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Ganezh [65]
2 years ago
5

Passing an electric current through a sample of water (H2O) can cause the water to decompose into hydrogen gas (H2) and oxygen g

as (O2) according to the following equation. 2H2O Right arrow. 2H2 O2 The molar mass of H2O is 18. 01 g/mol. The molar mass of O2 is 32. 00 g/mol. What mass of H2O, in grams, must react to produce 50. 00 g of O2? 14. 07 23. 05 28. 14 56. 28.
Chemistry
1 answer:
Lerok [7]2 years ago
8 0

The mass of water decomposed to produce 50 g oxygen has been 56.28 g. Thus, option D is correct.

The reaction for the decomposition of water has been:

\rm 2\;H_2O\;\rightarrow\;H_2\;+\;O_2

From the balanced equation, 2 moles of water decomposes to form 1 moles of hydrogen and 1 mole of oxygen.

The mass of oxygen produced has been 50 g. The moles of oxygen has been given by:

\rm Moles=\dfrac{mass}{molar\;mass}

The moles of oxygen has been:

\rm Moles_O_2=\dfrac{50}{32}\;mol\\Moles_O_2=1.5625\;mol

The moles of oxygen produced has been 1.5625 mol.

The moles of hydrogen decomposed has been given from the balanced chemical equation as:

\rm 1 \;mole\;O_2=2\;mole\;H_2O\\1.5625\;mol\;O_2=1.5625\;\times\;2\;mol\;H_2O\\1.5625\;mol\;O_2=3.125\;mol\;H_2O

The moles of hydrogen decomposes has been 3.125 mol.

The mass of hydrogen decomposed has been given by:

\rm Mass=moles\;times\;molar\;mass\\Mass_{H_2O}=3.125\;\times\;18.01\;g\\Mass_{H_2O}=56.28\;g

The mass of water decomposed to produce 50 g oxygen has been 56.28 g. Thus, option D is correct.

For more information about moles produced, refer to the link:

brainly.com/question/10606802

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