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How many grams of H2 are needed to react with 2.45 g of N2 ?

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Answer:

0.525g of Hydrogen is needed to react with 2.45 g of Nitrogen.

Step-by-step explanation:

First, we will need the equation. The chemical equation is:

N2 + 3H2 → 2NH3

Now we have to take the mole-mole ratio to find the moles of H2 and convert it to grams.

N2 : H2

1 : 3

y : x

We don't have the actual moles of N2 but we can find it by using the formula:

moles= mass/molar mass

To find the molar mass we should use the periodic table. In the periodic table, the atomic mass of N2 is 14. To find the molar mass we have to multiply the moles and by the atomic mass and add it to the number of molecules.

1 ×(14+14) (2 nitrogens are present)

Molecular mass= 28 g/mol

Plug in the values into the earlier equation:

moles= 2.45 g/ 28 g/mol

moles= 0.0875 mol

So going back to the ratio:

N2 : H2

1 : 3

0.0875 : x

x= 3 × 0.0875 (cross multiplication)

x= 0.2625

To convert these moles into grams we may use the formula:

mass= moles × molar mass

mass= 0.2625 mol × 2 g/mol

mass= 0.525 g

User Tobias Gies
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