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Chapter 3: Problem 92

Nitrogen reacts with hydrogen to form ammonia. Represent each nitrogen atom by a square and each hydrogen atom with a circle. Starting with five molecules of both hydrogen and nitrogen, show pictorially what you have after the reaction is complete.

Short Answer

Expert verified
Answer: After the reaction, the final pictorial representation is: Unreacted nitrogen (N_2) molecules: □ □ □ □ Unreacted hydrogen (H_2) molecules: ○ ○ Produced ammonia (NH_3) molecules: NH_3 NH_3

Step by step solution

01

Understand the chemical reaction

The chemical reaction between nitrogen and hydrogen to form ammonia can be represented as follows: N_2 + 3H_2 -> 2NH_3 Here, one molecule of nitrogen (N_2) reacts with three molecules of hydrogen (H_2) to form two molecules of ammonia (NH_3).
02

Represent given nitrogen and hydrogen molecules

We start with five molecules of both hydrogen (circles) and nitrogen (squares). Since nitrogen exists as a diatomic molecule (N_2), we will have 5 nitrogen molecules (10 nitrogen atoms), and 5 hydrogen molecules (10 hydrogen atoms). Nitrogen molecules (N_2) : □ □ □ □ □ Hydrogen molecules (H_2) : ○ ○ ○ ○ ○
03

Perform the reaction

Now, we will let the nitrogen and hydrogen molecules react to form ammonia following the reaction previously described. We will use up as many nitrogen and hydrogen molecules as possible based on the stoichiometry of the reaction: 1 N_2 molecule + 3 H_2 molecules -> 2 NH_3 molecules Since we have 5 nitrogen and 5 hydrogen molecules, it's crucial to notice that our limiting reactant is hydrogen in this case. We have enough hydrogen to react with 5/3 ≈ 1.67 nitrogen molecules. Therefore, only one nitrogen molecule can fully react with three hydrogen molecules to form ammonia. Reaction outcome: 1 N_2 molecule + 3 H_2 molecules -> 2 NH_3 molecules □ + ○ ○ ○ -> NH_3 NH_3
04

Show the final pictorial representation

Considering one nitrogen molecule has reacted with three hydrogen molecules to form two ammonia molecules, this is the pictorial representation of the system after the reaction is complete: Unreacted nitrogen (N_2) molecules: □ □ □ □ Unreacted hydrogen (H_2) molecules: ○ ○ Produced ammonia (NH_3) molecules: NH_3 NH_3

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Most popular questions from this chapter

Determine the simplest formulas of the following compounds: (a) the food enhancer monosodium glutamate (MSG), which has the composition \(35.51 \%\) C, \(4.77 \% \mathrm{H}, 37.85 \% \mathrm{O}, 8.29 \% \mathrm{~N}\), and \(13.60 \% \mathrm{Na} .\) (b) zircon, a diamond-like mineral, which has the composition \(34.91 \%\) \(\mathrm{O}, 15.32 \% \mathrm{Si}\), and \(49.76 \% \mathrm{Zr}\) (c) nicotine, which has the composition \(74.0 \%\) C, \(8.65 \% \mathrm{H}\), and \(17.4 \% \mathrm{~N} .\)

Determine whether the statements given below are true or false. (a) The mass of an atom can have the unit mole. (b) In \(\mathrm{N}_{2} \mathrm{O}_{4}\), the mass of the oxygen is twice that of the nitrogen. (c) One mole of chlorine atoms has a mass of \(35.45 \mathrm{~g}\). (d) Boron has an average atomic mass of \(10.81\) amu. It has two isotopes, \(\mathrm{B}-10(10.01\) amu \()\) and \(\mathrm{B}-11(11.01 \mathrm{amu}) .\) There is more naturally occurring B-10 than B-11. (e) The compound \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{2} \mathrm{~N}\) has for its simplest formula \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{ON}_{1 / 2}\). (f) A 558.5-g sample of iron contains ten times as many atoms as \(0.5200 \mathrm{~g}\) of chromium. (g) If \(1.00\) mol of ammonia is mixed with \(1.00\) mol of oxygen the following reaction occurs, $$ 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) $$ All the oxygen is consumed. (h) When balancing an equation, the total number of moles of reactant molecules must equal the total number of moles of product molecules.

A compound \(\mathrm{YO}_{2}\) is \(50.0 \%\) (by mass) oxygen. What is the identity of Y? What is the molar mass of \(\mathrm{YO}_{2} ?\)

Calculate the molar masses (in grams per mole) of (a) cane sugar, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) (b) laughing gas, \(\mathrm{N}_{2} \mathrm{O}\). (c) vitamin A, \(\mathrm{C}_{20} \mathrm{H}_{30} \mathrm{O}\).

Calculate the molar masses (in grams per mole) of (a) gallium, Ga, a metal that literally melts in your hands. (b) plaster of paris, \(\mathrm{CaSO}_{4} \cdot \frac{1}{2} \mathrm{H}_{2} \mathrm{O}\), once used in making casts for broken bones. (c) benzoyl peroxide, \(\mathrm{C}_{14} \mathrm{H}_{10} \mathrm{O}_{4}\), the active ingredient in many lotions used to treat acne.
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