Chapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard

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1 Chapter 1 IB Chemistry Warm Ups Stoichiometry Mrs. Hilliard

2 Vocabulary 1. Atomic theory 2. Kelvin 3. Mole 4. Relative abundance 5. Molar Mass 6. Empirical formula 7. Molecular formula 8. Stoichiometry 9. Percentage yield 10.Limiting Reagent 11.Theoretical yield 12.Experimental yield 13.Standard Temperature and Pressure (STP) 14.Avogadro s law 15.Molar concentration

Vocabulary 1. Atomic theory- all matter is composed of atoms which cannot be created or destroyed during chemical reactions. 2. Kelvin- the SI unit for temperature. 3.

3 Vocabulary 1. Atomic theory- all matter is composed of atoms which cannot be created or destroyed during chemical reactions. 2. Kelvin- the SI unit for temperature. 3. Mole- the SI base unit used to measure the amount of a substance, equal to 6.02 x particles. 4. Relative abundance- a measure of the percentage that occurs in a sample of the element. 5. Molar Mass- the mass in grams of one mole of any substance. 6. Empirical formula- the simplest whole-number ratio of atoms of each element present in a compound. 7. Molecular formula- the actual number of atoms of each element in one molecule of a substance. 8. Stoichiometry- the quantitative method of examining the relative amounts of reactants and products. 9. Percentage yield- the ratio of actual yield to theoretical yield expressed as a percent. 10. Limiting Reagent- the reagent that is totally consumed during a chemical reaction, limits the extent of the reaction, and determines the amount of product. 11. Theoretical yield- the maximum amount of product that can be produced from a given amount of reactant. 12. Experimental yield- the actual amount of product that is produced in a chemical reaction. 13. Standard Temperature and Pressure (STP)- a standard temperature of 273K and pressure of 100kPa. 14. Avogadro s law- equal volumes of any gas measured at the same temperature and pressure contains the same number of molecules. 15. Molar concentration- the amount in mol of a substance dissolved in 1 dm 3 of solvent.

4 Balancing Equations 1. What is the sum of the coefficients for the equation when balancing using the smallest possible whole numbers? 2. What is the sum of all coefficients when the following equation is balanced using the smallest whole numbers? C 4 H 10 + O 2 CO 2 + H 2 O 3. 9 molecules of Calcium, Ca, and 6 molecules of chlorine gas, Cl 2 (g), were mixed together under conditions which allowed the reaction to go to completion, according to the following equation. The following diagram represents the mixture of reactants. Which reaction diagram represents the reaction mixture when the reaction was complete? Key: Purple= Chlorine Green= Calcium A B C D

Balancing Equations 1. What is the sum of the coefficients for the equation when balancing using the smallest possible whole numbers? 11 1 6 4 2.

5 Balancing Equations 1. What is the sum of the coefficients for the equation when balancing using the smallest possible whole numbers? What is the sum of all coefficients when the following equation is balanced using the smallest whole numbers? 2C 4 H O 2 8CO H 2 O = 33 total 3. 9 molecules of Calcium, Ca, and 6 molecules of chlorine gas, Cl 2 (g), were mixed together under conditions which allowed the reaction to go to completion, according to the following equation. The following diagram represents the mixture of reactants. Which reaction diagram represents the reaction mixture when the reaction was complete? Key: Purple= Chlorine Green= Calcium A B C D

6 Balancing Equations 4. What is the coefficient of Fe 3 O 4 when the following equation is balanced using the lowest whole numbers? Fe 3 O 4 + C Fe + CO 5. What is the coefficient for O 2 (g) when the equation for the combustion of 1 mole of propane is balanced? C 3 H 8 + O 2 CO 2 + H 2 O 6. Which coefficients would balance this equation? HCl + SnO 2 SnCl 2 + Cl 2 + H 2 O A B C D What is the coefficient for MgSO 4 (aq) when the following equation is balanced, using the smallest possible integers? Mg 3 N 2 + H 2 SO 4 MgSO 4 + (NH 4 ) 2 SO 4

Balancing Equations 4. What is the coefficient of Fe 3 O 4 when the following equation is balanced using the lowest whole numbers? 1 1Fe 3 O 4 + 4C 3Fe + 4CO 5.

