1-Step
What is the mole ratio of water to oxygen in the following equation?
2 H2 + O2 --> 2 H2O
2:1
32 grams of oxygen are used in the following equation. How many moles of water are produced?
2 H2 + O2 --> 2 H2O
2 moles H2O
If the following reaction is run to completion with 100 grams of oxygen and an excess of hydrogen, how many grams of water will be produced?
2 H2 + O2 --> 2 H2O
112.63 grams H2O
What is an excess reactant?
Answers May Vary
- The reactant that there is plenty of or that you do not run out of
What is the equation for percent yield?
Percent Yield = Actual Yield / Theoretical Yield x100
If I have 10 moles of water, how many grams of water do I have?
2 H2 + O2 --> 2 H2O
180.2 grams H2O
30 moles of hydrogen are plugged into the following equation, how many liters of water are produced?
2 H2 + O2 --> 2 H2O
672 L H2O
Which of the following conversions would you need to complete the following problem?
Grams of compound A to Liters of Compound B.
I - Molar Mass of Compound A
II - Molar Mass of Compound B
III - Mole Ratio
IV - 1 Mole = 22.4 Liters
V - 1 Mole = 6.02 x 1024 atoms
I, III, IV
Grams A --> Moles A --> Moles B --> Liters B
What is a limiting reactant?
Answers May Vary.
- The reactant that STOPS the reaction from happening
- The reactant that produces the smaller theoretical yield
A recipe card reads that 35 cookies should be made from from the ingredients provided. After baking, you have 30 cookies. What is the percent yield of your baking?
85.71%
If the following reaction is run to completion with 100 moles of oxygen, how many moles of water will be produced?
2 H2 + O2 --> 2 H2O
200 mol H2O
How many atoms of oxygen are produced from 4 moles of H2?
2 H2 + O2 --> 2 H2O
1.20x1024 atoms H2
How many liters of oxygen are needed to fully react 40 grams of hydrogen?
2 H2 + O2 --> 2 H2O
221.78 Liters O2
25 grams of hydrogen and 50 grams of oxygen are used in the following reaction. What is the limiting reactant of this process?
2 H2 + O2 --> 2 H2O
Oxygen
The following reaction is run with 40 liters of oxygen and an excess of hydrogen. When run in the lab, 45 liters of H2O are collected. What is the percent yield of this reaction?
2 H2 + O2 --> 2 H2O
56.25% Yield
If 45 moles of water are produced, how many moles of hydrogen were initially used?
2 H2 + O2 --> 2 H2O
45 moles H2
250 liters of water are needed. How many moles of oxygen will be used to produce this?
2 H2 + O2 --> 2 H2O
5.58 moles O2
Which of the following conversions would you need to complete the following problem?
Atoms of compound A to Grams of Compound B.
I - Molar Mass of Compound A
II - Molar Mass of Compound B
III - Mole Ratio
IV - 1 Mole = 22.4 Liters
V - 1 Mole = 6.02 x 1023 atoms
V, III, II
Atoms A --> Moles A --> Moles B --> Grams B
What is the theoretical yield of liters of water when 50 liters of hydrogen and 50 liters of oxygen are allowed to fully react?
2 H2 + O2 --> 2 H2O
50 Liters of H2O
Limiting Reactant: Hydrogen
Excess Reactant: Oxygen
The following reaction is run to completion with 25 grams of hydrogen and 100 grams of oxygen. 100 liters of water are collected. What is the percent yield of this reaction?
2 H2 + O2 --> 2 H2O
71.43%
If I have 25 moles of hydrogen, how many grams of hydrogen do I have?
2 H2 + O2 --> 2 H2O
50.5 grams H2
If 50 grams of oxygen are used in the following equation, how many moles of hydrogen would be needed to fully react?
2 H2 + O2 --> 2 H2O
3.13 moles H2
An excess of oxygen is combined with 3.42x1023 atoms of hydrogen. How many liters of water is produced?
2 H2 + O2 --> 2 H2O
12.73 L H2O
**TRIPLE POINTS**
The following reaction is run to completion with 15 grams of hydrogen, and 15 grams of oxygen.
2 H2 + O2 --> 2 H2O
Determine the limiting reactant, excess reactant, theoretical yield, and amount of excess remaining.
Limiting Reactant: Oxygen
Excess Reactant: Hydrogen
Theoretical Yield: 16.89 g H2O
Excess Remaining: 13.11 g H2
**DOUBLE POINTS**
The following reaction is run to completion with 45 grams of sulfuric acid and 45 grams of sodium hydroxide. Once completed, 5.0 grams of water are collected. Determine the limiting reactant, excess reactant, and percent yield of this reaction.
H2SO4 + 2 NaOH --> Na2SO4 + H2O
Limiting Reactant: H2SO4
Excess Reactant: NaOH
Percent Yield: 60.46%