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.

particle   p is an electron and particle q is a neutron

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.