AP Chemistry Flashcards: Stoichiometry

Study Stoichiometry in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.

AP Chemistry

Stoichiometry

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QUESTION

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What is the first step in a stoichiometry problem?

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ANSWER

Write a balanced chemical equation. Ensures atom conservation for stoichiometric calculations.

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What this deck covers

This deck focuses on Stoichiometry, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

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Flashcard 1: What is the first step in a stoichiometry problem?

Answer: Write a balanced chemical equation. Ensures atom conservation for stoichiometric calculations.

Flashcard 2: What is the formula to calculate the number of particles from moles?

Answer: $\text{particles} = \text{moles} \times 6.022 \times 10^{23}$ . Multiplies moles by Avogadro's number for particle count.

Flashcard 3: How many moles of $H_2$ are needed to produce 2 moles of $NH_3$ in $N_2 + 3H_2 \rightarrow 2NH_3$ ?

Answer: 3 moles. 3:2 mole ratio from balanced equation coefficients.

Flashcard 4: Calculate the percent composition of oxygen in $H_2O$ .

Answer: 88.81%. Oxygen mass ( $16$ ) divided by $H_2O$ mass ( $18$ ) $\times 100\%$ .

Flashcard 5: Find the molar mass of $CO_2$ .

Answer: 44 g/mol. Carbon (12) + 2 oxygen atoms (16 each) = 44 g/mol.

Flashcard 6: Identify the unit for molar mass.

Answer: grams per mole (g/mol). Standard unit expressing mass per mole of substance.

Flashcard 7: Which unit is used to express concentration in stoichiometry?

Answer: Molarity (M). Standard concentration unit for solution calculations.

Flashcard 8: What is the formula for percent yield?

Answer: $\text{Percent yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100$ . Compares actual to theoretical yield as a percentage.

Flashcard 9: Calculate the percent composition of oxygen in $H_2O$ .

Answer: 88.81%. Oxygen mass (16) divided by $H_2O$ mass (18) × 100%.

Flashcard 10: Calculate the molarity of a solution with 10 moles in 5 L.

Answer: 2 M. $\frac{10 \text{ moles}}{5 \text{ L}} = 2$ M concentration.

Flashcard 11: Identify the limiting reactant in 4 moles $N_2$ and 10 moles $H_2$ for $N_2 + 3H_2 \rightarrow 2NH_3$ .

Answer: $H_2$ . Need 12 moles $H_2$ but only have 10; $H_2$ limits.

Flashcard 12: What is the stoichiometric coefficient for $H_2$ in $2H_2 + O_2 \rightarrow 2H_2O$ ?

Answer:

Coefficient shows 2 molecules react in balanced equation.

Flashcard 13: What is the molar mass of $H_2SO_4$ ?

Answer: 98.1 g/mol. 2H (2) + S (32) + 4O (64) = 98 g/mol total.

Flashcard 14: Which unit is used to express concentration in stoichiometry?

Answer: Molarity (M). Standard concentration unit for solution calculations.

Flashcard 15: What is the molecular formula for a compound with empirical formula $CH_2O$ and molar mass 180 g/mol?

Answer: $C_6H_{12}O_6$ . $180 \div 30 = 6$ , so multiply $CH_2O$ by 6.

Flashcard 16: What is the molecular formula for a compound with empirical formula $CH_2O$ and molar mass 180 g/mol?

Answer: $C_6H_{12}O_6$ . $180 \div 30 = 6$ , so multiply $CH_2O$ by 6.

Flashcard 17: What is the concentration of a solution with 5 moles of solute in 2 L of solution?

Answer: 2.5 M. $\frac{5 \text{ moles}}{2 \text{ L}} = 2.5$ M concentration.

Flashcard 18: What is the first step in a stoichiometry problem?

Answer: Write a balanced chemical equation. Ensures atom conservation for stoichiometric calculations.

Flashcard 19: Determine the empirical formula for a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen.

Answer: $CH_2O$ . Convert percentages to moles, then find simplest ratio.

Flashcard 20: What is the excess reactant in $2H_2 + O_2 \rightarrow 2H_2O$ with 5 moles $H_2$ and 2 moles $O_2$ ?

Answer: $O_2$ . Remains after limiting reactant is completely consumed.

Flashcard 21: Determine the limiting reactant in $2H_2 + O_2 \rightarrow 2H_2O$ given 5 moles $H_2$ and 2 moles $O_2$ .

Answer: $H_2$ . Needs 2.5 moles $O_2$ , but only 2 available, so $H_2$ limits.

Flashcard 22: How is actual yield different from theoretical yield?

Answer: Actual yield is the measured amount of product obtained. Theoretical assumes perfect conditions; actual is experimental.

Flashcard 23: How is theoretical yield calculated?

Answer: Use stoichiometry from the balanced equation. Assumes complete reaction with limiting reactant consumed.

Flashcard 24: What is the formula to calculate the number of particles from moles?