7 Balancing Equations 4. What is the coefficient of Fe 3 O 4 when the following equation is balanced using the lowest whole numbers? 1 1Fe 3 O 4 + 4C 3Fe + 4CO 5. What is the coefficient for O 2 (g) when the equation for the combustion of 1 mole of propane is balanced? 3 1C 3 H 8 + 5O 2 3CO 2 + 4H 2 O 6. Which coefficients would balance this equation? HCl + SnO 2 SnCl 2 + Cl 2 + H 2 O A B C D What is the coefficient for MgSO 4 (aq) when the following equation is balanced, using the smallest possible integers? 3 _1_Mg 3 N 2 + _4_H 2 SO 4 _3_MgSO 4 + _1_(NH 4 ) 2 SO 4

8 Molar Mass 8. What is the approximate molar mass, in g mol -1, of MgSO 4 3 H 2 O? 9. The molar mass of a compound is approximately 125 g mol -1. Which formula is possible for this compound? A. KOH B. AgOH C. NaNO 3 D. MgO 10. Which non-metal forms an oxide XO 2 with a relative molecular mass of 46? A. Si B. S C. C D. N

Molar Mass 8. What is the approximate molar mass, in g mol -1, of MgSO 4 3 H 2 O? 174 9. The molar mass of a compound is approximately 125 g mol -1.

9 Molar Mass 8. What is the approximate molar mass, in g mol -1, of MgSO 4 3 H 2 O? The molar mass of a compound is approximately 125 g mol -1. Which formula is possible for this compound? A. KOH B. AgOH C. NaNO 3 D. MgO 10. Which non-metal forms an oxide XO 2 with a relative molecular mass of 46? A. Si B. S C. C D. N

10 Mole calculations 11. How many molecules are present in a drop of ethanol, C 2 H 5 OH, of mass 1.7 x 10-2 g? 12. What sample has the greatest mass? A. 2 mol of KOH B. 1 mol of SO 2 C. 4 mol of H 2 O D. 2 mol of Ar 13. What is the total number of carbon atoms contained in 1.5 mol of glucose, C 6 H 12 O 6?

Mole calculations 11. How many molecules are present in a drop of ethanol, C 2 H 5 OH, of mass 1.7 x 10-2 g? 2.2 x 10 20 12. What sample has the greatest mass? A. 2 mol of KOH B. 1 mol of SO 2 C.

11 Mole calculations 11. How many molecules are present in a drop of ethanol, C 2 H 5 OH, of mass 1.7 x 10-2 g? 2.2 x What sample has the greatest mass? A. 2 mol of KOH B. 1 mol of SO 2 C. 4 mol of H 2 O D. 2 mol of Ar 13. What is the total number of carbon atoms contained in 1.5 mol of glucose, C 6 H 12 O 6? 6 carbon atoms in glucose= 6 mol of C 1.5 mol x 6 mol C= 9 mol C x (6.02 x ) = 5.42 x 10 24

Mole calculations 14. What is the mass, in g, of one molecule of ethanol, C 2 H 5 OH? 15. What is the total number of nitrogen atoms in three mol of NH 4 NO 3? 16.

12 Mole calculations 14. What is the mass, in g, of one molecule of ethanol, C 2 H 5 OH? 15. What is the total number of nitrogen atoms in three mol of NH 4 NO 3? 16. What is the number of oxygen atoms in one mole of CuSO 4 4H 2 O? 17. Which sample has the greatest mass? A. 1.5 x 10 2 g of Copper B. 1.3 x atoms of gold C. 5.0 mol of Ne D. 6.0 x molecules of hydrogen

Mole calculations 14. What is the mass, in g, of one molecule of ethanol, C 2 H 5 OH? 7.68 x 10-23 15. What is the total number of nitrogen atoms in three mol of NH 4 NO 3? 3.61 x 10 24 16.

