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Questions and Answers
What is the mole ratio of Ca to P in the reaction Ca3(PO4)2 → CaO + P4O10?
What is the mole ratio of Ca to P in the reaction Ca3(PO4)2 → CaO + P4O10?
3:2
In the reaction 2A + 3B → 2C, if 10 moles of A reacts with 15 moles of B, which reactant is in excess and how many moles of it are left unreacted?
In the reaction 2A + 3B → 2C, if 10 moles of A reacts with 15 moles of B, which reactant is in excess and how many moles of it are left unreacted?
B; 3 moles
What is the percent yield of a reaction if the actual yield is 25 grams and the theoretical yield is 30 grams?
What is the percent yield of a reaction if the actual yield is 25 grams and the theoretical yield is 30 grams?
83.3%
What is the theoretical yield of NO2 in the reaction 2NO + O2 → 2NO2 if 10 moles of NO reacts with 5 moles of O2?
What is the theoretical yield of NO2 in the reaction 2NO + O2 → 2NO2 if 10 moles of NO reacts with 5 moles of O2?
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In the reaction 2H2 + O2 → 2H2O, if 10 moles of H2 reacts with 5 moles of O2, which reactant is limiting and how many moles of the other reactant are in excess?
In the reaction 2H2 + O2 → 2H2O, if 10 moles of H2 reacts with 5 moles of O2, which reactant is limiting and how many moles of the other reactant are in excess?
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What is the mole ratio of CO to CO2 in the reaction CO + O2 → CO2?
What is the mole ratio of CO to CO2 in the reaction CO + O2 → CO2?
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If the reaction 2A + B → 2C has a percent yield of 80%, what is the actual yield if the theoretical yield is 40 grams?
If the reaction 2A + B → 2C has a percent yield of 80%, what is the actual yield if the theoretical yield is 40 grams?
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What is the excess reactant in the reaction 3H2 + N2 → 2NH3 if 12 moles of H2 reacts with 4 moles of N2?
What is the excess reactant in the reaction 3H2 + N2 → 2NH3 if 12 moles of H2 reacts with 4 moles of N2?
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Study Notes
Mole Ratio
- The mole ratio is the ratio of moles of one reactant to moles of another reactant in a chemical reaction.
- It is used to determine the amount of each reactant required for a reaction to occur.
- Mole ratio is calculated by dividing the coefficient of the reactant in the balanced equation by the coefficient of the other reactant.
- Example: In the reaction 2H2 + O2 → 2H2O, the mole ratio of H2 to O2 is 2:1.
Excess Reactant
- An excess reactant is a reactant that is present in a greater amount than is required for the reaction to occur.
- The excess reactant is not completely consumed during the reaction, and some of it remains unreacted.
- The amount of excess reactant can be calculated by subtracting the amount of reactant required for the reaction from the initial amount of reactant.
Percent Yield
- Percent yield is a measure of the efficiency of a chemical reaction.
- It is calculated by dividing the actual yield of a reaction (the amount of product obtained) by the theoretical yield (the amount of product expected) and multiplying by 100.
- Percent yield = (actual yield / theoretical yield) x 100
- A percent yield of 100% indicates that the reaction is perfectly efficient, while a percent yield less than 100% indicates that the reaction is not perfectly efficient.
Theoretical Yield
- Theoretical yield is the maximum amount of product that can be obtained from a reaction, based on the amount of reactants present.
- It is calculated using the mole ratio of the reactants and the amount of limiting reactant.
- Theoretical yield is often used as a benchmark to compare the actual yield of a reaction.
Reaction Stoichiometry
- Reaction stoichiometry is the study of the quantitative relationships between reactants and products in a chemical reaction.
- It involves the use of mole ratios, limiting reactants, and excess reactants to predict the amount of product that can be obtained from a reaction.
- Reaction stoichiometry is important in chemical synthesis and engineering, as it allows chemists to predict the amount of reactants required and the amount of product that can be obtained from a reaction.
Mole Ratio
- The mole ratio is a ratio of moles of one reactant to moles of another reactant in a chemical reaction, used to determine the amount of each reactant required.
- Calculated by dividing the coefficient of the reactant in the balanced equation by the coefficient of the other reactant.
- Example: In the reaction 2H2 + O2 → 2H2O, the mole ratio of H2 to O2 is 2:1, meaning two moles of H2 react with one mole of O2.
Excess Reactant
- An excess reactant is a reactant present in a greater amount than required for the reaction to occur.
- Not completely consumed during the reaction, with some remaining unreacted.
- Amount of excess reactant can be calculated by subtracting the amount of reactant required from the initial amount.
Percent Yield
- Measures the efficiency of a chemical reaction, calculated by dividing the actual yield by the theoretical yield and multiplying by 100.
- Expressed as a percentage, with 100% indicating perfect efficiency and less than 100% indicating imperfect efficiency.
- Example: If the actual yield is 80g and the theoretical yield is 100g, the percent yield is 80%.
Theoretical Yield
- The maximum amount of product that can be obtained from a reaction, based on the amount of reactants present.
- Calculated using the mole ratio of reactants and the amount of limiting reactant.
- Used as a benchmark to compare the actual yield of a reaction.
Reaction Stoichiometry
- The study of quantitative relationships between reactants and products in a chemical reaction.
- Involves the use of mole ratios, limiting reactants, and excess reactants to predict the amount of product that can be obtained.
- Important in chemical synthesis and engineering, as it allows chemists to predict reactants required and product obtained.
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Description
Learn about the mole ratio, a critical concept in chemistry stoichiometry, and how it's used to determine the amount of each reactant required for a reaction. Also, understand what an excess reactant is and its role in chemical reactions.
