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Published byLily Mitchener Modified over 2 years ago

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Ideal Gas Law PV=nRT

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Remember… Boyles Law Charles Law: Combined Gas Law: (Units MUST Match Temp in Kelvin!!!)

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A gas with a volume of 350 ml is collected at 15 o C and 120 kPa. If the temperature changes to 30 o C, what pressure would be required to put this gas in a 300 ml container?

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A balloon has a volume of 500 ml at a temperature of 22 o C and a pressure of 755 mmHg. If the balloon is cooled to 0 o C and a pressure of 145 mmHg, what is its new volume?

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Avogadros Principle Under similar conditions (same Temp and Pressure) equal volumes of gases contain equal numbers of particles. 10 L of H 2 (g) and 10 L of O 2 (g) Both at Standard Temperature and Pressure (STP) contain… The same number of particles!

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Molar Volume The volume of 1 mole of gas particles at STP is 22.4 L

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Ideal Gas Law Animation: Ideal Gas Law Animation:

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Try this: 1 mole of gas occupies 22.4 L at STP = __________ ml (22400) = ___________ moles of gas (1 mole) = ___________ particles (6.02 x )

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How many particles in 11.2 dm 3 of gas at STP? 0.5 moles = 3.01 x particles 0.5 moles = 3.01 x particles 22,400 cm 3 of NH 3 gas at STP weighs? = 22.4 L = 1 mole = 17 grams (add up MW) = 22.4 L = 1 mole = 17 grams (add up MW) 44.8 L of NH 3 at STP weighs? = 2 moles = 34 grams = 2 moles = 34 grams _____ grams = 1 mole of nitrogen gas = _____ L at STP?

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How many N 2 molecules are in 22.4 dm 3 at STP? = 1 mole = 6.02 x = 1 mole = 6.02 x What volume will 1.2 x H 2 molecules occupy at STP? = 2 moles = 44.8 L at STP = 2 moles = 44.8 L at STP

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Ideal Gas Equation Use when NOT at STP!!! PV= nRT P = Pressure (in kPa) V = Volume (in Liters or dm 3 ) n = number of moles T = Temperature (in Kelvin) R = 8.31 L kPa mole K

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Development of R in

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1. What volume will 2 moles of NO 2 occupy at 300 Kelvin and 90 kPa?

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What will be the temp of 2 grams of H 2 if 5000 cm 3 is at 5 atm?

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Finding Molecular Weight of a Gas Remember: MW = grams / moles Converting grams to moles –D–D–D–Divide grams by the molecular weight

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1) 5.0 L of a gas weighs g at 20 o C & 92 kPa. What is the mole weight of the gas? PV=nRT 92kPa 5.0 L= n K n = 0.19 mol

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2)If the mole weight of a gas is 26 g/mol and g of the gas is 30 L at 21 o C, what is the pressure of the gas? PV= nRT P x 30 L=0.69 mol x 8.31 x 294 K P = 56.2kPa

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Stoichiometry Solving Steps. –Balance the Equation –Change grams to moles –Use mole ratio to solve –Change moles to volumes

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Use mole ratio (coefficients) Use 22.4 STP Or PV = nRT Use MW on P.T. Use MW on P.T. Use 22.4 STP Or PV = nRT

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Mg (c) + HCl (ag) MgCl 2 + H 2 (g) If 2.43 g Mg react what volume of H 2 is produced? (at STP) Mg (c) + HCl (ag) MgCl 2 + H 2 (g) Mg (c) + HCl (ag) MgCl 2 + H 2 (g) 2.43 g Mg 0.1 mole 1:1 0.1 moles L H 2 ? L

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Mg (c) +2 HCl (ag) MgCl 2 + H 2 (g) If 2.43 g Mg react what volume of H 2 is produced at 40 o C and 85 kPa? Mg (c) + HCl (ag) MgCl 2 + H 2 (g) Mg (c) + HCl (ag) MgCl 2 + H 2 (g) 2.43 g Mg 0.1 mole 1:1 0.1 moles L H 2 ? L

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If 250 ml of H 2 is produced at 20 o C & 100 kPa, what mass of Mg reacted? Mg (c) + HCl (ag) MgCl 2 + H 2 (g) Mg (c) + HCl (ag) MgCl 2 + H 2 (g) 2 ? g 250 ml 0.01 moles 0.01 mole 1: g Mg

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Volume to Volume THE MOLE RATIO IS THE SAME AS THE VOLUME RATIO. Liters B Use mole ratio (coefficients) Liters A

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Burning of methane: What vol. of oxygen is needed to completely burn 1 L of methane? CH 4 + O 2 CO 2 (g) + H 2 O (l) CH 4 + O 2 CO 2 (g) + H 2 O (l) 2.0 L 1:2 1.0 L 22

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Burning of methane: To produce 11.2 L of CO 2 requires how many moles of O 2 at STP? CH 4 + O 2 CO 2 (g) + H 2 O (l) CH 4 + O 2 CO 2 (g) + H 2 O (l) 22.4 L 2: L 1 mole = 22

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