13 Mole calculations 14. What is the mass, in g, of one molecule of ethanol, C 2 H 5 OH? 7.68 x What is the total number of nitrogen atoms in three mol of NH 4 NO 3? 3.61 x What is the number of oxygen atoms in one mole of CuSO 4 4H 2 O? O= 8 in 1 mole 8 x (6.02 x )= 4.82 x Which sample has the greatest mass? A. 1.5 x 10 2 g of Copper B. 1.3 x atoms of gold C. 5.0 mol of Ne D. 6.0 x molecules of hydrogen

14 Mole calculations and empirical formulas 18. How many oxygen atoms are there in 0.30 mol of ethanoic acid, CH 3 COOH? 19. The relative molecular mass of a gas is 56 and its empirical formula is CH 2. What is the molecular formula of the gas? 20. Which is both an empirical and a molecular formula? A. CH 4 B. C 6 H 12 O 6 C. C 2 H 4 D. C 3 H 6

Mole calculations and empirical formulas 18. How many oxygen atoms are there in 0.30 mol of ethanoic acid, CH 3 COOH? 2 oxygen in 1 mol ethanoic acid 2 mol oxygen x 0.30 mol = 0.6 mol oxygen x (6.

15 Mole calculations and empirical formulas 18. How many oxygen atoms are there in 0.30 mol of ethanoic acid, CH 3 COOH? 2 oxygen in 1 mol ethanoic acid 2 mol oxygen x 0.30 mol = 0.6 mol oxygen x (6.02 x )= 3.61 x The relative molecular mass of a gas is 56 and its empirical formula is CH 2. What is the molecular formula of the gas? 56/14= 4 C 4 H Which is both an empirical and a molecular formula? A. CH 4 B. C 6 H 12 O 6 C. C 2 H 4 D. C 3 H 6

16 Molecular formulas and empirical formulas 21. On analysis, a compound with a molar mass 64 g mol -1 was found to contain 2 g of hydrogen, 14g of nitrogen and 16 g of oxygen. What is the molecular formula of the compound? 22. Equal masses of the metals Be, Mg, Au, and Ca are added to separate sample of excess HCl (aq). Which metal produces the greatest total volume of H 2 (g)? 23. Which compound has the empirical formula with the largest mass? A. C 2 H 6 B. C 2 H 12 C. C 2 H 4 D. C 3 H 6

Molecular formulas and empirical formulas 21. On analysis, a compound with a molar mass 64 g mol -1 was found to contain 2 g of hydrogen, 14g of nitrogen and 16 g of oxygen.

17 Molecular formulas and empirical formulas 21. On analysis, a compound with a molar mass 64 g mol -1 was found to contain 2 g of hydrogen, 14g of nitrogen and 16 g of oxygen. What is the molecular formula of the compound? 2 g H +14g N + 16g O = 32 g NO 64g/32g= 2 H 4 N 2 O Equal masses of the metals Be, Mg, Au, and Ca are added to separate sample of excess HCl (aq). Which metal produces the greatest total volume of H 2 (g)? Be 23. Which compound has the empirical formula with the largest mass? A. C 2 H 6 B. C 2 H 12 C. C 2 H 4 D. C 3 H 6

Molecular formulas, empirical formulas, Stoichi. 24.5.00 mol of a hydrocarbon with an empirical formula of CH 2 has a mass of 140 g. What is the molecular formula of this compound? 25.4.0 mol of aluminum reacts with oxygen to form aluminum oxide.

18 Molecular formulas, empirical formulas, Stoichi mol of a hydrocarbon with an empirical formula of CH 2 has a mass of 140 g. What is the molecular formula of this compound? mol of aluminum reacts with oxygen to form aluminum oxide. What is the amount of oxygen, in mol, needed for complete reaction? 26.What mass, in g, of hydrogen is formed when 2 mol of aluminum react with excess hydrochloric acid according to the following equation? 2 Al (s) + 6 HCl (aq) 2 AlCl 3 (aq) + 3 H 2 (g)

19 Molecular formulas, empirical formulas, Stoichi mol of a hydrocarbon with an empirical formula of CH 2 has a mass of 140 g. What is the molecular formula of this compound? 140g/ 14g= 10 mol/ 5 mol = 2 C 2 H mol of aluminum reacts with oxygen to form aluminum oxide. What is the amount of oxygen, in mol, needed for complete reaction? 3 mol O What mass, in g, of hydrogen is formed when 2 mol of aluminum react with excess hydrochloric acid according to the following equation? 2 Al (s) + 6 HCl (aq) 2 AlCl 3 (aq) + 3 H 2 (g) 2 mol Al x 3 mol H 2 / 2 mol Al x g H 2 / 1 mol H 2 = g H 2

20 Stoichiometry 27.What is the maximum mass, in g, of calcium oxide that can be obtained from the reaction of oxygen with 2.4 g of calcium? 28.Air bags in cars inflate when sodium azide decomposes to form sodium and nitrogen: 2NaN 3 (s) 2 Na (s) + 3 N 2 (g) Calculate the amount, in moles, of nitrogen gas produced by the decomposition of 4.6 mol of NaN 3 (s).

