Respuesta :
Answer : The mass of oxygen consumed in the reaction is 14.6 grams.
Explanation :
First we have to calculate the change in moles of oxygen.
Formula used :
[tex]w=\Delta nRT[/tex]
or,
[tex]\Delta n=\frac{w}{RT}[/tex]
where,
w = work done = 850.1 J
[tex]\Delta n[/tex] = change in moles of gas = ?
R = gas constant = 8.314 J/mol.K
T = temperature = 675 K
Now put all the given values in the above formula, we get:
[tex]\Delta n=\frac{850.1J}{(8.314J/mol.K)\times (675K)}=0.152mol[/tex]
Now we have to calculate the mass of oxygen consumed.
The balanced chemical reaction is,
[tex]2ZnS(s)+3O_2(g)\rightarrow 2ZnO(s)+2SO_2(g)[/tex]
Here, the volume changes of solids can be ignored.
From the balanced chemical reaction, we conclude that
The number of moles oxygen required for the complete reaction = 3
Change in mole of oxygen = 0.152 mol
Molar mass of [tex]O_2[/tex] = 32 g/mol
So,
The mass of oxygen consumed = 3 x 0.152 mol x 32 g/mol = 14.6 g
Therefore, the mass of oxygen consumed in the reaction is 14.6 grams.
14.6 g of oxygen are consumed in the reaction.
The given reaction is
[tex]\rm \bold{ 2ZnS(s) 3O_2(g)\rightarrow2ZnO(s) 2SO_2(g) }[/tex]
The molar mass of oxygen is 32 g/mol
The number of moles consumed in reaction,
[tex]\rm \bold{ \Delta n = \frac{RT}{w} }[/tex]
Where,
w = work done = 850.1 J
R = gas constant = 8.314 J/mol.K
T = temperature = 675 K
put the values in formula we get number of moles consumed in reaction is 0.152mol
The mass of oxygen are consumed in the reaction,
[tex]\rm \bold { \Rightarrow 3\times 32 \times 0.152}\\\rm \bold { \Rightarrow 14.6 g}[/tex]
Hence, we can conclude that 14.6 g of oxygen are consumed in the reaction.
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https://brainly.com/question/22997914?referrer=searchResults
