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Consider the reaction of hydrogen and oxygen producing water. If 26.1 g of water is produced and 23.0 g of oxygen is used, how many g of hydrogen are needed?

Respuesta :

sebassandin

Answer:

[tex]m_{H_2}=3.1gH_2[/tex]

Explanation:

Hello,

In this case, given the reaction:

[tex]2H_2+O_2\rightarrow 2H_2O[/tex]

When 23.0 g of oxygen react and 26.1 g of water are yielded, given the law of conservation of mass which states the mass of reactants must equal the mass of products:

[tex]m_{H_2}+m_{O_2}=m_{H_2O}[/tex]

The mass of hydrogen turns out:

[tex]m_{H_2}=m_{H_2O}-m_{O_2}\\\\m_{H_2}=26.1g-23.0g\\\\m_{H_2}=3.1gH_2[/tex]

Best regards.

Cricetus

Grams of hydrogen needed is "3.1 g".

According to the question,

  • Water produced = 26.1 g
  • Oxygen used = 23.0 g

The reaction will be:

  • [tex]2H_2 + O_2 \rightarrow 2H_2 O[/tex]

Now,

→ [tex]m H_2 +mO_2 = mH_2 O[/tex]

or,

→ [tex]mH_2 = mH_2O-mO_2[/tex]

By substituting the values,

          [tex]= 26.1-23.0[/tex]

          [tex]= 3.1 \ g[/tex]

Thus the answer above is right.

Learn more about oxygen here:

https://brainly.com/question/25199910

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