Answer: $\text{particles} = \text{moles} \times 6.022 \times 10^{23}$ . Multiplies moles by Avogadro's number for particle count.

Flashcard 25: Find the moles of $H_2O$ in 36 grams.

Answer: 2 moles. $36 \div 18 = 2$ using $H_2O$ molar mass of 18 g/mol.

Flashcard 26: What is the stoichiometric coefficient for $H_2$ in $2H_2 + O_2 \rightarrow 2H_2O$ ?

Answer:

Coefficient shows 2 molecules react in balanced equation.

Flashcard 27: Identify the limiting reactant in 4 moles $N_2$ and 10 moles $H_2$ for $N_2 + 3H_2 \rightarrow 2NH_3$ .

Answer: $H_2$ . Need 12 moles $H_2$ but only have 10; $H_2$ limits.

Flashcard 28: How do you calculate mass from moles?

Answer: $\text{mass (g)} = \text{moles} \times \text{molar mass (g/mol)}$ . Multiplies moles by molar mass to get mass in grams.

Flashcard 29: Find the volume of gas at STP for 1 mole.

Answer: 22.4 L. Standard molar volume at 0°C and 1 atm pressure.

Flashcard 30: What is the percent yield if the theoretical yield is 100g and actual yield is 80g?

Answer: 80%. $\frac{80}{100} \times 100\% = 80\%$ efficiency.

Flashcard 31: Calculate the number of molecules in 2 moles of $H_2$ .

Answer: $1.204 \times 10^{24}$ molecules. $2 \times 6.022 \times 10^{23}$ molecules per mole.

Flashcard 32: What is the molar mass of $H_2SO_4$ ?

Answer: 98.1 g/mol. 2H (2) + S (32) + 4O (64) = 98 g/mol total.

Flashcard 33: Convert 3 moles of $NaCl$ to grams.

Answer: 175.5 grams. $3 \times 58.5 = 175.5$ using $NaCl$ molar mass.

Flashcard 34: Calculate the percent composition of oxygen in $H_2O$ .

Answer: 88.81%. Oxygen mass (16) divided by $H_2O$ mass (18) × 100%.

Flashcard 35: How do you calculate mass from moles?

Answer: $\text{mass (g)} = \text{moles} \times \text{molar mass (g/mol)}$ . Multiplies moles by molar mass to get mass in grams.

Flashcard 36: What is the stoichiometric coefficient for $H_2$ in $2H_2 + O_2 \rightarrow 2H_2O$ ?

Answer:

Coefficient shows 2 molecules react in balanced equation.

Flashcard 37: Determine the empirical formula for a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen.

Answer: $CH_2O$ . Convert percentages to moles, then find simplest ratio.

Flashcard 38: Determine the moles of $NaOH$ needed to neutralize $1$ mole of $HCl$ .

Answer: $1$ mole. $1:1$ mole ratio from balanced acid-base equation.

Flashcard 39: Determine the limiting reactant in $2H_2 + O_2 \rightarrow 2H_2O$ given 5 moles $H_2$ and 2 moles $O_2$ .

Answer: $H_2$ . Needs 2.5 moles $O_2$ , but only 2 available, so $H_2$ limits.

Flashcard 40: Define molar mass.

Answer: The mass of one mole of a substance in grams. Equals the atomic/molecular weight expressed in g/mol.

Flashcard 41: State Avogadro's number.

Answer: $6.022 \times 10^{23}$ . The number of particles in one mole of any substance.

Flashcard 42: Find the volume of gas at STP for 1 mole.

Answer: 22.4 L. Standard molar volume at 0°C and 1 atm pressure.

Flashcard 43: What is the first step in a stoichiometry problem?

Answer: Write a balanced chemical equation. Ensures atom conservation for stoichiometric calculations.

Flashcard 44: What is the molecular formula for a compound with empirical formula $CH_2O$ and molar mass 180 g/mol?

Answer: $C_6H_{12}O_6$ . $180 \div 30 = 6$ , so multiply $CH_2O$ by 6.

Flashcard 45: Calculate the mass of 0.5 moles of $C_6H_{12}O_6$ .

Answer: 90 grams. $0.5 \times 180 = 90$ using glucose molar mass.

Flashcard 46: How is theoretical yield calculated?

Answer: Use stoichiometry from the balanced equation. Assumes complete reaction with limiting reactant consumed.

Flashcard 47: What is the concentration of a solution with 5 moles of solute in 2 L of solution?

Answer: 2.5 M. $\frac{5 \text{ moles}}{2 \text{ L}} = 2.5$ M concentration.

Flashcard 48: Identify the unit for molar mass.

Answer: grams per mole (g/mol). Standard unit expressing mass per mole of substance.

Flashcard 49: Find the moles of $H_2O$ in 36 grams.

Answer: 2 moles. $36 \div 18 = 2$ using $H_2O$ molar mass of 18 g/mol.

