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Name: ____________________________________________ Unit 1C Study Guide Minerals and Moles What is the role of chemistry in the life cycle of metals? 1 Date: ___________ Right Now: 1. If you have a dozen donuts how many do you have? 2. If you have four dozen donuts how many do you have? Quick Notes: 1. 1 mole = _________________________________________ 2. Define the unit, mole: __________________________________________________________________ ____________________________________________________________________________________ ____________________________________________________________________________________ _. 3. The number of particles in one mole, 6.02 x 1023, is known as ___________________________________. 4. Avogadro’s constant can be used to convert an amount of moles into ____________________________________________________________________________________ ___________________________________________________________________________________. 5. Define Molar Mass: __________________________________________________________________ ___________________________________________________________________________________. 6. What is the molar mass of Carbon: _________________________________________. 7. What is the molar mass of hydrogen peroxide: ___________________________________________. 2 Calculating Molar Mass Date: __________________ Chemical equations describe the relationships among atoms. In the lab, we measure substances with grams. Therefore we need to be able to count atoms with mass. The unit of a mole allows a chemist to scale up to measurable quantities allowing one to determine the amount of material they may need or may wish to produce. Converting between particles, moles, and mass is critical for chemists. At the center of this conversion is molar mass (MM). The molar mass of a substance is the mass of one mole (6.02 × 1023 units) of the substance. It allows one to covert from moles to mass which is measurable. MM has the label of “g/mol.” The Periodic Table lists the relative mass of a mole of that element. Therefore the molar mass of a compound is simply the sum of the atomic masses of its components. Example: What is the molar mass of water, H2O? Steps Involved List all of the elements Write down the subscript of each element (multiply the subscripts inside and outside of a parenthesis) Look up the atomic mass on the periodic table Multiply the subscript by the atomic mass Add up all of the products Element Subscript Atomic Mass Product Total = Try it! Find the molar mass of each of the following substances. 1. Nitrogen atom (N) 4. Sucrose (C12H22O12) Element Subscript Atomic Mass Product Element Subscript Atomic Mass Product Total = 2. Nitrogen Gas (N2) Element Subscript Atomic Mass Product Total = Total = 5. Magnesium phosphate Mg3(PO4)2 Element Subscript Atomic Mass 3. Sodium Chloride (NaCl) Element Subscript Atomic Mass Product Total = Total = 3 Product 4. potassium hydroxide: KOH 4 5 Date: ___________ Right Now: 1. Calculate the percent body fat of a 58-kg female distance runner who has 9.1-kg of body fat. 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EXTRA CREDIT Date: ______________ A mole is 6.02 x 1023 of anything. A mole of basketballs would just about fit into a ball bag the size of the Earth! However a mole of atoms can fit in the palm of your hands. Although calculations using the mole involve simple multiplication and division, they seem hard because scientific notation involving really large or really small numbers is used. Scientific notation is a short-hand way to express really big and really small numbers. The power of the ten tells you how many places to move the decimal point. If the power is positive, you move the decimal to the right; if the power is negative, you move the decimal to the left. When you use your calculator, you have to use the scientific notation button (EE). 1. Write the decimal form of the following numbers a. 2.0 x 102 cm _______________________ which is (larger, smaller) than zero b. 6.0 x 10-4 cm _______________________ which is (larger, smaller) than zero 2. Multiply 2.0 x 102 cm and 6.0 x 10-4 cm. When you use your calculator you type 2.0 EE 2 x 6.0 EE – 4. The EE button is usually above the “7” key. For graphing calculators only one E shows up on the screen. 3. Use your calculator to get the answer to: (3.1 x 103 g) x (12.1 x 106 g) = ____________ (6.5 x 10-10 g) 4. Spend exactly one minute making dots in the box below. 5. Now, count the dots. This is your rate in dots/minute. 6. Working at this rate, how many dots could you make in an hour? Convert dots/min to dots/hour. Show your work! 7. Working at this rate, how many dots could you make in a year? Convert dots/hour to dots/year. Show your work! 8. So how long would it take you to make a mole of dots? That’s 6.02 x 1023 dots! Show your work! 21 UNIT 1.C STATIONS REVIEW ANSWER SHEET STATION 1 STATION 2 STATION 3 STATION 4 STATION 5 STATION 6 22