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

`\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

Step-by-step 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((1 \ mol \ N_2)/(2 \ mol \ NH_3))`
2. [DA] Multiply/Divide [Cancel out units]:
   `\displaystyle 6 \ mol \ N_2`

Answer 2

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

Step-by-step 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.

`( 1 \ mol \ N_2)/(2 \ mol \ NH_3)`

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

`12 \ mol \ NH_3 *( 1 \ mol \ N_2)/(2 \ mol \ NH_3)`

The moles of nitrogen trihydride cancel.

`12 *( 1 \ mol \ N_2)/(2) = ( 12 \ mol \ N_2)/(2)`

`6 \ mol \ N_2`

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