Achemist needs to find out how large of a container would be required to contain the products of an ammonia decomposition. if 8.91 mol h2 are produced during the reaction, how many moles of n2 are produced? 2.97 mol n2 26.7 mol n2 8.91 mol n2

2.97 mol N2. The decomposition of ammonia to produce 8.91 mol H2 also produces 2.97 mol N2.

(a)Write the balanced equation.

2NH3 → N2 + 3H2

(b)Use the balanced equation to find the molar ratio of H2:N2.

Molar ratio = 1 mol N2:3 mol H2

(c)Use the molar ratio to calculate the moles of N2.

Moles of N2 = 8.91 mol H2 x (1 mol N2/3 mol H2) = 2.97 mol N2

The result makes dense because the balanced equation tells us that the amount of N2 is one-third the amount of H2.

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%