Ideal Gas Law & Gas Stoichiometry Work out each problem in the 3-step format. Gases notes #4 - Ideal Gas Law & Gas Stoichiometry.pptx.

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Ideal Gas Law & Gas Stoichiometry Work out each problem in the 3-step format. Gases notes #4 - Ideal Gas Law & Gas Stoichiometry.pptx

After this lesson you will be able to: Solve problems involving the gas laws involving chemical reactions Apply stoichiometry principles in addition to gas laws Recognize which equations to apply in different types of problems involving gases

QUESTION #1 How many grams of CO 2 are produced from 75 L of CO at 35°C and 96.2 kPa? 2CO + 1O 2  2CO 2

Find the moles of CO: n = ? mol V = 75 L P = 96.2 kPa T = 35°C R = L  atm/mol  K Use: PV = nRT n = mol CO 2CO + 1O 2  2CO 2 ? g 75 L, 35 °C, 96.2 kPa ANSWER #1, part 1 = atm = 308 K

ANSWER #1, part 2 Use stoichiometry: 2CO + 1O 2  2CO mol ? g mol CO 2 mol CO 2 2 mol CO g CO 2 1 mol CO 2 = 120 g CO 2

QUESTION #2 How many moles of oxygen will occupy a volume of 2.5 L at 1.2 atm and 25°C?

ANSWER #2 n = ? V = 2.5 L P = 1.2 atm T = 25°C R = L  atm/mol  K Use: PV = nRT n = 0.12 mol = 298 K

QUESTION #3 What volume will 56.0 grams of nitrogen gas occupy at 96.0 kPa and 21°C?

ANSWER #3 V = ? n = 56.0 g P = 96.0 kPa T = 21°C R = L  atm/mol  K Use:PV = nRT V = 50.9 L = mol = atm = 294 K

QUESTION #4 What volume of NH 3 at STP is produced if 25.0 g of N 2 is reacted with excess H 2 ? 1N 2 + 3H 2  2NH 3

ANSWER # g N 2 1 mol N g N 2 = 40.0 L NH 3 1 N H 2  2 NH 3 2 mol NH 3 1 mol N L NH 3 1 mol NH g? L, STP Use stoichiometry: excess limiter

QUESTION #5 What volume of hydrogen is produced from 25.0 g of water at 27°C and 1.16 atm? 2H 2 O  2H 2 + 1O 2

ANSWER #5, part g H 2 O 1 mol H 2 O g H 2 O = mol H 2 2 mol H 2 2 mol H 2 O 2H 2 O  2H 2 + 1O g ? L, 27  C, 1.16 atm Use stoichiometry:

ANSWER #5, part 2 Find the product volume: n = mol V = ? P = 1.16 atm T = 27°C R = L  atm/mol  K Use: PV = nRT V = 29.4 L 2H 2 O  2H 2 + 1O 2 ? L, 27  C, 1.16 atm (= mol) 25.0 g = 300 K

QUESTION #6 How many atmospheres of pressure will be exerted by 25 g of CO 2 at 25°C and L?

ANSWER #6 P = ? n = 25 g T = 25°C V = L R = L  atm/mol  K Use: PV = nRT P = 28 atm = mol = 298 K

QUESTION #7 How many grams of CaCO 3 are required to produce 45.0 L of CO 2 at 25°C and 2.3 atm? 1CaCO 3 + 2HCl  1CO 2 + 1H 2 O + 1CaCl 2

ANSWER #7, part 1 Find the moles of product: n = ? V = 45.0 L P = 2.3 atm T = 25°C R = L  atm/mol  K Use: PV = nRT n = mol ? g 45.0 L, 25  C, 2.3 atm 1 CaCO HCl  1 CO H 2 O + 1 CaCl 2 = 298 K

ANSWER #7, part mol CO 2 = 4.2 x 10 2 g CaCO 3 1 CaCO HCl  1 CO H 2 O + 1 CaCl 2 1 mol CaCO 3 1 mol CO 2 ? g 45.0 L, 25  C, 1 atm, mol g CaCO 3 1 mol CaCO 3 Use stoichiometry:

QUESTION #8 Find the number of grams of CO 2 that exert a pressure of 785 torr at 32.5 L and 32°C.

ANSWER #8 n = ? P = 785 torr V = 32.5 L T = 32°C R = L ⋅ atm / mol ⋅ K Use: PV = nRT n = mol Convert using molar mass: = 59.0 g CO 2 = atm = 305 K

Tips for solving problems with gases: 1.Is there a chemical reaction happening? If yes, then write the balanced equation and use stoichiometry. 2.Are there changing conditions? If yes, then use the Everything Law (convert T to Kelvins). 3.No changing conditions? Use the Ideal Gas Law (convert all units to match R).