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What are the three main steps of stoichiometry?
What are the three main steps of stoichiometry?
Convert to moles, convert moles of known to moles of unknown, convert to the desired unit.
What does the ideal gas law allow you to convert to, that other methods do not?
What does the ideal gas law allow you to convert to, that other methods do not?
The ideal gas law allows you to convert to mole amounts under any condition, not just standard temperature and pressure (STP).
What is the conversion factor used to convert from particles to moles?
What is the conversion factor used to convert from particles to moles?
Avogadro's number, which is approximately $6.022 \times 10^{23}$ particles per mole.
What is used to convert between mass and moles for a pure substance?
What is used to convert between mass and moles for a pure substance?
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What quantity is used to convert between volume and moles for solutions?
What quantity is used to convert between volume and moles for solutions?
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What equation links volume, pressure, temperature, and moles for gases?
What equation links volume, pressure, temperature, and moles for gases?
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In the reaction $N_{2(g)} + 3H_{2(g)}
ightarrow 2NH_{3(g)}$, if 1.00 L of nitrogen reacts, what volume of ammonia is produced at SATP?
In the reaction $N_{2(g)} + 3H_{2(g)} ightarrow 2NH_{3(g)}$, if 1.00 L of nitrogen reacts, what volume of ammonia is produced at SATP?
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What three units can be used to convert 'to/from' moles based on the provided content?
What three units can be used to convert 'to/from' moles based on the provided content?
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In the reaction $N_2 + 3H_2 \rightarrow 2NH_3$, if you start with 0.0404 moles of $N_2$, how many moles of $NH_3$ will be produced?
In the reaction $N_2 + 3H_2 \rightarrow 2NH_3$, if you start with 0.0404 moles of $N_2$, how many moles of $NH_3$ will be produced?
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What does SATP stand for in the context of gas reactions?
What does SATP stand for in the context of gas reactions?
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According to Avogadro's law, what is the relationship between moles and volume for gases under the same conditions?
According to Avogadro's law, what is the relationship between moles and volume for gases under the same conditions?
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In the reaction of nitrogen and hydrogen to produce ammonia, if 1.00 L of nitrogen reacts, how many liters of ammonia will be produced, assuming the same conditions?
In the reaction of nitrogen and hydrogen to produce ammonia, if 1.00 L of nitrogen reacts, how many liters of ammonia will be produced, assuming the same conditions?
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What law should be applied if the conditions (temperature or pressure) change during a gas reaction?
What law should be applied if the conditions (temperature or pressure) change during a gas reaction?
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In the reaction $Fe + H_2SO_4 \rightarrow H_2 + FeSO_4$, what is the mole ratio between iron and hydrogen gas produced?
In the reaction $Fe + H_2SO_4 \rightarrow H_2 + FeSO_4$, what is the mole ratio between iron and hydrogen gas produced?
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If 40.0g of iron reacts with excess sulfuric acid, what is the first step to finding the volume of hydrogen produced at 18.0°C and 100.3kPa?
If 40.0g of iron reacts with excess sulfuric acid, what is the first step to finding the volume of hydrogen produced at 18.0°C and 100.3kPa?
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After calculating the moles of hydrogen gas produced from 40.0g of iron reacting with sulfuric acid, which equation would be used to calculate the volume if the temperature and pressure conditions are known?
After calculating the moles of hydrogen gas produced from 40.0g of iron reacting with sulfuric acid, which equation would be used to calculate the volume if the temperature and pressure conditions are known?
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Study Notes
Gas Law Stoichiometry
- Gas law stoichiometry is the same as other stoichiometry.
- It involves three steps:
- Convert to moles
- Convert moles of known to moles of unknown
- Convert to desired unit
- The ideal gas law provides a different way to convert to moles for any gas conditions, not just standard temperature and pressure (STP).
Summary of SCH3U0 Units (Converting to/from Moles)
- Using: Particles, Mass, Volume (Solutions), Volume, Pressure, Temperature (Gases)
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Unit-Conversion Factor/Method:
- Particles: Avogadro's number (6.022 x 1023 particles/mol)
- Mass: Molar mass (g/mol)
- Volume (Solutions): Concentration (mol/L)
- Volume, Pressure, Temperature (Gases): PV = nRT
Example 1: Nitrogen and Hydrogen Reaction
- Nitrogen (N2) gas reacts with hydrogen (H2) gas to form ammonia (NH3).
- If 1.00 L of N2 reacts with excess hydrogen under standard ambient temperature and pressure (SATP), the volume of ammonia produced is 2.00 L.
- The volume ratio follows the mole ratio for gases in a reaction.
Example 2: Iron and Sulfuric Acid Reaction
- What volume of hydrogen gas is produced when 40.0 g of iron reacts with excess sulfuric acid at 18.0 °C and 100.3 kPa?
- Given parameters are iron mass (40.0 g), temperature (18.0°C), and pressure (100.3 kPa).
- The required reaction is provided: Fe(s) + H2SO4(aq) → H2(g) + FeSO4(aq)
- The calculation steps (likely using the ideal gas law) and the final volume of hydrogen gas produced are needed to complete the answer.
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Description
Test your understanding of gas law stoichiometry with this quiz. It covers the three main steps of stoichiometry and the ideal gas law, along with unit conversions for moles related to gases. Dive into practical examples to solidify your grasp on the topic.
