So in our exploration of chemistry, eventually, we're going to reach a topic called dimensional analysis, which can be thought of as more complex word problems where our job is to isolate a particular unit. Now a key component of dimensional analysis is the conversion factor. The conversion factor can be thought of as just simply a ratio or fraction that ties together two different units. Now, for example, we can say that a day is composed of 24 hours. So this is saying that one day equals 24 hours. It is a conversion factor because it is tying together day as a unit with hours, which is a different unit. To make it into a conversion factor, we have to change it into a fractional ratio. So we can set it up as one day is 24 hours or 24 hours is one day. There, we're combining these two different types of units and showing their relationship to one another. Besides the conversion factor, we can also have a given amount. Now a given amount is just a value containing only one unit. For example, we spent 3 hours studying chemistry today, and trust me, there will be times when you're spending that many hours or more in preparation for a quiz or exam. So here, our given amount is just 3 hours. I am not tying those 3 hours to any other units. So it's just 3 hours by itself. And it's these combinations of conversion factors and given amounts that will be vital in our understanding of dimensional analysis. But, again, before we get to dimensional analysis, let's look over some questions where it's just our responsibility to help identify the conversion factors and given amounts within the particular question. So click on the next video and let's get started.

- 1. Matter and Measurements4h 29m
- What is Chemistry?5m
- The Scientific Method9m
- Classification of Matter16m
- States of Matter8m
- Physical & Chemical Changes19m
- Chemical Properties8m
- Physical Properties5m
- Intensive vs. Extensive Properties13m
- Temperature (Simplified)9m
- Scientific Notation13m
- SI Units (Simplified)5m
- Metric Prefixes24m
- Significant Figures (Simplified)11m
- Significant Figures: Precision in Measurements7m
- Significant Figures: In Calculations19m
- Conversion Factors (Simplified)15m
- Dimensional Analysis22m
- Density12m
- Specific Gravity9m
- Density of Geometric Objects19m
- Density of Non-Geometric Objects9m

- 2. Atoms and the Periodic Table5h 23m
- The Atom (Simplified)9m
- Subatomic Particles (Simplified)12m
- Isotopes17m
- Ions (Simplified)22m
- Atomic Mass (Simplified)17m
- Atomic Mass (Conceptual)12m
- Periodic Table: Element Symbols6m
- Periodic Table: Classifications11m
- Periodic Table: Group Names8m
- Periodic Table: Representative Elements & Transition Metals7m
- Periodic Table: Elemental Forms (Simplified)6m
- Periodic Table: Phases (Simplified)8m
- Law of Definite Proportions9m
- Atomic Theory9m
- Rutherford Gold Foil Experiment9m
- Wavelength and Frequency (Simplified)5m
- Electromagnetic Spectrum (Simplified)11m
- Bohr Model (Simplified)9m
- Emission Spectrum (Simplified)3m
- Electronic Structure4m
- Electronic Structure: Shells5m
- Electronic Structure: Subshells4m
- Electronic Structure: Orbitals11m
- Electronic Structure: Electron Spin3m
- Electronic Structure: Number of Electrons4m
- The Electron Configuration (Simplified)22m
- Electron Arrangements5m
- The Electron Configuration: Condensed4m
- The Electron Configuration: Exceptions (Simplified)12m
- Ions and the Octet Rule9m
- Ions and the Octet Rule (Simplified)8m
- Valence Electrons of Elements (Simplified)5m
- Lewis Dot Symbols (Simplified)7m
- Periodic Trend: Metallic Character4m
- Periodic Trend: Atomic Radius (Simplified)7m

- 3. Ionic Compounds2h 18m
- Periodic Table: Main Group Element Charges12m
- Periodic Table: Transition Metal Charges6m
- Periodic Trend: Ionic Radius (Simplified)5m
- Periodic Trend: Ranking Ionic Radii8m
- Periodic Trend: Ionization Energy (Simplified)9m
- Periodic Trend: Electron Affinity (Simplified)8m
- Ionic Bonding6m
- Naming Monoatomic Cations6m
- Naming Monoatomic Anions5m
- Polyatomic Ions25m
- Naming Ionic Compounds11m
- Writing Formula Units of Ionic Compounds7m
- Naming Ionic Hydrates6m
- Naming Acids18m