21 Stoichiometry 27.What is the maximum mass, in g, of calcium oxide that can be obtained from the reaction of oxygen with 2.4 g of calcium? 2.4 g Ca x 1/ 40.08g Ca x 2 mol CaO/2 mol Ca x 56 g CaO/ 1 mol = 3.4 g CaO 28.Air bags in cars inflate when sodium azide decomposes to form sodium and nitrogen: 2NaN 3 (s) 2 Na (s) + 3 N 2 (g) Calculate the amount, in moles, of nitrogen gas produced by the decomposition of 4.6 mol of NaN 3 (s). 6.9 mol N 2

Stoichiometry and Limiting Reagents 29. Chloroethene, C 2 H 3 Cl, reacts with oxygen according to the equation below. What is the amount, in mol, of H 2 O produced when 5.0 mol of C 2 H 3 Cl and 5.

22 Stoichiometry and Limiting Reagents 29. Chloroethene, C 2 H 3 Cl, reacts with oxygen according to the equation below. What is the amount, in mol, of H 2 O produced when 5.0 mol of C 2 H 3 Cl and 5.0 mol of O 2 are mixed together, and the above reaction goes to completion? 2 C 2 H 3 Cl (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O(g) + 2 HCl (g) dm 3 of carbon monoxide, CO (g), and 3 dm 3 of oxygen, O 2 (g), at the same temperature and pressure are mixed together. Assuming complete reaction according to the equation given, what is the maximum volume of carbon dioxide, CO 2 (g), in dm 3, that can be formed? 2 CO (g) + O 2 (g) 4 CO 2

23 Stoichiometry and Limiting Reagents 29. Chloroethene, C 2 H 3 Cl, reacts with oxygen according to the equation below. What is the amount, in mol, of H 2 O produced when 5.0 mol of C 2 H 3 Cl and 5.0 mol of O 2 are mixed together, and the above reaction goes to completion? 2 C 2 H 3 Cl (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O(g) + 2 HCl (g) 5.0 mol C 2 H 3 Cl x 2 mol H 2 O/ 2 mol C 2 H 3 Cl = 5 mol H 2 O 5.0 mol O 2 x 2 mol H 2 O/ 5 mol O 2 = 2 mol H 2 O 2.00 mol H 2 O dm 3 of carbon monoxide, CO (g), and 3 dm 3 of oxygen, O 2 (g), at the same temperature and pressure are mixed together. Assuming complete reaction according to the equation given, what is the maximum volume of carbon dioxide, CO 2 (g), in dm 3, that can be formed? 2 CO (g) + O 2 (g) 4 CO 2 7 dm 3 CO x 1 mol/ 22.4 dm 3 CO x 4 mol CO 2 / 2 mol CO x 22.4 dm 3 O 2 / 1mol = 14 dm 3 CO 2 3 dm 3 O 2 x 1 mol/ 22.4 dm 3 O 2 x 4 mol CO 2 / 1 mol O 2 x 22.4 dm 3 O 2 / 1mol = 12 dm 3 O 2 (limiting reagent)

Stoichiometry/ Limiting Reagents/ and Gases 31.What volume of sulfur trioxide, in cm 3, can be prepared using 60 cm 3 sulfur dioxide and 30 cm 3 oxygen gas by the following reaction?

24 Stoichiometry/ Limiting Reagents/ and Gases 31.What volume of sulfur trioxide, in cm 3, can be prepared using 60 cm 3 sulfur dioxide and 30 cm 3 oxygen gas by the following reaction? Assume all volumes are measured at the same temperature and pressure. 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) 32.What volume of carbon dioxide, in dm 3 under standard conditions, is formed when g of ethene (C 2 H 4, M r = 28.1) undergoes complete combustion? 33.The volume of an ideal gas at 35 C is increased from 3.00 dm 3 to 6.00 dm 3. At what temperature in C, will the gas have the original pressure?

