# Stoichiometry Jeopardy

## Presentation on theme: "Stoichiometry Jeopardy"— Presentation transcript:

Stoichiometry Jeopardy
Percent Yield Mass-Mass Mass-Volume Limiting Reactants “Stoiched” About Chemistry Q \$100 Q \$100 Q \$100 Q \$100 Q \$100 Q \$200 Q \$200 Q \$200 Q \$200 Q \$200 Q \$300 Q \$300 Q \$300 Q \$300 Q \$300 Q \$400 Q \$400 Q \$400 Q \$400 Q \$400 Q \$500 Q \$500 Q \$500 Q \$500 Q \$500 Final Jeopardy

Mg + HCl -------> MgCI2 + H2
\$100 Mass-Mass If 20.0 g of magnesium react with excess hydrochloric acid, how many grams of magnesium chloride will be produced? Mg + HCl > MgCI2 + H2

39.2g MgCl2

Al + Fe2O3 ------> Fe + Al2O3
\$200 Mass-Mass How many grams of aluminum would be required to produce 550 g of Fe using the following reaction? Al + Fe2O > Fe + Al2O3

265.1g Al

\$300 Mass-Mass What mass of oxygen is needed to completely react with 84.9 g of Fe according to the following reaction? Fe + O2 ----> Fe2O

12.2g O2

\$400 Mass-Mass Sodium oxide reacts with water to produce sodium hydroxide. What mass of sodium oxide must be used to produce 275 grams of sodium hydroxide?

\$400 Answer from Mass Mass 212.9g Na2O

\$500 Mass Mass When butane, C4H10 burns in oxygen, the products are carbon dioxide and water. What mass of carbon dioxide will be produced when 4.42 g of butane is burned in excess oxygen?

\$500 Answer from Mass Mass 13.35g CO2

\$100 Mass-Volume In the following equation, what volume of hydrogen gas is produced when 135 grams of aluminum are completely reacted with excess sulfuric acid?     2 Al    +  3  H2SO >    3 H2      +    Al2(SO4)3

168.6 L H2

\$200 Question from Mass-Volume
In the  reaction below, how many liters of   ammonia gas are produced when 35 grams of liquid nitrogen completely react with excess hydrogen?       N 2       +       3H2         >        2 NH3

56.0 L NH3

\$300 Question from Mass-Volume
What volume of oxygen is produced in the decomposition reaction of g sodium chlorate ? NaClO3  NaCl O2

15.3 L O2

\$400 Question from Mass-Volume
How many grams of Al2O3 will be formed from 17.4 liters of O2? Al + O2  Al2O3

58.2 g Al2O3

\$500 Question from Mass-Volume
How many liters of carbon dioxide will form from the combustion grams of C5H12 with excess oxygen?

497.8 L CO2

\$100 Question from % Yield Calculate the theoretical yield of Calcium Oxide if 24.8 grams of Calcium Carbonate decomposes. Calculate the percent yield if you got 13.1 grams in the laboratory. CaCO3 → CaO CO2

\$100 Answer from % Yield 94%

\$200 Question from % Yield What is the percent yield if you experimentally produce 3.65 grams of copper when 1.87 grams of Aluminum reacts with 9.65 grams of Copper (II) Sulfate? Al CuSO4 → Cu Al2(SO4)3

\$200 Answer from % Yield 95%

\$300 Question from % Yield There are grams of each reactant available. Determine the limiting reactant in this equation. SO NaOH → Na2SO H2O

\$300 Answer from % Yield LR=NaOH

\$400 Question from % Yield Find the theoretical yield of silicon carbide if 50.0 grams of silicon dioxide reacts with 79.1 grams of Carbon.  SiO C → SiC CO

\$400 Answer from % Yield 33.3g SiC

\$500 Question from % Yield What is the percent yield if 155 grams of calcium carbonate is treated with 250 grams of hydrochloric acid and 142 grams of calcium chloride is obtained? CaCO HCl → CaCl CO H2O

\$500 Answer from % Yield 56.6%

\$100 Question from Limiting Reactants
If 10.4 moles of hydrogen, H2, and 9.1 moles of oxygen, O2, are placed together in a container and allowed to react according to the equation. How many moles of water, H2O, would be produced by the reaction? 2 H2 + O2  2 H2O

10.4 mol H2O

\$200 Question from Limiting Reactants
If 83.7 grams of aluminum, Al, and grams of sulfur, S, are put into a container and allowed to react according to the above equation, which substance(s) and how many grams of each would be present in the container after the reaction is complete? 2 Al S  Al2S3

LR= Al

\$300 Question from Limiting reacatants
If grams of vanadium (II) oxide, VO, and 832 grams of iron (III) oxide, Fe2O3, are put into a container and allowed to react according to the equation above, which substance(s) and how many grams of FeO would be present in the container after the reaction is complete? 2 VO Fe2O3  6 FeO + V2O5

748.6g FeO

\$400 Question from Limiting Reactants
Methyl alcohol (wood alcohol), CH3OH, is produced via the reaction CO(g) + 2 H2(g)  CH3OH(l) A mixture of 1.20 g H2(g) and 7.45 g CO(g) are allowed to react. Which reagent is the limiting reagent?

8.5g CH3OH

\$500 Question from Limiting Reactants
A welder has 20.0 moles of acetylene gas (C2H2) and 10.0 moles of oxygen gas (O2). They combine to form water and carbon dioxide. Identify the limiting reactant. How many moles of carbon dioxide gas (CO2) will form?

O2 yields 8.0 mol CO2 C2H2 yields 40.0 mol CO2 O2 is the limiting reactant

\$100 Question from “Stoiched” About Chemistry
0.300 moles of bromine gas (Br2) and moles of chlorine gas (Cl2) react to form tribromochlorine (Br3Cl). How many moles of this product will form?

0.2 mol Br3Cl

\$200 Question from “Stoiched” About Chemistry
Determine the % yield when 7.80 grams of benzene (C6H6) burns in oxygen gas to form 3.00 grams of CO2 gas and water vapor.

11.5%

\$300 Question from “Stoiched” About Chemistry
25.3 g of magnesium reacts with 44.3 g of copper (II) nitrate to form copper and magnesium nitrate. What mass of copper will form? What mass of reactants will remain unreacted?

16.Og Cu will form 19.3 g un-reacted reactants

\$400 Question from “Stoiched” About Chemistry
2 NH O2  N2O H2O If 80.0 grams of O2 are reacted in the above reaction, how many grams of N2O will be produced?

55.2g N2O

\$500 Question from “Stoiched” About Chemistry
Methyl alcohol (wood alcohol), CH3OH, is produced via the reaction CO(g) + 2 H2(g)  CH3OH(l) A mixture of 1.20 g H2(g) and 7.45 g CO(g) are allowed to react. Which reagent is the limiting reagent? What is the yield of CH3OH? [Assume theoretical yield ing is what is wanted here.] How much of the reagent present in excess is left over? Suppose the actual yield is 7.52 g of CH3OH. What is the % yield?