Answer to Question #79026 in General Chemistry for alex

Question

If 45.6 grams of water decompose at 301 Kelvin and 1.24 atmospheres, how many liters of oxygen gas can be produced? Show all of the work used to solve this problem.

2H2O (l) yields 2H2 (g) + O2 (g)

Answer 1

If 45.6 grams of water decompose at 301 Kelvin and 1.24 atmospheres, how many liters of oxygen gas can be produced? Show all of the work used to solve this problem.

2H2O (l) yields 2H2 (g) + O2 (g)
Answer:
Number of moles of water = 45.6 g / 18 g/mole = 2.53 moles of water
From stoichiometric coefficients number of moles of oxygen = 2.53 moles/ 2 =1.27 moles of oxygen;
Universal gas law pV =nRT, therefore V =nRT/p;
Volume of oxygen at given temperature and pressure V = (1.27 moles x 0.082057 L atm mol-1K-1 x 301 K) / 1.24 atm = 25.3 L