25 Stoichiometry/ Limiting Reagents/ and Gases 31. What volume of sulfur trioxide, in cm 3, can be prepared using 60 cm 3 sulfur dioxide and 30 cm 3 oxygen gas by the following reaction? Assume all volumes are measured at the same temperature and pressure. 2 SO 2 (g) + O 2 (g) 2 SO 3 (g).06 dm 3 x 1mol/22.4 dm 3 x 2 mol/2 mol x 22.4 dm 3 =.06 dm 3 = 60 cm 3.03 dm 3 x 1mol/22.4 dm 3 x 2 mol/1 mol x 22.4 dm 3 =.06 dm 3 = 60 cm What volume of carbon dioxide, in dm 3 under standard conditions, is formed when g of ethene (C 2 H 4, M r = 28.1) undergoes complete combustion? 14g C 2 H 4, x 1mol/ 28.1g C 2 H 4 x 2 mol CO 2 / 1 mol C 2 H 4 x 22.4 dm 3 /1mol = 22.3 dm The volume of an ideal gas at 35 C is increased from 3.00 dm 3 to 6.00 dm 3. At what temperature in C, will the gas have the original pressure? V 1 /T 1 = V 2 /T dm 3 /308= 6.00 dm 3 /T 2 = = 343 C

26 Gases 34. Which sample of oxygen gas, O 2, contains the greatest number of oxygen molecules? A. 2.1 mol O 2 B. 2.1 x O 2 molecules C. 2.1 dm 3 O 2 at 1.01 x 10 5 Pa and 273 K D. 2.1 g O A fixed mass of gas has a certain volume at a temperature of 100 C. What temperature is required to double its volume while keeping the pressure constant?

Gases 34. Which sample of oxygen gas, O 2, contains the greatest number of oxygen molecules? A. 2.1 mol O 2 B. 2.1 x 10 23 O 2 molecules C. 2.1 dm 3 O 2 at 1.01 x 10 5 Pa and 273 K D. 2.1 g O 2 35.

27 Gases 34. Which sample of oxygen gas, O 2, contains the greatest number of oxygen molecules? A. 2.1 mol O 2 B. 2.1 x O 2 molecules C. 2.1 dm 3 O 2 at 1.01 x 10 5 Pa and 273 K D. 2.1 g O A fixed mass of gas has a certain volume at a temperature of 100 C. What temperature is required to double its volume while keeping the pressure constant? V 1 /T 1 = V 2 /T 2 1L/373K= 2L /T 2 = 746K

28 Solutions g of NaNO 3 (M r = 85) is dissolved in water to prepare 3.0 dm 3 of solution. What is the concentration of the resulting solution in mol dm -3? 37. The graph below represents the relationship between two variables in a fixed amount of gas. Which variables could be represented by each axis? X- axis Y-axis A. Pressure Volume B. Pressure Temperature C. Volume Temperature D. Temperature Volume Y x

Solutions 36. 2.6 g of NaNO 3 (M r = 85) is dissolved in water to prepare 3.0 dm 3 of solution. What is the concentration of the resulting solution in mol dm -3? 2.6 g x 1mol/85g NaNO 3 = 0.

29 Solutions g of NaNO 3 (M r = 85) is dissolved in water to prepare 3.0 dm 3 of solution. What is the concentration of the resulting solution in mol dm -3? 2.6 g x 1mol/85g NaNO 3 = 0.03 mol NaNO 3 M= mol/l M= 0.03mol/ 3.0 dm 3 = 0.01M 37. The graph below represents the relationship between two variables in a fixed amount of gas. Which variables could be represented by each axis? X- axis Y-axis A. Pressure Volume B. Pressure Temperature C. Volume Temperature D. Temperature Volume Y x

Solutions 2 38. 3.5 g of NH 3 are dissolved in H 2 O to prepare a 500 cm 3 solution. Which statements are correct? I. [NH 3 ] = 0.42 mol dm -3 II. NH 3 is the solute and H 2 O is the solution III.

30 Solutions g of NH 3 are dissolved in H 2 O to prepare a 500 cm 3 solution. Which statements are correct? I. [NH 3 ] = 0.42 mol dm -3 II. NH 3 is the solute and H 2 O is the solution III. The concentration of the solution is 17g dm What volume, in cm 3, of mol dm -3 HCl (aq) is required to neutralize 50.0 cm 3 of mol dm -3 Ca(OH) 2 (aq)? 40. Which statement about solutions is correct? I. The concentration of a solution is the amount of solvent dissolved in 1 dm 3 of solution. II. III. IV. When vitamin D dissolves in fat, vitamin D is the solvent and fat is the solute. An aqueous solution consists of water dissolved in a solute. In a solution of NaI in water, NaI is the solute and water is the solvent.