- 4. Molecular Compounds2h 18m
- Covalent Bonds6m
- Naming Binary Molecular Compounds6m
- Molecular Models4m
- Bonding Preferences6m
- Lewis Dot Structures: Neutral Compounds (Simplified)8m
- Multiple Bonds4m
- Multiple Bonds (Simplified)6m
- Lewis Dot Structures: Multiple Bonds10m
- Lewis Dot Structures: Ions (Simplified)8m
- Lewis Dot Structures: Exceptions (Simplified)12m
- Resonance Structures (Simplified)5m
- Valence Shell Electron Pair Repulsion Theory (Simplified)4m
- Electron Geometry (Simplified)8m
- Molecular Geometry (Simplified)11m
- Bond Angles (Simplified)11m
- Dipole Moment (Simplified)15m
- Molecular Polarity (Simplified)7m

- 5. Classification & Balancing of Chemical Reactions3h 17m
- Chemical Reaction: Chemical Change5m
- Law of Conservation of Mass5m
- Balancing Chemical Equations (Simplified)13m
- Solubility Rules16m
- Molecular Equations18m
- Types of Chemical Reactions12m
- Complete Ionic Equations18m
- Calculate Oxidation Numbers15m
- Redox Reactions17m
- Spontaneous Redox Reactions8m
- Balancing Redox Reactions: Acidic Solutions17m
- Balancing Redox Reactions: Basic Solutions17m
- Balancing Redox Reactions (Simplified)13m
- Galvanic Cell (Simplified)16m

- 6. Chemical Reactions & Quantities2h 35m
- 7. Energy, Rate and Equilibrium3h 46m
- Nature of Energy6m
- First Law of Thermodynamics7m
- Endothermic & Exothermic Reactions7m
- Bond Energy14m
- Thermochemical Equations12m
- Heat Capacity19m
- Thermal Equilibrium (Simplified)8m
- Hess's Law23m
- Rate of Reaction11m
- Energy Diagrams12m
- Chemical Equilibrium7m
- The Equilibrium Constant14m
- Le Chatelier's Principle23m
- Solubility Product Constant (Ksp)17m
- Spontaneous Reaction10m
- Entropy (Simplified)9m
- Gibbs Free Energy (Simplified)18m

- 8. Gases, Liquids and Solids3h 25m
- Pressure Units6m
- Kinetic Molecular Theory14m
- The Ideal Gas Law18m
- The Ideal Gas Law Derivations13m
- The Ideal Gas Law Applications6m
- Chemistry Gas Laws16m
- Chemistry Gas Laws: Combined Gas Law12m
- Standard Temperature and Pressure14m
- Dalton's Law: Partial Pressure (Simplified)13m
- Gas Stoichiometry18m
- Intermolecular Forces (Simplified)19m
- Intermolecular Forces and Physical Properties11m
- Atomic, Ionic and Molecular Solids10m
- Heating and Cooling Curves30m

- 9. Solutions4h 10m
- Solutions6m
- Solubility and Intermolecular Forces18m
- Solutions: Mass Percent6m
- Percent Concentrations10m
- Molarity18m
- Osmolarity15m
- Parts per Million (ppm)13m
- Solubility: Temperature Effect8m
- Intro to Henry's Law4m
- Henry's Law Calculations12m
- Dilutions12m
- Solution Stoichiometry14m
- Electrolytes (Simplified)13m
- Equivalents11m
- Molality15m
- The Colligative Properties15m
- Boiling Point Elevation16m
- Freezing Point Depression9m
- Osmosis16m
- Osmotic Pressure9m

