 # Do NOW Please draw the Lewis Dot structure of NO3-1 and identify if it is a polar or nonpolar molecule.

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Do NOW Please draw the Lewis Dot structure of NO3-1 and identify if it is a polar or nonpolar molecule.

Ideal Gas Law

STP Standard Temperature and Pressure T = 273 K (0 °C) P = 1 atm

Ideal Gas Law PV = nRT R = ideal gas constant

Ideal Gas Constant R = (L atm)/(mol K) R= (L kPa)/(mol K) R = 62.4 (L mmHg)/(mol K)

Example Calculate the number of moles of gas contained in a 3.0 L vessel at 3.00 x 102 K with a pressure of 1.50 atm. 0.18 mol

Example What volume will an ideally behaving gas containing 1.00 mole of particles occupy at STP?

If I have 17 moles of gas at a temperature of 340 K, and a volume of liters, what is the pressure of the gas?

If I have 1.9 moles of gas held at a pressure of 5 atm and in a container with a volume of 50 liters, what is the temperature of the gas?

Gas Stoichiometry 2C4H10(g) + 13O2(g)  8CO2(g) + 10H2O(g)
What type of reaction is this? How many moles of butane gas react with how many moles of oxygen gas?

2C4H10(g) + 13O2(g)  8CO2(g) + 10H2O(g)
Gas Stoichiometry 2C4H10(g) + 13O2(g)  8CO2(g) + 10H2O(g) Avogadro’s Principle: = V of gas at same T & P contain = # of particles  Coefficients represent not only molar amounts, but also relative volumes

Gas Stoichiometry- Volume Only
CH4(g) + 2O2(g)  CO2(g) + 2H2O (g) It takes 2 L of O2 to react completely with 1 L of CH4 The complete combustion of 1 L of methane produces 1 L of carbon dioxide and 2 L of water vapor. What volume of methane is needed to produced 26 L of water vapor?

Gas Stoichiometry- Volume Only
What volume of oxygen gas is needed for the complete combustion of 4 L of propane gas? Assume constant pressure and temperature. C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g) 20.0 L O2

Gas Stoichiometry- Volume & Mass
Balanced chemical equations allow you to find ratios for moles and volume – not for masses!

Gas Stoichiometry- Volume & Mass
N2(g) + 3H2(g)  2NH3(g) If 5.00 L of nitrogen reacts completely by this reaction at a constant pressure and temperature of 3.00 atm and 298 K, how many grams of ammonia are produced? Givens: VN2 = 5.00 L P = 3.00 atm T = 298 K Unknown: mNH3 = ?

N2(g) + 3H2(g)  2NH3(g) Find VNH3.
Rearrange Ideal Gas Law equation to solve for n. Convert moles of ammonia to grams.

N2(g) +3H2 (g)→ 2NH3(g) What volume of nitrogen at STP would be required to react with mol of hydrogen to produce ammonia?

4Fe(s) + 3O2(g)  2Fe2O3(s) Calculate the volume of oxygen gas at STP that is required to completely react with 52.0 g of iron. Convert Fe mass to moles. Determine number of moles of O2. Determine volume of O2 using Ideal Gas Law. Givens: mFe = 52.0 g T = 273 K P = 1 atm 15.6 L Unknown: VO2 = ?

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