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*Given
  Mass of hydrogen ([tex] H_{2} [/tex])  -  32.0 grams
  Mass of oxygen ([tex] O_{2} [/tex])     -  32.0 grams

*Additional Information 
  Molar mass of hydrogen ([tex] H_{2} [/tex]) - 2.00 g/mol
  Molar mass of oxygen ([tex] O_{2} [/tex])    - 32.00 g/mol
  Molar mass of water ([tex] H_{2}O [/tex])    - 18.00 g/mol
 
Chemical Reaction:
                    
 [tex] 2H_{2(g)} [/tex]  +  [tex] O_{2(g)} [/tex]   --------> [tex] 2H_{2}O_{g} [/tex]
                                  
*Solution

From the chemical reaction above, we can see that for every 1 molecule or mole of oxygen ([tex] O_{2} [/tex]), we would need 2 molecules or moles of hydrogen ([tex] H_{2} [/tex]) to form water ([tex] H_{2}O [/tex]). 


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The amount in grams of water will be formed when 32.0 g H₂ is mixed with 32.0 g O₂ is 36 grams.

How we convert mass into moles?

Moles from mass of any susbatnce will be calculated as:

n = W/M, where

W = given mass

M = molar mass

Given chemical reaction is:

2H₂  +  O₂  →  2H₂O

Moles of H₂ = 32g / 2g/mol = 16 mol

Moles of O₂ = 32g / 32g/mol = 1 mol

From the stoichiometry of the reaction, it is clear that

1 mole of O₂ = reacts with 2 moles of H₂

So in the given question, oxygen is the limiting reagent as hydrogen is present in excess quantity & predominated the formation of water.

1 mole of O₂ = produces 2 moles of H₂O

Now grams of water will be obtained by using mass-moles equation as:

W = (2mol)(18g/mol) = 36 grams.

Hence required mass of water is 36 grams.

To know more about mass & moles, visit the below link:

https://brainly.com/question/15249931

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