How many moles of hydrogen are needed to completely react with two moles of nitrogen?
Understand the Problem
The question is asking for the number of moles of hydrogen required to completely react with a specific amount of nitrogen, which involves applying stoichiometric principles from chemistry.
Answer
6 moles of hydrogen are needed to completely react with two moles of nitrogen.
Answer for screen readers
6 moles of hydrogen are needed to completely react with two moles of nitrogen.
Steps to Solve
- Write the balanced chemical equation
The first step is to write the balanced chemical equation for the reaction between nitrogen and hydrogen. The reaction is represented as: $$ N_2 + 3H_2 \rightarrow 2NH_3 $$ This means that 1 mole of nitrogen reacts with 3 moles of hydrogen.
- Identify the stoichiometric ratio
From the balanced equation, we see that 1 mole of nitrogen ($N_2$) requires 3 moles of hydrogen ($H_2$) to completely react. Therefore, the stoichiometric ratio is: $$ \text{Ratio} = \frac{3 \text{ moles } H_2}{1 \text{ mole } N_2} $$
- Calculate the moles of hydrogen needed for 2 moles of nitrogen
Using the stoichiometric ratio, we can set up the following calculation: $$ \text{Moles of } H_2 = 2 \text{ moles } N_2 \times \frac{3 \text{ moles } H_2}{1 \text{ mole } N_2} $$ This simplifies to: $$ \text{Moles of } H_2 = 6 \text{ moles } H_2 $$
6 moles of hydrogen are needed to completely react with two moles of nitrogen.
More Information
In ammonia synthesis, the reaction between nitrogen and hydrogen is crucial for producing ammonia, which is an essential chemical in fertilizers. The balanced equation helps in understanding the exact proportions in which reactants combine, ensuring efficiency in chemical reactions.
Tips
- Forgetting to balance the chemical equation before using it for calculations.
- Misinterpreting stoichiometric ratios, leading to incorrect calculations of required moles.
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