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Standard Temperature and Pressure

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Sections
Pressure Units
The Ideal Gas Law
The Ideal Gas Law Derivations
The Ideal Gas Law Applications
Chemistry Gas Laws
Chemistry Gas Laws: Combined Gas Law
Mole Fraction
Partial Pressure
The Ideal Gas Law: Molar Mass
The Ideal Gas Law: Density
Gas Stoichiometry
Standard Temperature and Pressure
Effusion
Root Mean Square Speed
Kinetic Energy of Gases
Maxwell-Boltzmann Distribution
Velocity Distributions
Kinetic Molecular Theory
Van der Waals Equation
Boyle's Law (IGNORE)
Charles Law (IGNORE)
Ideal Gas Law (IGNORE)

In order to accurately study the effect that changes in pressure, temperature and moles have on volume, chemists will often run their experiments under Standard Temperature and Pressure

Stand Temperature and Pressure (STP)

Concept #1: Standard Temperature and Pressure

Example #1: A sample of oxygen gas has a measured volume of 325 mL at STP. How many grams are present?

Concept #2: STP and Volume

Example #2: How many moles of chlorine gas occupy a volume of 15.7 L at STP?

Practice: A sample of dichloromethane gas (CH2Cl2) occupies 32.6 L at 310 K and 5.30 atm. Determine its volume at STP?

Practice: Which gas sample has the greatest volume at STP?

Practice: Nitrogen and hydrogen combine to form ammonia via the following reaction:

1 N2 (s)  +  3 H2 (g) → 2 NH3 (g)

What mass of nitrogen is required to completely react with 800.0 mL Hat STP?