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The information shows the masses after the compounds are balanced.
2MgO + 2Cl2 → 2MgCl2 + ?
80g + 140g + 1889 + ?
If the following materials are used during the reaction of magnesium,
oxygen, and chlorine, what mass oxygen would we expect to see after
the reaction and why?
O A. 40g of Oz, because all mass must be conserved, it would be half of the
compound Mgo in the products
O B. 32g of Oz, because all mass must be conserved
c. 32g of Oz, because all mass must be conserved, it would be half of the
compound Mgo in the products
D. 40g of Oz, because all mass must be conserved

The information shows the masses after the compounds are balanced 2MgO 2Cl2 2MgCl2 80g 140g 1889 If the following materials are used during the reaction of mag class=

Respuesta :

B .32g of Oz because all

32g mass of oxygen would we expect to see after the reaction, because all mass must be conserved.

How we calculate the mass of any substance from moles?

Mass of any substance can be calculated from moles as:

n = W/M, where

n = moles

W = given weight or mass

M = molar mass

Given balanced complete chemical reaction is:

2MgO + 2Cl₂ → 2MgCl₂ + O₂

From the stoichiometry of the reaction it is clear that 2 moles of MgO & Cl₂ is required for the formation of 2 moles of MgCl₂ & 1 mole of O₂. Also the masses of the compound is also given for the balanced reaction as:

Mass of MgO for 2 mole = 80g

Mass of Cl₂ for 2 mole = 140g

Mass of MgCl₂ for 2 mole = 188g

So, it is clear that given masses will show conservation for their standard 1 mole of masses as mass of MgO, Cl₂ & MgCl₂ for 1 mole is 40.3g/mol, 70.90g/mol & 95.2g/mol respectively.

Hence,  we conclude that mass for 1 mole of O₂ should be 32g.

Therefore, option (B) is correct i.e. 32g of O₂, because all mass must be conserved.

To know more about mole to mass conversion, visit the below link:

https://brainly.com/question/13314627

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