### Chemistry Exercises: Calculating Molecules and Mass#### Calculate the **number of molecules** in each of the following samples:6. 3.04 mol of C₈H₁₈7. 0.002 mol of aspirin, C₉H₈O₄#### Calculate the **mass** of each of the following samples: 8. 17.2 mol of CO₂ 9. 0.053 mol of (NH₄)₃PO₄ **Chemistry Mole Calculations**Calculate the **number of moles** in each of the following samples:10) \(3.69 \times 10^{24}\) atoms of uranium, U11) \(7.54 \times 10^{23}\) molecules of \(H_2O\)12) 76.9 g of \(BaSO_4\)13) 146.2 g of \(C_2H_5OH\)---**Methane Production from Carbon Dioxide Reaction**Under certain circumstances, carbon dioxide, \(CO_2(g)\), can be made to react with hydrogen gas, \(H_2(g)\), to produce methane, \(CH_4(g)\), and water vapor, \(H_2O(g)\):\[ CO_2(g) + 4H_2(g) \rightarrow CH_4(g) + 2H_2O(g) \]14) How many moles of methane are produced when 71.1 moles of carbon dioxide gas react?---**Graphical Illustration**:This section contains a detailed chemical equation representing a reaction where carbon dioxide reacts with hydrogen gas to produce methane and water vapor. This balanced equation is instrumental in stoichiometric calculations.

As per rules maximum the first three questions (6,7 and 8) can be answered

Answered: Calculate the number of molecules in…

Calculate the number of molecules in each of the following samples: 6) 3.04 mol of C8H18 7) 0.002 mol of aspirin, CgHgO4 Calculate the mass of each of the following samples: 8) 17.2 mol of CO2

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter8: Chemical Composition

Section: Chapter Questions

Problem 39QAP: Calculate the number of molecules present in each of the following samples. l type="a"> 4.75 mmol of...

See similar textbooks

Related questions

Q: Each step in the following process has a yield of 80.0%. CH, +4CL, + CCI, + 4HCH CCI, +2 HF =→…

A: The reactions given are, Given: Percent yield of both steps = 80 %. Moles of CH4 reacting = 5.5…

Q: How many molecules (not moles) of NH3NH3 are produced from 7.93×10−4 gg of H2H2?

Q: If 2 molecules of CH, react with 5 molecules of O,. determine the number of molecules of CO, that…

A: A balanced reaction is the reaction in which both sides of the reaction have equal numbers of each…

Q: g H2 is allowed to react with 9.89 gg N2, producing 1.84 g NH3. a) What is the theoretical yield in…

Q: Complete the following stoichiometric relationships. 1 mol NH3 contains ? mol N and ? mol H.

A: Given, No of mole of NH3 =1 mole

Q: 1 of 11 ► Vitamin C has the formula C H₂O₂. You burn 0.117 g of the compound in a combustion…

Q: 2. C,H,,0; + 6CO,– 6H,0 + 60, a) CH,0̟ to 0, b) o, to Co, c) H,0 to CO,

A: C6H12O6 + 6CO2 -----> 6H2O + 6O2 1mole 6mole 6mole 6mole

Q: 10. What are the empirical formulas of the compounds with the following compositions? (a) 40.1…

A: To determine the empirical formula of the compound with the given percent compositions, we need to…

Q: How many molecules (not moles) of NH3 are produced from 7.42×10−4 g of H2?

A: To obtain the number of molecules, first of all the reaction for the production of NH3 should be…

Q: If 4.11 mol of C,H, reacts with excess O,, how many moles of CO, will be produced by the following…

Q: A compound of mass 0.496g consisted of only C,H and O. It was completely burned in oxygen,producing…

Q: How many moles of NH, can be produced from 4.10 moles of nitrogen in the following reaction: N, (g)…

A: We will use mole concept to solve above problem.

Q: When copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment,…

Q: Balance the following chemical equation. NaN, - Na + Products Reactants Na = Na = N = N = Calculate…

A: The first question is about balancing the Chemical Equation and the second question is about…

Q: Fill in all 3 stoichiometric conversions that properly calculate how many grams of aspirin will be…

Q: How many molecules (not moles) of NH3NH3 are produced from 7.93×10−4 gg of H2H2?