- 10. Acids and Bases3h 29m
- Acid-Base Introduction11m
- Arrhenius Acid and Base6m
- Bronsted Lowry Acid and Base18m
- Acid and Base Strength17m
- Ka and Kb12m
- The pH Scale19m
- Auto-Ionization9m
- pH of Strong Acids and Bases9m
- Acid-Base Equivalents14m
- Acid-Base Reactions7m
- Gas Evolution Equations (Simplified)6m
- Ionic Salts (Simplified)23m
- Buffers25m
- Henderson-Hasselbalch Equation16m
- Strong Acid Strong Base Titrations (Simplified)10m

- 11. Nuclear Chemistry56m
- BONUS: Lab Techniques and Procedures1h 38m
- BONUS: Mathematical Operations and Functions47m
- 12. Introduction to Organic Chemistry1h 34m
- 13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
- 14. Compounds with Oxygen or Sulfur1h 6m
- 15. Aldehydes and Ketones1h 1m
- 16. Carboxylic Acids and Their Derivatives1h 11m
- 17. Amines38m
- 18. Amino Acids and Proteins1h 51m
- 19. Enzymes1h 37m
- 20. Carbohydrates1h 46m
- Intro to Carbohydrates4m
- Classification of Carbohydrates4m
- Fischer Projections4m
- Enantiomers vs Diastereomers8m
- D vs L Enantiomers8m
- Cyclic Hemiacetals8m
- Intro to Haworth Projections4m
- Cyclic Structures of Monosaccharides11m
- Mutarotation4m
- Reduction of Monosaccharides10m
- Oxidation of Monosaccharides7m
- Glycosidic Linkage14m
- Disaccharides7m
- Polysaccharides7m

- 21. The Generation of Biochemical Energy2h 8m
- 22. Carbohydrate Metabolism2h 22m
- 23. Lipids2h 26m
- Intro to Lipids6m
- Fatty Acids25m
- Physical Properties of Fatty Acids6m
- Waxes4m
- Triacylglycerols12m
- Triacylglycerol Reactions: Hydrogenation8m
- Triacylglycerol Reactions: Hydrolysis13m
- Triacylglycerol Reactions: Oxidation7m
- Glycerophospholipids15m
- Sphingomyelins13m
- Steroids15m
- Cell Membranes7m
- Membrane Transport10m

- 24. Lipid Metabolism1h 45m
- 25. Protein and Amino Acid Metabolism1h 37m
- 26. Nucleic Acids and Protein Synthesis2h 54m
- Intro to Nucleic Acids4m
- Nitrogenous Bases16m
- Nucleoside and Nucleotide Formation9m
- Naming Nucleosides and Nucleotides13m
- Phosphodiester Bond Formation7m
- Primary Structure of Nucleic Acids11m
- Base Pairing10m
- DNA Double Helix6m
- Intro to DNA Replication20m
- Steps of DNA Replication11m
- Types of RNA10m
- Overview of Protein Synthesis4m
- Transcription: mRNA Synthesis9m
- Processing of pre-mRNA5m
- The Genetic Code6m
- Introduction to Translation7m
- Translation: Protein Synthesis18m

# Conversion Factors (Simplified) - Online Tutor, Practice Problems & Exam Prep

Dimensional analysis involves using conversion factors, which are ratios that relate different units, to solve complex problems. Key conversion factors to memorize include: 1 inch = 2.54 cm, 1 yard = 3 feet, and 1 liter = 1.057 quarts. Understanding given amounts, such as 3 hours, is essential for applying these conversion factors effectively. Mastery of these concepts is crucial for tackling various chemistry problems, including those related to mass, volume, and length.

**Conversion Factors** are used to tie together 2 different units.

## Conversion Factors & Given Amounts

### Conversion Factors (Simplified) Concept 1

#### Video transcript

The given amount contains one unit type and the conversion factor connects two different units together.

