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Gas Stoichiometry At STP

Gas Stoichiometry At STP. Start with a balanced equation . Convert mass to moles (use molar mass) or volume to moles (use 22.4 L/mol) , if necessary. Use mole ratios to calculate moles of unknown. Convert moles to mass (use molar mass) or volume (use 22.4 L/mol) , if necessary.

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Gas Stoichiometry At STP

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  1. Gas Stoichiometry At STP • Start with a balanced equation. • Convert mass to moles (use molar mass) or volume to moles (use 22.4 L/mol), if necessary. • Use mole ratios to calculate moles of unknown. • Convert moles to mass (use molar mass) or volume (use 22.4 L/mol), if necessary.

  2. Gas Stoichiometry If reactants and products are at the same conditions of temperature and pressure, then mole ratios of gases are also volume ratios. 3 H2(g) + N2(g)  2NH3(g) 3moles H2 +1mole N2 2moles NH3 3liters H2 + 1liter N2 2liters NH3

  3. Volume-Volume Calculation How many liters of ammonia can be produced when 12 liters of hydrogen react with an excess of nitrogen? 3 H2(g) + N2(g)  2NH3(g) 12 L H2 2 L NH3 = L NH3 8.0 3 L H2 Volume ratio

  4. Mass-Volume Calculation How many liters of oxygen gas, at STP, can be collected from the complete decomposition of 50.0 grams of potassium chlorate? 2 KClO3(s)  2 KCl(s) + 3 O2(g) Molar volume 50.0 g KClO3 1 mol KClO3 3 mol O2 22.4 L O2 122.55 g KClO3 2 mol KClO3 1 mol O2 = 13.7 L O2 Molar mass Mole ratio

  5. Gas Stoichiometry NOT at STP • Start with a balanced equation. • Convert to moles (if amount is L, use n = PV/RT). • Use mole ratios to calculate moles of unknown. • Convert moles to desired measurement (to convert to L use PV=nRT).

  6. Mass-Volume NOT at STP How many liters of oxygen gas, at 37.0C and 0.930 atmospheres, can be collected from the complete decomposition of 50.0 grams of potassium chlorate? 2KClO3(s)  2KCl(s) + 3O2(g) 50.0 g KClO3 1 mol KClO3 3mol O2 0.612 = mol O2 122.55 g KClO3 2mol KClO3 = 16.7 L

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