A: The number of molecules are determined by the number of moles of compound. Number of moles of…

Q: A 3.0 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon…

Question

### Chemistry Exercises: Calculating Molecules and Mass

#### Calculate the **number of molecules** in each of the following samples:

6. 3.04 mol of C₈H₁₈

7. 0.002 mol of aspirin, C₉H₈O₄

#### Calculate the **mass** of each of the following samples:

8. 17.2 mol of CO₂

9. 0.053 mol of (NH₄)₃PO₄

**Chemistry Mole Calculations**

Calculate the **number of moles** in each of the following samples:

10) \(3.69 \times 10^{24}\) atoms of uranium, U

11) \(7.54 \times 10^{23}\) molecules of \(H_2O\)

12) 76.9 g of \(BaSO_4\)

13) 146.2 g of \(C_2H_5OH\)

---

**Methane Production from Carbon Dioxide Reaction**

Under certain circumstances, carbon dioxide, \(CO_2(g)\), can be made to react with hydrogen gas, \(H_2(g)\), to produce methane, \(CH_4(g)\), and water vapor, \(H_2O(g)\):

\[
CO_2(g) + 4H_2(g) \rightarrow CH_4(g) + 2H_2O(g)
\]

14) How many moles of methane are produced when 71.1 moles of carbon dioxide gas react?

---

**Graphical Illustration**:

This section contains a detailed chemical equation representing a reaction where carbon dioxide reacts with hydrogen gas to produce methane and water vapor. This balanced equation is instrumental in stoichiometric calculations.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Calculate the number of moles of carbon atoms present in eachof the following samples. l type="a"> 1.271 g of ethanol, C2H5OH i>3.982 g of 1 ,4-dichlorobenzene, C6H4Cl2 i>0.4438 g of carbon suboxide, C3O2 i>2.9 10 g of methylene chloride, CH2Cl2
Considering your answer to Exercise 79, which type of formula, empirical or molecular, can be obtained from elemental analysis that gives percent composition?
Use the average atomic masses given inside the front cover of this book to calculate the mass in grains of each of the following samples. l type='a'> 0.251 mole of lithium 1.51 moles of aluminum 8.75102 moles of lead 125 moles of chromium 4.25103 moles of iron 0.000105 mole of magnesium
f you have equal mole samples of NO2 and F2 , which of the following must be true? l type='a'> The number of molecules in each sample is the same. i>The number of atoms in each sample is the same. i>The masses of the samples are the same. i>6.0221023 molecules are present in each sample.
erhaps the most important concept in introductory chemistry concerns what a mole of a substance represents. The mole concept will come up again and again in later chapters in this book. What does one mole of a substance represent on a microscopic, atomic basis? What does one mole of a substance represent on a macroscopic, mass basis? Why have chemists defined the mole in this manner?
Calculate the percent by mass of the element listed first in the formulas for each of the following compounds. methane, CH4 sodium nitrate, NaNO3 carbon monoxide, CO nitrogen dioxide, NO2 1-octanol, C8H18O calcium phosphate, Ca3( PO4)2 3-phenyiphenol, C12H10O aluminum acetate, Al(C2H3O2)3
What information do we need to determine the molecular formula of a compound from the empirical formula?
e part of the problem-solving strategy for empirical formula determination is to base the calculation on 100 g of compound. What if you chose a mass other than 100 g? Would this work? What if you chose to base the calculation on 100 moles of compound? Would this work?
itamin B12 , cyancobalamin, is essential for human nutrition. Its molecular formula is C63H88CoN14O14P . A lack of this vita min in the diet can lead to anemia. Cyanocohalamin is the form of the vitamin found in vitamin supplements. l type='a'> What is the molar mass of cyanocobalamin to two decimal places? How many moles of cyanocohalamin molecules are present in 250 mg of cyanocobalamin? What is the mass of 0.60 mole of cyanocobalamin? How many atoms of hydrogen are in 1 .0 mole of cyanocobalamin? What is the mass of 1.0107 molecules of cyanocobalamin? What is the mass (in grams) of one molecule of cyanocobalamin?
3.35 Explain the concept of the mole in your own words.
3.78 Consider two samples of liquid: I mole of water (H2O) and 1 mole of ethanol. Answer each of the following questions. Note that none of these should require significant calculations. (a) Which sample contains more atoms? (b) Which sample contains more molecules? (c) Which sample has a larger mass?
Pain Relief Acetaminophen, a common aspirin substitute, has the formula C8H9NO2 . Determine the number of molecules of acetaminophen in a 500-mg tablet.