### Conversion Factors (Simplified) Example 1

#### Video transcript

So Klutch's ugly but good chocolate chip cookie recipe is always a hit at our office parties. My budget is $80. The recipe makes 18 servings for the party. Each serving requires 8 chocolate truffle chips at a cost of 50¢ per 5 chocolate truffle chips. From the information provided, determine the given amount and all conversion factors. Now our given amount, remember, that's when we have only 1 unit. That's it. Our given amount has to be the $80 because they're not saying $80 connected to some other units. It's just dollars by itself. The conversion factors though, these are when we have 2 units bonded together, 2 different units bonded together. This one is a little trickier. If we look at the sentence after the $80 budget, they tell me the recipe makes 18 servings. So that there is a conversion factor. The conversion factor is 1 recipe has 18 servings. Because recipe and servings are 2 different units, let's look at the next line. Each serving requires 8 chocolate truffle chips. So servings, each serving has this many chocolate truffle chips. That's also a conversion factor because it's one serving is 8 chocolate truffle chips, which I'll abbreviate as CTC. They tell me that it is 50¢ per 5. The word "per" there definitely is a big help because it tells us that that amount of 50¢ and 5 are connected together. So then that would be our last conversion factor. So 50¢ for every 5 chocolate truffle chips. Eventually, when we move on to dimensional analysis later on, we'll see how these units cancel out with one another and help us isolate our final value. But remember, a given amount has 1 unit, a conversion factor is 2 different units mixed together. Now that we've seen this first example, let's continue onward with practice questions.

### Conversion Factors (Simplified) Concept 2

#### Video transcript

Now remember that a conversion factor deals with 2 units combined together. And when it comes to our conversion factors, the most common ones involve length, volume, or mass. Now, remember, we see a lot of different convergent factors here, but only the ones that are highlighted in purple you should commit to memory. The others will be given to you within the work problem that you're solving or some type of formula sheet. So let's start out with length. We know here that 1 inch is 2.54 cm. So we need to commit that to memory. Next, we can say that 1 yard is equal to 3 feet. One kilometer is 0.6214 miles. One meter is 1.094 yards, and 1 mile is 5,280 feet. For volume, the first two in purple are the ones you need to memorize, and that's 1 mL=1cm3, and 1 mL=1 cc. Next, we can say that 1 L=1.057 quarts, 1 L=1dm3, 1 fl oz=29.574 mL, and 1 gallon=3.785 L. For mass, tablets can come in different types of masses. The most common one is when one tablet is equal to 254 mg. Now, if they're talking about a tablet and they don't give you the mass, usually they mean a 250 milligram tablet. But check the question. Sometimes the tablet may be a different mass and they'll tell you that new mass associated with it. Alright. Next, we can say here that 1 lb=approximately454 g, 1 oz=28.35 g, and then finally, 1 kg=2.205 lb. So these are all types of common conversion factors that you'll come into contact with when doing different types of problems. Now remember, only the ones that are highlighted in purple, you should commit to memory.

### Conversion Factors (Simplified) Example 2

#### Video transcript

So here in this example question, it says while packing for a trip to Spain, a traveler wishes to weigh their luggage to make sure it doesn't exceed 23 kilograms. Unfortunately, their bathroom scale, for some reason, can only weigh in ounces. What conversion factors could they use to determine the mass of their luggage? Alright. So in this question, they're telling us that we don't want to go over 23 kilograms. Since kilograms are not attached to any other unit, 23 must represent our given amount. We have 23 kilograms, and what we need to do here is we need to find a way of converting these kilograms into ounces. Because we're dealing with mass values, we know that the conversion factors we're going to have to utilize have to do with mass in some way. Now, we've kind of done this before when we did metric prefix conversions. We want to get rid of these kilograms. To get rid of these kilograms, we'd have to place them here on the bottom. And if we go to the conversion factors for mass, we see that kilograms are right here, and we want to get to ounces. Well, kilograms are attached to grams by the metric prefix conversion, and we want to go to grams because grams are connected to ounces. Here, we're not going to solve for it. Here, we're just setting up the conversion factors necessary for us to isolate ounces. We're just getting the hang of this whole idea of conversion factors, given amounts, and their general positions in dimensional analysis. Don't worry about calculations yet. We're kind of slowly building our way up to questions like that. Alright. So kilograms go here, which will be connected to grams over here. Since this is a metric prefix conversion, remember that the coefficient of 1 is always associated or always next to the metric prefix. And remember, from our metric prefix multipliers, 1 kilo is 10^{3}. So we started out here by using our conversion factor. So now kilograms are gone. Now we have grams. Grams are connected to ounces. So we're going to bring this conversion factor in. Right? So we're going to say here, that grams go here, ounces go here, and the conversion factor up here says that 1 ounce is equal to 28.35 grams. Grams would cancel out, and we'd be left with ounces. So for this question, the conversion factors that we'd have to use are this metric prefix conversion factor of 10^{3} grams over 1 kilogram and 1 ounce over 28.35 grams. Those are the two conversion factors we'd utilize to safely convert kilograms into ounces. We see that in everyday processes, we can incorporate chemistry and we can incorporate these different types of mathematical operations. Now that we've seen this example, let's move on and continue our discussion on conversion factors and given amounts.

