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1
**What is the % composition of carbon in benzene (C6H6)?**

2 slide

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**Total mass of carbon/Total mass of compound**

92%

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**How many grams of hydrogen are present in a 10**

How many grams of hydrogen are present in a 10.0 g sample of benzene (C6H6)? 2 slides

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1) 8% Hydrogen 2) 0.08 x 10.0 g = 0.800 g

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**What is the empirical formula for a compound that is 44% C, 26% N, & 30% O?**

3 slides

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**1) Assume 100. 0 g, so % is changed to grams**

1) Assume g, so % is changed to grams. 2) Convert each to moles by dividing by molar mass. 3) Divide each mole quantity by smallest mole quantity. (Rounding may occur.) C2NO

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**A compound has the empirical formula CH2O and molar mass of 120. 0 g**

A compound has the empirical formula CH2O and molar mass of g. What is its molecular formula? 3 slides

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**1) Mass of CH2O = 30 g/mol 2) 120/30 = 4 3) 4(CH2O) =**

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**What is the molarity of a solution that contains 104.4 g KCl in 250 mL?**

3 slides

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**1) Convert mass to moles 104. 4 g KCl x (1 mol/74. 4 g) = 1**

1) Convert mass to moles g KCl x (1 mol/74.4 g) = 1.40 mol KCl 2) Convert mL volume to L 250 mL x (1 L/1000 mL) = 0.25 L 3) Divide moles/volume = 5.67 M

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**What mass of KCl is dissolved in 500.0 mL to produce 2.50 M solution?**

3 slides

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1) Convert mL volume to L ( L) 2) Solve for moles L x (2.50 mol/L) = 1.25 mol 3) Convert moles to grams 1.25 mol x (74.4 g/mol) = 93 g

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**How many moles of CO2 are in 22.0 g?**

2 slides

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22.0 g x (1 mol/44.0 g) = 0.500 mol

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**How many moles of O2 are in 5.6 L?**

2 slides

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5.6 L x (1 mol/22.4 L) = 0.25 mol

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**What is the volume occupied by 56.0 g of N2 ?**

3 slides

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56.0 g x (1 mol/28.0 g) x (22.4 L/mol) = 44.8 L

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What is the density of O2 ? 2 slides

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32.0 g/ 22.4 L = 1.43 g/L

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**What is the molar mass of a gas that has a density of 2.25 g/L?**

2 slides

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(22.4 L/1 mol) x (2.25 g/L) = 50.4 g/mol

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**Use the following reaction: 4NH3 + 3O2 2N2 + 6H2O**

How many moles of oxygen, with excess ammonia, can produce 4 moles of nitrogen? 2 slides

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4 mol N2 x (3 mol O2 /2 mol N2) = 6 mol O2

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**Use the following reaction: 4NH3 + 3O2 2N2 + 6H2O**

How many grams of ammonia are needed to produce 14.0 g of N2? 3 slides

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**14.0 g N2 x (1 mol N2/28 g) x (4 mol NH3 /2 mol N2 ) x (17 g/1 mol) =**

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**Use the following reaction: 4NH3 + 3O2 2N2 + 6H2O**

How many grams of water are produced from 44.8 L of O2? 4 slides

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**44.8 L x (1 mol O2 /22.4 L) x (6 mol H2O/3 mol O2) x (18 g H2 O/1 mol) =**

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**Use the following reaction: 4NH3 + 3O2 2N2 + 6H2O**

If there are 5.00 moles of ammonia and 5.00 moles of oxygen, how many moles of nitrogen are produced? 4 slides

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**1) 5. 00 moles of each reactant is what you have 2) 5**

1) 5.00 moles of each reactant is what you have 2) 5.00 mol NH3 x (3 mol O2 /4 mol NH3 ) = 3.75 mol O2 is what I need 3) O2 : have (5.00 mol) > need (3.75 mol), so NH3 is limiting reactant 4) mol NH3 x (2 mol N2 / 4 mol NH3 ) = 2.50 mol N2

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**Use the following reaction: 4NH3 + 3O2 2N2 + 6H2O**

If excess oxygen reacts with 3.00 mol NH3 , what is the theoretical yield of H2O? 3 slides

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**3.00 mol NH3 x (6 mol H2O/4 mol NH3) x (18 g/mol) =**

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**If 70.0 g of water is produced, what is the percent yield?**

2 slides

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**1) 70.0 g = actual yield 2) 81.0 g = theoretical yield 3) [actual/theoretical] x 100 =**

86.4 %

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**Use the following reaction: Fe + 2HCl FeCl2 + H2**

If 20 atoms of iron are dropped into a beaker containing hydrochloric acid, how many molecules of hydrogen would be produced? 2 slides

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**20 Fe atoms x (1 H2 molecule/1 Fe atom) =**

20 H2 molecules

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Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Stoichiometry Stoichiometry - The study of quantities of materials consumed.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Stoichiometry Stoichiometry - The study of quantities of materials consumed.

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