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The substances nitrogen monoxide and hydrogen gas react to form nitrogen gas and water. Unbalanced equation: NO (g) + H2 (g) N2 (g) + H2O (l) In one reaction, 76.2 g of H2O is produced. What amount (in mol) of H2 was consumed? What mass (in grams) of N2 is produced?

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Answer:

H2 consumed 4.22 mol

N2 produced 59.107 g

Explanation:

Balanced equation:

2NO (g) + 2H2 (g) N2 (g) + 2H2O (l)

  • To perform the calculations, the molecular weights of the following compounds must be known:

H2O MW = 18.02 g/mol

N2 MW = 28.01 g/mol

To determine the moles of H2O produced, the following formula should be used:

[tex]MW=\frac{mass}{mol}[/tex]

The value of moles is cleared:

[tex]mol=\frac{mass}{MW} =\frac{76.2g}{18.02\frac{g}{mol} } =4.22 mol[/tex]

  • Now, to calculate the grams of N2 consumed, we look at the balanced equation and note that 2 moles of H2 produce 1 mole of N2. Therefore, through said observation, the amount of moles of H2 consumed can be determined.

2 mol H2      ⇒ 1 mol N2

4.22 mol H2 ⇒ X

[tex]X=\frac{4.22mol*1 mol}{2 mol} =2.11 mol[/tex]

To calculate the mass of H2 consumed, the molecular weight equation is used again:

[tex]mass=MW*mol=28.013\frac{g}{mol}*2.11mol=59.107g[/tex]

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