Given: N2 + 3H2 → 2NH3
In the chemical reaction, how many grams of nitrogen are needed to completely react with 24.3 grams of hydrogen? Use the periodic table to get the weights of the elements.
Drag each number to the correct location to complete the analysis.

113.4g of N2

Explanation:

Step 1:

The balanced equation for the reaction.

N2 + 3H2 —> 2NH3

Step 2:

Determination of the mass of N2 and H2 that reacted from the balanced equation. This is illustrated below:

Molar mass of N2 = 2x14 = 28g/mol

Mass of N2 from the balanced equation = 1 x 28 = 28g

Molar mass of H2 = 2x1 = 2g/mol

Mass of H2 from the balanced equation = 3 x 2 = 6g

From the balanced equation above, 28g of N2 reacted with 6g of H2.

Step 3:

Determination of the mass N2 required to react with 24.3g of H2.

The mass of N2 required to react with 24.3g of H2 can be obtained as follow:

From the balanced equation above, 28g of N2 reacted with 6g of H2.

Therefore, Xg of N2 will react 24.3g of H2 i.e

Xg of N2 = (28 x 24.3)/6

Xg of N2 = 113.4g

Therefore, 113.4g of N2 is required to react completely with 24.3g of H2.

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.