/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 55 Ammonia and oxygen react to form... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 5: Problem 55

Ammonia and oxygen react to form nitrogen and water. $$ 4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) $$ a. How many grams of \(\mathrm{O}_{2}\) are needed to react with \(13.6 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) ? b. How many grams of \(\mathrm{N}_{2}\) can be produced when \(6.50 \mathrm{~g}\) of \(\mathrm{O}_{2}\) reacts? c. How many grams of water are formed from the reaction of \(34.0 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) ?

Short Answer

Expert verified
a. 19.2 g of \(\mathrm{O}_2\) b. 3.79 g of \(\mathrm{N}_2\) c. 54.0 g of water.

Step by step solution

01

Write the balanced chemical equation

The balanced chemical equation is given by: \[ 4 \mathrm{NH}_{3}(g) + 3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{~N}_{2}(g) + 6 \mathrm{H}_{2} \mathrm{O}(g) \]
02

Calculate the molar masses

Determine the molar masses of all involved substances:\[\text{Molar mass of } \mathrm{NH}_{3} = (1 \times 14) + (3 \times 1) = 17 \text{ g/mol} \]\[\text{Molar mass of } \mathrm{O}_{2} = (2 \times 16) = 32 \text{ g/mol} \]\[\text{Molar mass of } \mathrm{N}_{2} = (2 \times 14) = 28 \text{ g/mol} \]\[\text{Molar mass of } \mathrm{H}_{2} \mathrm{O} = (2 \times 1) + (1 \times 16) = 18 \text{ g/mol} \]
03

Part A - Step 1: Calculate moles of \( \mathrm{NH}_{3} \)

Using the mass given for \(13.6\text{ g of }\mathrm{NH}_{3}\):\[ \text{Moles of } \mathrm{NH}_{3} = \frac{13.6 \text{ g}}{17 \text{ g/mol}} = 0.8 \text{ mol} \]
04

Part A - Step 2: Determine moles of \( \mathrm{O}_2 \) needed

Using the balanced equation, the mole ratio of \(\mathrm{NH}_{3}\) to \(\mathrm{O}_2\) is 4:3:\[ \text{Moles of } \mathrm{O}_2 \text{ needed} = 0.8 \text{ mol } \mathrm{NH}_{3} \times \frac{3 \text{ mol } \mathrm{O}_2}{4 \text{ mol } \mathrm{NH}_{3}} \ = 0.6 \text{ mol } \mathrm{O}_2 \]
05

Part A - Step 3: Calculate the mass of \( \mathrm{O}_2 \) needed

Using the molar mass of \(\mathrm{O}_2\), find the mass:\[ \text{Mass of } \mathrm{O}_2 = 0.6 \text{ mol} \times 32 \text{ g/mol} = 19.2 \text{ g} \]
06

Part B - Step 1: Calculate moles of \( \mathrm{O}_2 \)

Using the mass given for \(6.50\text{ g of } \mathrm{O}_2\):\[ \text{Moles of } \mathrm{O}_2 = \frac{6.50 \text{ g}}{32 \text{ g/mol}} = 0.203125 \text{ mol} \]
07

Part B - Step 2: Determine moles of \( \mathrm{N}_2 \) produced

Using the balanced equation, the mole ratio of \(\mathrm{O}_2\) to \(\mathrm{N}_2\) is 3:2:\[ \text{Moles of } \mathrm{N}_2 \text{ produced} = 0.203125 \text{ mol } \mathrm{O}_2 \times \frac{2 \text{ mol } \mathrm{N}_2}{3 \text{ mol } \mathrm{O}_2} = 0.1354167 \text{ mol } \mathrm{N}_2 \]
08

Part B - Step 3: Calculate the mass of \( \mathrm{N}_2 \) produced

Using the molar mass of \(\mathrm{N}_2\):\[ \text{Mass of } \mathrm{N}_2 = 0.1354167 \text{ mol} \times 28 \text{ g/mol} = 3.7916667 \text{ g} \]
09

