROPORTIONALLY constant * value depends on UNITS used for PRESSURE and VOLUME * value of R when using kPa and L R = L. kPa / Mol. K Ideal Gas Law

GIVEN: P = ? atm n = mol T = 16°C = 289 K V = 3.25 L R = L  atm/mol  K WORK: PV = nRT P(3.25)=(0.412)(0.0821)(289) L mol L  atm/mol  K K P = 3.01 atm  Calculate the pressure in atmospheres of mol of He at 16°C & occupying 3.25 L. Ideal Gas Law Problem

GIVEN: V = ? n = 85 g T = 25°C = 298 K P = kPa R = dm 3  kPa/mol  K WORK: 85 g 1 mol = 2.7 mol g PV = nRT (104.5)V=(2.7) (8.315) (298) kPa mol dm 3  kPa/mol  K K V = 64 dm 3 Find the volume of 85 g of O 2 at 25°C and kPa. Ideal Gas Law Problem

II. Gas Stoichiometry at Non- STP conditions Moles  Liters of a Gas:Moles  Liters of a Gas: –STP - use 22.4 L/mol –Non-STP - use ideal gas law Non-STPNon-STP –Given liters of gas? start with ideal gas law –Looking for liters of gas? start with stoichiometry conv.

What volume of CO 2 forms from 5.25 g of CaCO 3 at 103 kPa & 25ºC? Gas Stoichiometry Problem CaCO 3  CaO + CO g L non-STP Looking for liters: Start with stoich and calculate moles of CO 2. 1 mol CaCO g CaCO g CaCO 3 = 1.26 mol CO 2 1 mol CO 2 1 mol CaCO 3

What volume of CO 2 forms from 5.25 g of CaCO 3 at 103 kPa & 25ºC? Gas Stoichiometry Problem WORK: PV = nRT (103 kPa)V =(1mol)(8.315 dm 3  kPa/mol  K )(298K) V = 1.26 dm 3 CO 2 GIVEN: P = 103 kPa V = ? n = 1.26 mol T = 25°C = 298 K R = dm 3  kPa/mol  K

WORK: PV = nRT (97.3 kPa) (15.0 L) = n (8.315 dm 3  kPa/mol  K ) (294K) n = mol O 2 How many grams of Al 2 O 3 are formed from 15.0 L of O 2 at 97.3 kPa & 21°C? GIVEN: P = 97.3 kPa V = 15.0 L n = ? T = 21°C = 294 K R = dm 3  kPa/mol  K 4 Al + 3 O 2  2 Al 2 O L non-STP ? g Given liters: Start with Ideal Gas Law and calculate moles of O 2. NEXT  Gas Stoichiometry Problem

2 mol Al 2 O 3 3 mol O 2 How many grams of Al 2 O 3 are formed from 15.0 L of O 2 at 97.3 kPa & 21°C? mol O 2 = 40.6 g Al 2 O 3 4 Al + 3 O 2  2 Al 2 O g Al 2 O 3 1 mol Al 2 O L non-STP ? g Use stoich to convert moles of O 2 to grams Al 2 O 3. Gas Stoichiometry Problem