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Title: Using Molar Volume in Gas Stoichiometric Calculations Post by: chementhusiast on May 9, 2018 1. How many grams of water form when 1.24 L of H_2 gas at STP (Standard conditions for temperature and pressure) completely reacts with O_2?
2. How many liters of oxygen (at STP) are required to form 10.5 g of H_2 O? Title: Re: Using Molar Volume in Gas Stoichiometric Calculations Post by: Aliya1 on May 20, 2018 for #1. 2 H₂(g) + O₂ (g) → 2 H₂O (g) ====> note that 2 moles of H₂ produces 2 moles of H₂O
1.24-L H₂ x ( 1 mol H₂ / 22.4-L H₂) x ( 2 mol H₂O / 2 mol H₂) x (18.0-g H₂O / 1 mol H₂O) = 0.996-g H₂O #2.steps... 1) convert mass H2O to moles H2O 2) use coefficients of balanced equation to convert to moles O2 3) convert moles O2 to L O2. solution... 10.5 g H2O x (1 mole H2O / 18.0 g H2O) = 0.583 moles H2O from the balanced equation, 1 mole O2 --> 2 moles H2O.. therefore... 0.583 moles H2O x (1 mole O2 / 2 moles H2O) = 0.292 moles O2 from here you can either use the specific form of the ideal gas law for STP... 0.292 moles O2 x (22.4 L O2 / mole O2) = 6.54 L O2 or you can use the more general form of the ideal gas law... V = nRT/P = (0.292 moles) x (0.0821 Latm/moleK) x (273 K) / (1 atm) V = 6.54 L O2 found this on these websites #2. https://answers.yahoo.com/question/index?qid=20090627131045AAokR6Y #1.https://answers.yahoo.com/question/index?qid=20130423194303AAHrkxE hope this helps you ;) Title: Re: Using Molar Volume in Gas Stoichiometric Calculations Post by: bio_man on Jun 14, 2018 2. How many liters of oxygen (at STP) are required to form 10.5 g of H_2 O? https://www.youtube.com/watch?v=cAq7tHx9N_k 1. How many grams of water form when 1.24 L of H_2 gas at STP (Standard conditions for temperature and pressure) completely reacts with O_2? https://www.youtube.com/watch?v=On3nGLZFNU4 |