31 Solutions g of NH 3 are dissolved in H 2 O to prepare a 500 cm 3 solution. Which statements are correct? I. [NH 3 ] = 0.42 mol dm -3 II. NH 3 is the solute and H 2 O is the solution III. The concentration of the solution is 17g dm What volume, in cm 3, of mol dm -3 HCl (aq) is required to neutralize 50.0 cm 3 of mol dm -3 Ca(OH) 2 (aq)? 2HCl + Ca(OH) 2 2H 2 O + CaCl dm 3 x 1mol/22.4 dm 3 Ca(OH) 2 x 2 mol HCl/ 1 mol Ca(OH) 2 x 22.4 dm 3 /1mol =.1 dm 3 = 100 cm Which statement about solutions is correct? I. The concentration of a solution is the amount of solvent dissolved in 1 dm 3 of solution. II. III. IV. When vitamin D dissolves in fat, vitamin D is the solvent and fat is the solute. An aqueous solution consists of water dissolved in a solute. In a solution of NaI in water, NaI is the solute and water is the solvent.

32 Solutions 3 41.What will be the concentration of sulfate ions in mol dm -3 when 0.60 mol of Ca(SO 4 ) 2 is dissolved in water to give 100 cm 3 of aqueous solution? cm 3 of water is added to a solution of 200 cm 3 of 0.4 mol dm -3 sodium chloride. What is the concentration of sodium chloride in the new solution?

Solutions 3 41.What will be the concentration of sulfate ions in mol dm -3 when 0.60 mol of Ca(SO 4 ) 2 is dissolved in water to give 100 cm 3 of aqueous solution? M= mol/dm 3 M= 0.60 mol/.

33 Solutions 3 41.What will be the concentration of sulfate ions in mol dm -3 when 0.60 mol of Ca(SO 4 ) 2 is dissolved in water to give 100 cm 3 of aqueous solution? M= mol/dm 3 M= 0.60 mol/.1dm 3 = 6 x 2 molecules of SO 4 = cm 3 of water is added to a solution of 200 cm 3 of 0.4 mol dm -3 sodium chloride. What is the concentration of sodium chloride in the new solution? (0.4 mol dm -3 )(.200 dm 3 )=(.600 dm 3 )(M)= 0.13 mol dm -3

Solutions 4 43.What is the concentration of NaCl, in mol dm -3, when 10.0 cm 3 of 0.300 mol dm -3 NaCl solution is added to 40.0 cm 3 of 0.700 mol dm - 3 NaCl solution?

34 Solutions 4 43.What is the concentration of NaCl, in mol dm -3, when 10.0 cm 3 of mol dm -3 NaCl solution is added to 40.0 cm 3 of mol dm - 3 NaCl solution? 44.Which amount of the following compounds contains the least number of ions? 1. 1 mol Al 2 O mol CaCl mol NH 4 OH 4. 2 mol NaCl

35 Solutions What is the concentration of NaCl, in mol dm -3, when 10.0 cm 3 of mol dm -3 NaCl solution is added to 40.0 cm 3 of mol dm -3 NaCl solution? (0.700 mol dm -3 )(0.8 dm 3 ) + (0.300 mol dm -3 )(0.2 dm 3 )= Which amount of the following compounds contains the least number of ions? 1. 1 mol Al 2 O 3 Al 2 O 3 2Al + 3O 2 = 5 mol total 2. 2 mol CaCl 2 CaCl 2 1Ca + 1Cl 2 = 2 + 2= 4 mol total 3. 1 mol NH 4 OH NH 4 OH 1NH 4 + 1OH = 2 mol total 4. 2 mol NaCl 2NaCl 2Na + 1Cl 2 = 4+ 2 = 6 mol total

1. What is the sum of all coefficients when the following equation is balanced using the smallest possible whole numbers? D.

1. What is the sum of all coefficients when the following equation is balanced using the smallest possible whole numbers? A. 5 B. 7 C. 11 C 2 H 2 + O 2 CO 2 + H 2 O D. 13 2. 1.7 g of NaNO 3 (M r = 85)