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Questions and Answers
In stoichiometry problems involving mass, what is the correct sequence of conversions?
In stoichiometry problems involving mass, what is the correct sequence of conversions?
- Mass to moles, then between moles of different chemicals, then moles to mass. (correct)
- Moles to mass, then between masses of different chemicals, then mass to moles.
- Moles to mass, then between moles of different chemicals, then mass to moles.
- Mass to moles, then between masses of different chemicals, then moles to mass.
If you have 22 pounds of hot dog meat, how many pounds of buns are needed, assuming each hot dog requires one bun and each bun weighs 0.1 pounds?
If you have 22 pounds of hot dog meat, how many pounds of buns are needed, assuming each hot dog requires one bun and each bun weighs 0.1 pounds?
- 2.2 pounds of buns.
- 22 pounds of buns.
- 17.6 pounds of buns. (correct)
- 8.8 pounds of buns.
In the electrolysis of water, what is the molar ratio between water ($H_2O$) and oxygen ($O_2$)?
In the electrolysis of water, what is the molar ratio between water ($H_2O$) and oxygen ($O_2$)?
- 2:1 (correct)
- 2:3
- 1:2
- 1:1
During the electrolysis of water, if you start with 50 grams of $H_2O$, approximately how many grams of $H_2$ will be produced?
During the electrolysis of water, if you start with 50 grams of $H_2O$, approximately how many grams of $H_2$ will be produced?
What mass of water ($H_2O$) in grams will be required to produce 16 grams of oxygen ($O_2$) during electrolysis?
What mass of water ($H_2O$) in grams will be required to produce 16 grams of oxygen ($O_2$) during electrolysis?
If the reaction 1 bun + 1 hot dog meat = 1 hot dog with bun, what is the limiting reactant if you have 50 buns and 40 pieces of hot dog meat?
If the reaction 1 bun + 1 hot dog meat = 1 hot dog with bun, what is the limiting reactant if you have 50 buns and 40 pieces of hot dog meat?
In the hot dog and bun example, assuming you have 10 pounds of buns, how many complete hot dogs with buns can you produce?
In the hot dog and bun example, assuming you have 10 pounds of buns, how many complete hot dogs with buns can you produce?
Why is it reasonable that the amount of oxygen produced during the electrolysis of 100 grams of water is less than 100 grams?
Why is it reasonable that the amount of oxygen produced during the electrolysis of 100 grams of water is less than 100 grams?
Flashcards
Stoichiometry
Stoichiometry
The calculation of reactants and products in chemical reactions.
Mass to Moles Conversion
Mass to Moles Conversion
Converting mass of a substance to moles using molar mass.
Balanced Reaction
Balanced Reaction
An equation representing a chemical reaction with equal number of atoms.
Electrolysis of Water
Electrolysis of Water
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Molar Mass of H2O
Molar Mass of H2O
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Mass of Oxygen from Water
Mass of Oxygen from Water
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Conversion Factors
Conversion Factors
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Final Mass Confirmation
Final Mass Confirmation
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Study Notes
Stoichiometry With Mass
- Stoichiometry problems involving mass require converting mass to moles, then converting between moles of different chemicals, and finally converting back to mass.
- The example problem involves a chef ordering buns for hot dogs, given 11 pounds of hot dog meat.
- The balanced reaction (recipe) is: 1 bun + 1 hot dog meat = 1 hot dog.
- The individual masses are:
- 1 bun = 0.1 pounds
- 1 hot dog = 0.125 pounds
- 1 hot dog with bun = 0.225 pounds
- To calculate the number of hot dogs, the conversion factor is the weight of one hot dog (0.125 pounds).
- The calculation is 11 pounds of hot dogs * (1 hot dog / 0.125 pounds) = 88 hot dogs.
- To calculate the number of buns needed, the conversion factor is the balanced reaction (1 hot dog : 1 bun).
- The calculation is 88 hot dogs * (1 bun / 1 hot dog) = 88 buns.
- To convert the number of buns to pounds, the conversion factor is the weight of one bun (0.1 pounds).
- The calculation is 88 buns * (0.1 pounds / 1 bun) = 8.8 pounds of buns.
Electrolysis of Water
- The electrolysis of water is a decomposition reaction where water breaks down into oxygen and hydrogen.
- The balanced equation is: 2H2O -> 2H2 + O2.
- To solve the problem of how many grams of oxygen are produced from 100 grams of water, you need to convert grams of water to moles of water, then moles of water to moles of oxygen, and finally moles of oxygen to grams of oxygen.
- The molar masses of the chemicals are:
- H2O = 18.02 g/mol
- H2 = 2.016 g/mol
- O2 = 32 g/mol
- The calculation for converting 100 grams of water to moles is: 100 grams of H2O * (1 mol H2O / 18.02 grams H2O) = 5.55 moles of H2O.
- The calculation for converting moles of water to moles of oxygen is: 5.55 moles of H2O * (1 mol O2 / 2 mol H2O) = 2.775 moles of O2.
- The calculation for converting moles of oxygen to grams is: 2.775 moles of O2 * (32 grams O2 / 1 mol O2) = 88.8 grams of O2.
- The final answer is 88.8 grams of oxygen.
- The answer is reasonable because it is less than 100 grams, which is expected as water decomposes into two products, and oxygen is heavier than hydrogen, so most of the mass should be in oxygen.
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