The mass of water formed in the reaction is [tex]\rm 1.63\;\times\;10^-^3[/tex] g. Thus, option A is correct.
The balanced chemical equation for the formation of water is:
[tex]\rm 2\;H_2\;+\;O_2\;\rightarrow\;2\;H_2O[/tex]
From the balanced chemical equation, 1 mole of oxygen forms 2 moles of water.
The moles of a compound is given by:
[tex]\rm Moles=\dfrac{Mass}{Molar\;mass}[/tex]
The moles of oxygen reacted in the reaction are:
[tex]\rm Moles\;O_2=\dfrac{1.45\;\times\;10^-^3\;g}{32\;g/mol} \\Moles\;O_2=0.045\;\times\;10^-^3\;mol[/tex]
The moles of water formed is:
[tex]\rm 1\;mol\;O_2=2\;mol\;H_2O\\0.045\;\times\;10^-^3\;mol\;O_2=0.045\;\times\;10^-^3\;\times\;2\;mol\;H_2O\\0.045\;\times\;10^-^3\;mol\;O_2=0.09\;\times\;10^-^3\;mol\;H_2O[/tex]
The moles of water formed are [tex]\rm 0.09\;\times\;10^-^3[/tex] mol.
The mass of water is given as:
[tex]\rm Mass=Moles\;\times\;Molar\;mass\\Mass\;H_2O=0.09\;\times\;10^-^3\;\times\;18\;g\\Mass\;H_2O=1.63\;\times\;10^-^3\;g[/tex]
The mass of water formed in the reaction is [tex]\rm 1.63\;\times\;10^-^3[/tex] g. Thus, option A is correct.
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