Part C - Step 1: Calculate moles of \( \mathrm{NH}_3 \)

Using the mass given for \(34.0\text{ g of } \mathrm{NH}_3\):\[ \text{Moles of } \mathrm{NH}_3 = \frac{34.0 \text{ g}}{17 \text{ g/mol}} = 2.0 \text{ mol} \]
10

Part C - Step 2: Determine moles of water produced

Using the balanced equation, the mole ratio of \(\mathrm{NH}_3\) to \(\mathrm{H}_2 \mathrm{O}\) is 4:6:\[ \text{Moles of water produced} = 2.0 \text{ mol } \mathrm{NH}_3 \times \frac{6 \text{ mol } \mathrm{H}_2 \mathrm{O}}{4 \text{ mol } \mathrm{NH}_3} = 3.0 \text{ mol } \mathrm{H}_2 \mathrm{O} \]
11

Part C - Step 3: Calculate the mass of water produced

Using the molar mass of \(\mathrm{H}_2\mathrm{O}\):\[ \text{Mass of water} = 3.0 \text{ mol} \times 18 \text{ g/mol} = 54.0 \text{ g} \]

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Balanced Chemical Equations
To solve any stoichiometry problem, we start with a balanced chemical equation. This equation shows the reactants and products in the reaction, and the proportion in which they react. Balancing involves ensuring the number of atoms of each element is the same on both sides of the equation. For instance, in our example reaction: \[4 \mathrm{NH}_{3}(g) + 3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{~N}_{2}(g) + 6 \mathrm{H}_{2} \mathrm{O}(g) \] we see that 4 molecules of ammonia (\

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

In the mitochondria of human cells, energy for the production of ATP is provided by the oxidation and reduction reactions of the iron ions in the cytochromes in electron transport. Identify each of the following reactions as an oxidation or reduction: a. \(\mathrm{Fe}^{3+}+e^{-} \longrightarrow \mathrm{Fe}^{2+}\) b. \(\mathrm{Fe}^{2+} \longrightarrow \mathrm{Fe}^{3+}+e^{-}\)

Calculate the molar mass for each of the following compounds: a. \(\mathrm{KC}_{4} \mathrm{H}_{5} \mathrm{O}_{6}\) (cream of tartar) b. \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (rust) c. \(\mathrm{C}_{19} \mathrm{H}_{20} \mathrm{FNO}_{3}\) (Paxil, an antidepressant) d. \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) (antiperspirant) e. \(\mathrm{Mg}(\mathrm{OH})_{2}\) (antacid) f. \(\mathrm{C}_{16} \mathrm{H}_{19} \mathrm{~N}_{3} \mathrm{O}_{5} \mathrm{~S}\) (amoxicillin, an antibiotic)

a. Why is the following reaction called a combination reaction? $$ \mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \longrightarrow 2 \mathrm{HBr}(g) $$ b. Why is the following reaction called a double replacement reaction? $$ \mathrm{AgNO}_{3}(a q)+\mathrm{NaCl}(a q) \longrightarrow \mathrm{AgCl}(s)+\mathrm{NaNO}_{3}(a q) $$

Nitrogen gas reacts with hydrogen gas to produce ammonia by the following equation: $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) $$ a. If you have \(3.64 \mathrm{~g}\) of \(\mathrm{H}_{2}\), how many grams of \(\mathrm{NH}_{3}\) can be produced? b. How many grams of \(\mathrm{H}_{2}\) are needed to react with \(2.80 \mathrm{~g}\) of \(\mathrm{N}_{2}\) ? c. How many grams of \(\mathrm{NH}_{3}\) can be produced from \(12.0 \mathrm{~g}\) of \(\mathrm{H}_{2}\) ?

Write all the mole-mole factors for each of the following equations: a. \(2 \mathrm{Al}(s)+3 \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{AlCl}_{3}(s)\) b. \(4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Cl}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.