. This is just a review of simpler concepts or older material that you should know to be successful. This does not include sample problems, see your study.

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Presentation transcript:

. This is just a review of simpler concepts or older material that you should know to be successful. This does not include sample problems, see your study guide for those!

 1 mole of NaCl would equal x atoms. (F…NaCl is compoud) True or False

 There are 22.4 Liters of gas in 1 mole of ANY gas at STP.  (T) True or False

 In order to find the molar mass of a compound, you need to use the periodic table to look up ATOMIC NUMBERS.  (F…need atomic masses) True or False

 1 mole of carbon is equal to grams.  (T) True or False

 Avogadro’s number is equal to 22.4 L.  (F it is * ) True or False

 1 mole of molecules is equal to Avogadro’s number of molecules  (T) True or False

 The mole is a handy conversion factor because it can be equal to so many different things.  (T) True or False

 It would be impossible to hold 1 mole of any substance in the palm of your hand.  (F you can hold a mole of H atoms) True or False

 The molar mass of Oxygen gas is grams  (F…Oxygen gas is diatomic so g) True or False

 How many sig figs in 12.00?.  (4 sig figs)

 How many sig figs in the number x  (4 sig figs)

 The formula for Iron (II) Nitride is...  (Fe 3 N 2 )

 In order to calculate from mass to moles, you must use Avogadro’s number  (F, you need molar mass) True or False

 In order to calculate from moles to liters, you must use the molar mass of the gas.  (F, you need the conversion 22.4L/1mol) True or False

 In order to calculate from atoms to moles, you will need to use 6.02 x   (T) True or False

 How many atoms 1 formula unit of NaOH.   (3)

 How many Cl atoms in 1 mole of Carbon Tetrachloride, CCl 4 ? Just show work.  ( 6.022x10 23 x 4)

 1 mole of iron atoms is enough for a large building.  (F, it is about the size of ping pong ball) True or False

 1 mole of xenon gas will take up much more space than 1 mole of He gas.  (F, 1 mole of all gas = 22.4 L ) True or False

 It is impossible to calculate the molar mass of a substance if you do not know its formula.  (T) True or False

 Percent composition is found by finding the molar mass of the element and dividing it by the total molar mass of the compound  (T) True or False

 C 2 H 2 O is an empirical formula  (T) True or False

 H 2 O 2 is an empirical formula  (F) True or False

 To find an empirical formula, convert % to g to mole and then find the whole number ratio.  (T) True or False