Questions: Consider the following unbalanced equation: NH3(g) → N2(g) + H2(g) How many moles of N2 will be produced by the decomposition of 4.50 moles of ammonia? What is the mole ratio between NH3 and N2 in the balanced equation? 2 NH3(g) → N2(g) + 3 H2(g)

Consider the following unbalanced equation: NH3(g) → N2(g) + H2(g) How many moles of N2 will be produced by the decomposition of 4.50 moles of ammonia? What is the mole ratio between NH3 and N2 in the balanced equation? 2 NH3(g) → N2(g) + 3 H2(g)
Transcript text: Consider the following unbalanced equation: \[ \mathrm{NH}_{3}(g) \rightarrow \mathrm{N}_{2}(g)+\mathrm{H}_{2}(g) \] How many moles of $\mathrm{N}_{2}$ will be produced by the decomposition of 4.50 moles of ammonia? HOW DO WE GET THERE? What is the mole ratio between $\mathrm{NH}_{3}$ and $\mathrm{N}_{2}$ in the balanced equation? \[ 2 \mathrm{NH}_{3}(\mathrm{~g}) \rightarrow \mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \]
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Solution

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Solution Steps

Step 1: Balance the Chemical Equation

The given unbalanced equation is: \[ \mathrm{NH}_{3}(g) \rightarrow \mathrm{N}_{2}(g) + \mathrm{H}_{2}(g) \]

The balanced equation is: \[ 2 \mathrm{NH}_{3}(g) \rightarrow \mathrm{N}_{2}(g) + 3 \mathrm{H}_{2}(g) \]

Step 2: Determine the Mole Ratio

From the balanced equation, the mole ratio between \(\mathrm{NH}_{3}\) and \(\mathrm{N}_{2}\) is 2:1. This means that 2 moles of \(\mathrm{NH}_{3}\) produce 1 mole of \(\mathrm{N}_{2}\).

Step 3: Calculate Moles of \(\mathrm{N}_{2}\) Produced

Given that 4.50 moles of \(\mathrm{NH}_{3}\) decompose, we use the mole ratio to find the moles of \(\mathrm{N}_{2}\) produced: \[ \text{Moles of } \mathrm{N}_{2} = \frac{4.50 \text{ moles of } \mathrm{NH}_{3}}{2} = 2.25 \text{ moles of } \mathrm{N}_{2} \]

Final Answer

\[ \boxed{2.25 \text{ moles of } \mathrm{N}_{2}} \]

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