A patient has approximately 83 mL of blood pumping by their heart at each beat. By assuming they have a pulse of 75 beats per minute it is calculated that the patient pumps 8.964 x 10^{6} mL in one day. Identify the given amount and all conversion factors.

#### Problem Transcript

For 7 hours, an intravenous bag delivers medication to a patient at a rate of 2.75 drops a second with a mass of 42 mg per drop. Identify the given amount and all conversion factors.

The dispensing of prescription drugs are usually prescribed in units of mg per kg of body weight. A new prescription drug has a recommended dosage of 11 mg/kg. A 75 lb child requires three tablets each weighing 125 mg for their recommended dosage. Identify the given amount and all conversion factors.

#### Problem Transcript

## Do you want more practice?

### Here’s what students ask on this topic:

What is a conversion factor in chemistry?

A conversion factor in chemistry is a ratio or fraction that relates two different units, allowing you to convert a quantity expressed in one unit to another unit. For example, the conversion factor between inches and centimeters is 1 inch = 2.54 cm. This means you can convert inches to centimeters by multiplying by 2.54, or convert centimeters to inches by dividing by 2.54. Conversion factors are essential in dimensional analysis, which involves solving complex problems by isolating and converting units.

How do you use conversion factors in dimensional analysis?

In dimensional analysis, conversion factors are used to convert a given amount from one unit to another. You start with the given amount, multiply by the appropriate conversion factor(s), and ensure that units cancel out correctly. For example, to convert 5 miles to kilometers, you use the conversion factor 1 mile = 1.60934 km. Multiply 5 miles by 1.60934 km/mile to get 8.0467 km. This method helps solve complex problems by breaking them down into simpler unit conversions.

What are some common conversion factors for length, volume, and mass?

Common conversion factors for length include 1 inch = 2.54 cm, 1 yard = 3 feet, and 1 mile = 5280 feet. For volume, key conversion factors are 1 milliliter = 1 cm^{3}, 1 liter = 1.057 quarts, and 1 gallon = 3.785 liters. For mass, important conversion factors are 1 pound = 454 grams, 1 ounce = 28.35 grams, and 1 kilogram = 2.205 pounds. Memorizing these conversion factors is crucial for solving various chemistry problems involving different units.

Why is it important to memorize certain conversion factors?

Memorizing certain conversion factors is important because it allows you to quickly and accurately convert between units without needing to look up the values each time. This is especially useful in exams and real-world applications where time is limited. Key conversion factors, such as 1 inch = 2.54 cm and 1 liter = 1.057 quarts, are frequently used in chemistry problems, making them essential for efficient problem-solving and dimensional analysis.

Can you provide an example of a dimensional analysis problem using conversion factors?

Sure! Let's convert 10 kilometers to miles. The conversion factor is 1 kilometer = 0.6214 miles. Start with the given amount: 10 kilometers. Multiply by the conversion factor: 10 km × 0.6214 miles/km. The kilometers cancel out, leaving you with 6.214 miles. So, 10 kilometers is equal to 6.214 miles. This process demonstrates how dimensional analysis uses conversion factors to switch between units.

### Your GOB Chemistry tutor

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