WorksheetsUnit 8 Stoichiometry Review
Total questions: 17
Worksheet time: 50mins
According to the following balanced chemical equation, which molar ratio is consistent with the chemical equation based on the stoichiometric coefficients?
3 KOH + FeCl3 → Fe(OH)3 + 3 KCl
1 mol KOH : 1 mol Fe(OH)3
1 mol KOH : 1 mol KCl
3 mol FeCl3 : 1 mol KCl
1 mol FeCl3 : 3 mol Fe(OH)3
When silver nitrate (AgNO3) reacts with hydrochloric acid (HCl), silver chloride (AgCl) precipitates out of solution. What is the stoichiometric coefficient of HCl in the balanced chemical equation?
AgNO3 + HCl → AgCl + HNO3
1
2
3
4
A mixture of CO(g) and O2(g) is placed in a rigid, sealed container as shown in the particle diagram above. The CO(g) reacts with the O2(g) according to the following reaction. 2CO(g) + O2(g) → 2CO2(g). Which of the following diagrams correctly illustrates the reaction mixture after the reaction goes to completion?
Diagram A
Diagram B
Diagram C
Diagram D
Balance the chemical equation below using coefficients. The stoichiometric coefficient for oxygen gas is...
___ NH3(l) + ___ O2(g) → ___ NO2(g) + ___ H2O(l)
HINT: (Start by trying to balance hydrogen first. You may need to double some coefficients...)
1
4
6
7
What mass of dissolved HCl is needed to completely react with 1 mole of solid Mg?
Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
(Hint: Use the stoichiometry map. What units do they give us, what are they asking us for, and what path do we take?)
72.92 g
18.3 g
24.3 g
48.6 g
When 10.0 grams of magnesium react with excess hydrochloric acid, investigators expected to collect 39.2 g of magnesium chloride. Instead, the investigators only collected 30.0 grams of magnesium chloride. What is the percent yield of this experiment?
25.5%
33.0%
76.5%
131%
If the reaction produces 0.400 L of 1.5 M MgCl2, which setup shown will correctly calculate how many grams of HCl reacted with excess solid magnesium? (Type A, B, C, or D)
In the equation 2KClO3 → 2KCl + 3 O2, how many moles of KCl are produced when 5.0 moles of KClO3 decomposes completely?
1.5 mol KCl
2.0 mol KCl
3.0 mol KCl
5 mol KCl
When the limiting reactant in a chemical reaction is completely used up...
the reaction slows down.
the reaction stops.
the excess reactants begin combining.
the reaction speeds up.
For the reaction equation C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g), how many moles of H2O are produced from 2 moles of C3H8?
2 moles
3 moles
6 moles
8 moles
In the chemical reaction 4 A + 3 B → 5 C + 9 D, if 14 moles of A react with 15 moles of B, what is the limiting reactant?
Substance A
Substance B
Substance C
Substance D
Match the words with the correct definitions
A comparison between the amount of product that was able to be made and the amount of product that should have been able to be made in a specific chemical reaction scenario.
Percent Yield
The substance that is completely used up when known quantities of each reactant for a given
chemical reaction completely stop forming products.
Limiting Reactant
The amount of product that should be able to be made in a laboratory setting by a chemical
reaction that is determined mathematically using stoichiometry.
Theoretical Yield
A conversion factor that relates the amounts in moles of any two substances involved in a
chemical reaction.
Mole Ratio
The amount of product that was made by a chemical reaction that is determined experimentally in
a laboratory setting.
Actual Yield
Watney knows the Hab reclaims and fills the entire volume of a 5 L tank with carbon dioxide gas that is pressurized to 5 atm at a temperature of 300 K every 15 hours. Using the Ideal Gas Law and the Universal Gas Constant R from your Reference Packet, determine the number of moles of carbon dioxide in the tank when it is full. You must show ALL work to receive any credit, even if you put the correct answer in the box below. Round to the tenths place (0.1) and include all units. (HINT: Use the formula pV= nRT. R is a constant: R = 8.31446261815324)
Using 1 mole of carbon dioxide and the balanced oxygenator chemical reaction below, determine the liters of oxygen gas at STP that would be produced by the oxygenator if all moles of carbon dioxide in the tank fully reacted. You must show ALL work to receive any credit, even if your answer is correct. Round to the tenths place (0.1) and include all units.
Oxygenator Decomposing Carbon Dioxide: CO2(g) → C(s) + O2(g)
(Hint: use map. What do you start with, what do they want you to find and what path do we take? 1 mol = 22.4 L)
Draw a particulate diagram using the boxes provided below for a reaction between 5 moles of hydrogen gas and 2 moles of oxygen gas. Use the following reaction for this question:
Synthesis of Water 2 H2(g) + O2(g) → 2 H2O (l).
Consider that Mark Watney has confirmed that the hydrogen gas reactant is in excess, therefore mathematically all oxygen molecules should be reacting. In this scenario, the oxygen is not all reacting as predicted. The amount of water Mark is actually producing in his experiment is different than what he expected to produce before his experiment. In this scenario, would Mark Watney’s calculated percent yield be greater or lower than 100%? Explain your answer using evidence and reasoning.
What is the maximum number of moles of water that Mark Watney can produce with these volumes of hydrogen and oxygen gas? Justify your answer with stoichiometry for each reactant. (4 points)
