Stoichiometry Worksheet 1 (Mole-Mole Conversions)



Stoichiometry Worksheet 1 (Mole-Mole Conversions)

1. The combustion of the organic fuel, decane, is outlined in the chemical equation below. You must balance the equation in order to answer the subsequent questions a-c.

____C10H22 + ____O2 ____CO2 + ____H2O

a. How many moles of CO2 are produced if 5.0 moles of C10H22 react with an

excess of O2?

b. How many moles of O2 react with 0.75 moles of C10H22?

c. How many moles of O2 would be required to produce 4.0 moles of H2O?

2. Use the following equation to solve the problems below:

3 SiO2 + 4 Al 3 Si + 2 Al2O3

a. If 6.0 moles of SiO2 react, how many moles of:

i. Al react?

ii. Si are produced?

iii. Al2O3 are produced?

b. If 2.5 moles of Al2O3 are produced, how many moles of:

i. Al react?

ii. SiO2 react?

3. Given the following reaction:

3 H2 + N2 2 NH3

How many moles of nitrogen gas are required to produce 4.18 moles of ammonia?

4. Using the following unbalanced equation:

____FeS2 + ____O2 ____Fe2O3 + ____SO2

a. If 12 moles of FeS2 react, how many moles of:

i. Fe2O3 are produced?

ii. O2 react?

b. How many moles of FeS2 are needed to produce 8.6 moles of SO2?

Stoichiometry Worksheet #2 (mole-mass, mass-mole problems)

1. N2 + 2O2 → N2O4

a. If 15.0g of N2O4 was produced, how many moles of O2 were required?

b. If 4.0x10-3 moles of oxygen reacted, how many grams of N2 were needed?

2. K3PO4 + Al(NO3)3 → 3KNO3 + AlPO4

a. What is the mass of potassium nitrate that is produced when 2.04 moles of potassium phosphate react?

b. If 5.80g of aluminum phosphate are formed, how many moles of aluminum nitrate reacted?

3. CaC2 + 2H2O → Ca(OH)2 + C2H2

a. If you have 5.50 mol of CaC2, how much C2H2 do you get?

b. How many moles of water are needed when 65.0g of CaC2 have reacted?

4. In photosynthesis, water reacts with carbon dioxide to give oxygen and glucose (C6H12O6). Write and balance the chemical equation. How many moles of CO2 are required to make 120.0g of glucose?

5. _____NaClO3→ ____NaCl + ____O2 Balance and answer the following questions.

a. How many grams of NaCl are produced when 20.00mol of NaClO3 react?

b. How many moles of O2 are produced when 40g of NaCl are formed?

6. 8Fe + S8 → 8FeS

How many moles of FeS are produced when 0.93g of S8 react?

7. Write a balanced chemical equation to represent the combustion of decane (C10H22). How many moles of water will form with the combustion of 540.4g of decane?

8. Balance and then answer the following questions:

_____NH3(g) + ______O2(g) → 4NO(g) + ____H2O(g)

a. How many moles of NO are formed if 824g of NH3 react?

b. How many grams of water are formed if 2.55 mol of ammonia are oxidized?

9. Mercury (II) oxide decomposes into mercury and oxygen gas.

a. Write and balance the equation.

b. How many moles of mercury (II) oxide are needed to produce 125g of oxygen?

c. How many grams of mercury are produced if 24.5 moles of mercury (II) oxide decomposes?

10. Cu + 2AgNO3 → Cu(NO3)2 + 2Ag

How many moles of Cu are needed to react with 3.50g of AgNO3?

Stoichiometry Worksheet #3 (mass-mass problems)

1. Li3N(s) + 3H2O(l) → NH3(g) + 3LiOH(aq)

a. What mass of lithium hydroxide are produced when 0.38g of lithium nitride react?

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b. How many grams of lithium nitride would react with 4.05g of H2O?

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2. __NaI(s) + __Cl2(g) → __NaCl(s) + __I2(g) Balance and answer the following questions.

a. What mass of sodium chloride is produced when 0.294g of sodium iodide react?

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b. If 5.80g of iodine is formed, what is the mass of sodium iodide that reacted?

3. In the combustion of 54.50g of butane (C4H6), how many grams of CO2 are produced? Write and balance the equation before solving.

4. In the following unbalanced equation,

___ FeS2 + ___O2 → ___Fe2O3 + ___SO2

a. How many grams of iron (IV) sulphide are used when 9.0g of O2 react?

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b. What is the mass of iron (III) oxide produced when 25.0g of iron (IV) sulphide are used?

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5. Write and balance the double replacement reaction between lead (II) nitrate and sodium chloride. What is the mass of each product when 50.0g of lead (II) nitrate react?

