Nitrogen and hydrogen react together to form ammonia according to the equation: ___N₂(g)+ ___H₂(g)→ ___NH₃(g)(unbalanced)Balance the equation, and determine how many grams of hydrogen reactant would be required to produce 25.0 g of ammonia, assuming there is sufficient nitrogen available.

Question

Quizplus · Accepted Answer

The balanced equation for the reaction is:

N2(g) + 3H2(g) → 2NH3(g)

From this, we can see that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.

To find the amount of hydrogen required to produce 25.0 g of ammonia, we first need to convert the mass of ammonia to moles:

25.0 g NH3 × (1 mol NH3/17.03 g NH3) = 1.47 mol NH3

From the balanced equation, we know that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia. Therefore, if 1.47 moles of ammonia are produced, there must have been:

1.47 mol NH3 × (3 mol H2/2 mol NH3) = 2.21 mol H2

of hydrogen consumed.

Finally, we can convert the moles of hydrogen to grams:

2.21 mol H2 × (2.02 g H2/1 mol H2) = 4.46 g H2

Therefore, the answer is B) 4.46 g.

Nitrogen and Hydrogen React Together to Form Ammonia According to the Equation