Practice: A sample of dichloromethane gas (CH2Cl2) occupies 32.6 L at 310 K and 5.30 atm. Determine its volume at STP?
Subjects
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Pressure Units | 6 mins | 0 completed | Learn |
The Ideal Gas Law | 19 mins | 0 completed | Learn Summary |
The Ideal Gas Law Derivations | 6 mins | 0 completed | Learn |
The Ideal Gas Law Applications | 7 mins | 0 completed | Learn |
Chemistry Gas Laws | 16 mins | 0 completed | Learn |
Chemistry Gas Laws: Combined Gas Law | 12 mins | 0 completed | Learn |
Mole Fraction | 6 mins | 0 completed | Learn |
Partial Pressure | 19 mins | 0 completed | Learn Summary |
The Ideal Gas Law: Molar Mass | 19 mins | 0 completed | Learn |
The Ideal Gas Law: Density | 16 mins | 0 completed | Learn Summary |
Gas Stoichiometry | 7 mins | 0 completed | Learn |
Standard Temperature and Pressure | 14 mins | 0 completed | Learn |
Effusion | 13 mins | 0 completed | Learn Summary |
Root Mean Square Speed | 9 mins | 0 completed | Learn Summary |
Kinetic Energy of Gases | 5 mins | 0 completed | Learn |
Maxwell-Boltzmann Distribution | 8 mins | 0 completed | Learn |
Velocity Distributions | 5 mins | 0 completed | Learn |
Kinetic Molecular Theory | 7 mins | 0 completed | Learn |
Van der Waals Equation | 9 mins | 0 completed | Learn |
Additional Practice |
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Manometer |
Collecting Gas Over Water |
Additional Guides |
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Boyle's Law |
Charles Law |
Ideal Gas Law |
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 conditions.
Example #1: A sample of oxygen gas has a measured volume of 325 mL at STP. How many grams are present?
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 H2 at STP?
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