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6. Cu + 2AgNO3 → 2Ag + Cu(NO3)2

How many grams of silver are produced when 36.92g of copper react?

7. ___Al2(SO4)3 + ___Ca(OH)2 →___Al(OH)3 + ___CaSO4

Balance and answer the following questions.

a. What mass of aluminum (III) hydroxide are produced if 165.7g of aluminum (III) sulfate react?

b. How many grams of calcium hydroxide are needed to form 6.35g of calcium sulphate?

8. Balance and then answer the following questions:

__F2 +__AlBr3 → __Br2 + __AlF3

a. If 8.4g of aluminum bromide react, how many grams of bromine are produced?

b. If 90 g of aluminum fluoride are made, how many grams of fluorine have reacted?

9. 2 KI + Pb(NO3)2 → PbI2 + 2KNO3

a. Calculate the mass of PbI2 produced by reacting 30.0g KI.

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b. What mass of Pb(NO3)2 is required to make 50.69g of KNO3?

10. Write and balance the single replacement between aluminum and zinc chloride. What is the combined mass of the products when 3.0g of zinc chloride react?

Stoichiometry Worksheet 4 (Mass-Volume/Volume-Volume/Density/Molecules Problems)

1. The corrosion (rusting) of iron is represented as follows: (Density (Fe) = 7.86 g/cm3)

3 O2 (g) + 4 Fe(s) 2 Fe2O3 (s) Assume STP

a. What volume of Oxygen gas would be required to produce 16.0 g of Fe2O3?

b. What mass of Iron would be required to react with 10.0 L of O2 gas?

c. How many molecules of oxygen would be required to completely react with

6.50 g of Iron?

d. What volume of Iron would be required to produce 6.43 x 1024 molecules of

Iron III oxide if it was reacted with an excess of oxygen gas?

2. Given the following equation:

3 NO2 (g) + H2O(l) 2 HNO3 (aq) + NO(g) Assume STP

a. What mass of water is required to react with 15.5 L of Nitrogen dioxide?

b. What volume of Nitrogen monoxide would be produced from 100.0 g of water?

c. If 42.0 L of NO(g) is produced, what volume of NO2 (g) reacted?

d. How many hydrogen atoms would be required to react with an excess of

Nitrogen dioxide to produce 46.0 L of Nitrogen monoxide?

3. When Magnesium reacts with Nitric Acid, Hydrogen gas and aqueous Magnesium nitrate are formed. What volume of Hydrogen gas will be produced if 40.0 g of Magnesium is reacted with an excess of Nitric Acid?

4. Pentane (C5H12) burns according to the following unbalanced reaction: Assume STP

____C5H12 (g) + ____O2 (g) ____CO2 (g) + ____H2O(g)

a. What volume of O2 is required to produce 48.0 L of Carbon dioxide?

b. What volume of H2O(g) is produced when 106 L of CO2 is created?

c. What mass of Pentane would be required to produce 80.0 L of CO2?

5. Mercury (II) oxide decomposes when heated to produce liquid Mercury and Oxygen gas. What mass of Mercury (II) oxide would be required to produce 30.5 L of Oxygen gas? If the density of mercury liquid is 13.6 g/cm3, what volume is produced when 295 g of HgO2 is decomposed? Assume STP.

6. Magnesium metal reacts with hydrochloric acid to produce Magnesium chloride and hydrogen gas. If the density of Magnesium is 1.74 g/cm3, what volume of Mg is required to produce 84.0 L of hydrogen gas when it is reacted with an excess of HCl? Assume STP.

Name: __________________________

Limiting Reactant Worksheet

1) What mass of CS2 is produced when 17.5g of C are reacted with 39.5g of SO2 according to the equation 5C + 2SO2 CS2 + 4CO ? What mass of excess reactant will be left over?

2) What mass of NO is produced when 87.0g of Cu are reacted with 225g of HNO3 according to the equation 3Cu + 8HNO3 3Cu(NO3)2 + 2NO + 4H2O ? What mass of excess reactant will be left over?

3) What mass of Br2 is produced when 25.0g of K2Cr2O7, 55.0g of KBr and 60.0g of H2SO4 are reacted according to the equation

K2Cr2O7 + 6KBr + 7H2SO4 4K2SO4 + Cr2(SO4)3 + 3Br2 + 7H2O ?

How many grams of each excess reactant will remain unreacted?

4) What volume of CO2(g) at STP can be made when 0.0250L of C5H12(l) (density 626.0 g/L) is reacted with 40.0L of O2(g) at STP, according to the equation

C5H12(l) + 8O2(g) 5CO2(g) + 6H2O(l) ?

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