Question

1. 1 N2+ 3 H2→2 NH3

c.How many moles of nitrogen are needed to produce 12 moles of nitrogen trihydride?

Answer 1

Answer:

$\displaystyle 6 \ mol \ N_2$

General Formulas and Concepts:

Math

Pre-Algebra

Order of Operations: BPEMDAS

1. Brackets
2. Parenthesis
3. Exponents
4. Multiplication
5. Division
6. Addition
7. Subtraction

• Left to Right

Chemistry

Atomic Structure

• Writing Compounds

Stoichiometry

• Using Dimensional Analysis
• Reactions RxN

Explanation:

Step 1: Define

[RxN - Balanced] N₂ + 3H₂ → 2NH₃

[Given] 12 mol NH₃

[Solve] x mol N₂

Step 2: Identify Conversions

[RxN] 1 mol N₂ → 2 mol NH₃

Step 3: Stoich

1. [DA] Set up:                                                                                                   $\displaystyle 12 \ mol \ NH_3(\frac{1 \ mol \ N_2}{2 \ mol \ NH_3})$
2. [DA] Multiply/Divide [Cancel out units]:                                                       $\displaystyle 6 \ mol \ N_2$

Answer 2

Answer:

$\boxed {\boxed {\sf 6 \ moles \ of \ N_2}}$

Explanation:

1. Balance Equation

We are given the reaction:

$1 N_2+3H_2 \rightarrow 2 NH_3$

The equation is already balanced. Both sides have 2 moles of nitrogen and 6 moles of hydrogen.

2. Conversions

In this reaction, 1 mole of nitrogen produces 2 moles of nitrogen tryhdride:

$1 \ mol \ N_2 \rightarrow 2 \ mol \ NH_3$

3. Stoichiometry Calculations

Use the conversion rate as a fraction.

$\frac{ 1 \ mol \ N_2}{2 \ mol \ NH_3}$

Multiply the number of moles of nitrogen trihydride produced: 12 moles.

$12 \ mol \ NH_3 *\frac{ 1 \ mol \ N_2}{2 \ mol \ NH_3}$

The moles of nitrogen trihydride cancel.

$12 *\frac{ 1 \ mol \ N_2}{2} = \frac{ 12 \ mol \ N_2}{2}$

$6 \ mol \ N_2$

6 moles of nitrogen are needed to produce 12 moles of nitrogen trihydride.