Question

N2(g) + 3H2(g) → 2NH3(g) How many grams of N2 are required to produce 240.0g NH3?

Answer 1

Answer:

$\large \boxed{\text{197.4 g}}$

Explanation:

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ:     28.01               17.03

            N₂ + 3H₂ ⟶ 2NH₃

m/g:                          240.0

(a) Moles of NH₃

$\text{Moles of NH}_{3} = \text{240.0 g NH}_{3}\times \dfrac{\text{1 mol NH}_{3}}{\text{17.03 g NH}_{3}}= \text{14.09 mol NH}_{3}$

(b) Moles of N₂

$\text{Moles of N _{2} } = \text{14.09 mol NH}_{3} \times \dfrac{\text{1 mol N _{2} }}{\text{2 mol NH}_{3}} = \text{7.046 mol N _{2} }$

(c) Mass of N₂

$\text{Mass of N _{2} } =\text{7.046 mol N _{2} } \times \dfrac{\text{28.01 g N _{2} }}{\text{1 mol N _{2} }} = \textbf{197.4 g N _{2} }\\\\\text{The reaction requires \large \boxed{\textbf{197.4 g}} of N _{2} }$

Answer 2

Chemistry I need helpAnswer:

Explanation: