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2. How many grams of water would be produced if 20.0 liters of oxygen were burned at a temperature of
-10.0"C and a pressure of 1.3 atm?

Respuesta :

Eduard22sly

The mass of water H₂O that would be produced from the reaction is 43.2 g

How to determine the mole of oxygen

  • Volume (V) = 20 L
  • Temperature (T) = –10 ˚C = –10 + 273 = 263 K
  • Pressure (P) = 1.3 atm
  • Gas constant (R) = 0.0821 atm.L/Kmol
  • Number of mole (n) =?

The number of mole can be obtained as by using the ideal gas equation as illustrated below:

n = PV / RT

n = (1.3 × 20) / (0.0821 × 263)

n = 1.2 mole

How to determine mole of water  

Balanced equation

2H₂ + O₂ → 2H₂O

From the balanced equation above,

1 mole of O₂ reacted to produce 2 moles of H₂O.

Therefore,

1.2 mole of O₂ will react to produce = 1.2 × 2 = 2.4 moles of H₂O

How to determine the mass of water produced

  • Mole of H₂O = 2.4 moles
  • Molar mass of H₂O = (2×1) + 16 = 18 g/mol
  • Mass of H₂O =?

Mass = mole × molar mass

Mass of H₂O = 2.4 × 18

Mass of H₂O = 43.2 g

Thus, 43.2 g of water were produced from the reaction.

Learn more about stoichiometry:

https://brainly.com/question/14735801

Answer:

15.6g ofH2O

Explanation:

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