Beryllium nitride (Be3N2, molar mass =55.056 g/mol) reacts with water to produce beryllium hydroxide and ammonia.What mass of ammonia is produced from a complete reaction between 20.0 g of Be3N2 and 20.0 g of water? 56.7 g 12.4 g 6.30 g 18.9 g 23.1 g

To solve this problem, we need to use stoichiometry, which is a method in chemistry that uses balanced chemical equations to calculate quantities of reactants or products.

The balanced chemical equation for the reaction is:

Be3N2 + 6H2O -> 3Be(OH)2 + 2NH3

From the balanced equation, we can see that one mole of Be3N2 reacts with six moles of water to produce two moles of ammonia (NH3).

First, we need to calculate the number of moles of Be3N2 and H2O we have:

For Be3N2: Number of moles = mass / molar mass = 20.0 g / 55.056 g/mol = 0.363 moles

For H2O: Molar mass of H2O = 18.015 g/mol Number of moles = mass / molar mass = 20.0 g / 18.015 g/mol = 1.11 moles

From the balanced equation, we can see that the mole ratio of Be3N2 to H2O is 1:6. Therefore, Be3N2 is the limiting reactant because we have less than 6 times the amount of H2O compared to Be3N2.

Next, we can calculate the amount of NH3 produced. From the balanced equation, we can see that the mole ratio of Be3N2 to NH3 is 1:2. Therefore, the number of moles of NH3 produced is 2 * 0.363 moles = 0.726 moles.

Finally, we can calculate the mass of NH3 produced:

Mass = number of moles * molar mass Molar mass of NH3 = 17.031 g/mol Mass = 0.726 moles * 17.031 g/mol = 12.4 g

So, the mass of ammonia produced from a complete reaction between 20.0 g of Be3N2 and 20.0 g of water is 12.4 g.