Flashcard 50: What is the excess reactant in $2H_2 + O_2 \rightarrow 2H_2O$ with 5 moles $H_2$ and 2 moles $O_2$ ?

Answer: $O_2$ . Remains after limiting reactant is completely consumed.

Flashcard 51: How do you calculate mass from moles?

Answer: $\text{mass (g)} = \text{moles} \times \text{molar mass (g/mol)}$ . Multiplies moles by molar mass to get mass in grams.

Flashcard 52: Determine the moles of $NaOH$ needed to neutralize 1 mole of $HCl$ .

Answer: 1 mole. 1:1 mole ratio from balanced acid-base equation.

Flashcard 53: Convert 0.25 moles of $Mg$ to atoms.

Answer: $1.505 \times 10^{23}$ atoms. $0.25 \times 6.022 \times 10^{23}$ atoms per mole.

Flashcard 54: Calculate the number of molecules in 2 moles of $H_2$ .

Answer: $1.204 \times 10^{24}$ molecules. $2 \times 6.022 \times 10^{23}$ molecules per mole.

Flashcard 55: What is empirical formula?

Answer: The simplest whole-number ratio of atoms. Shows simplest ratio without molecular complexity.

Flashcard 56: What is the percent yield if the theoretical yield is 100g and actual yield is 80g?

Answer: 80%. $\frac{80}{100} \times 100\% = 80\%$ efficiency.

Flashcard 57: Which unit is used to express concentration in stoichiometry?

Answer: Molarity (M). Standard concentration unit for solution calculations.

Flashcard 58: Find the moles of $H_2O$ in 36 grams.

Answer: 2 moles. $36 \div 18 = 2$ using $H_2O$ molar mass of 18 g/mol.

Flashcard 59: What is the formula for molarity?

Answer: $\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}$ . Relates amount of solute to solution volume.

Flashcard 60: Convert 3 moles of $NaCl$ to grams.

Answer: 175.5 grams. $3 \times 58.5 = 175.5$ using $NaCl$ molar mass.

Flashcard 61: Calculate the volume at STP for 0.5 moles of gas.

Answer: 11.2 L. $0.5 \times 22.4 = 11.2$ liters at STP.

Flashcard 62: Find the molar mass of $CO_2$ .

Answer: 44 g/mol. Carbon (12) + 2 oxygen atoms (16 each) = 44 g/mol.

Flashcard 63: Convert 3 moles of $NaCl$ to grams.

Answer: 175.5 grams. $3 \times 58.5 = 175.5$ using $NaCl$ molar mass.

Flashcard 64: Calculate the mass of 0.5 moles of $C_6H_{12}O_6$ .

Answer: 90 grams. $0.5 \times 180 = 90$ using glucose molar mass.

Flashcard 65: What is the formula to calculate the number of moles from mass?

Answer: $\text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}$ . Divides mass by molar mass to find amount in moles.

Flashcard 66: What is empirical formula?

Answer: The simplest whole-number ratio of atoms. Shows simplest ratio without molecular complexity.

Flashcard 67: Determine the limiting reactant in $2H_2 + O_2 \rightarrow 2H_2O$ given 5 moles $H_2$ and 2 moles $O_2$ .

Answer: $H_2$ . Needs 2.5 moles $O_2$ , but only 2 available, so $H_2$ limits.

Flashcard 68: What is the concentration of a solution with 5 moles of solute in 2 L of solution?

Answer: 2.5 M. $\frac{5 \text{ moles}}{2 \text{ L}} = 2.5$ M concentration.

Flashcard 69: Calculate the mass of 0.5 moles of $C_6H_{12}O_6$ .

Answer: 90 grams. $0.5 \times 180 = 90$ using glucose molar mass.

Flashcard 70: How is actual yield different from theoretical yield?

Answer: Actual yield is the measured amount of product obtained. Theoretical assumes perfect conditions; actual is experimental.

Flashcard 71: How many moles of $H_2$ are needed to produce 2 moles of $NH_3$ in $N_2 + 3H_2 \rightarrow 2NH_3$ ?

Answer: 3 moles. 3:2 mole ratio from balanced equation coefficients.

Flashcard 72: How is theoretical yield calculated?

Answer: Use stoichiometry from the balanced equation. Assumes complete reaction with limiting reactant consumed.

Flashcard 73: Identify the unit for molar mass.

Answer: grams per mole (g/mol). Standard unit expressing mass per mole of substance.

Flashcard 74: Find the volume of gas at STP for 1 mole.

Answer: 22.4 L. Standard molar volume at 0°C and 1 atm pressure.

Flashcard 75: Determine the empirical formula for a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen.

Answer: $CH_2O$ . Convert percentages to moles, then find simplest ratio.

Flashcard 76: Find the volume of 3 moles of gas at STP.

Answer: 67.2 L. $3 \times 22.4 = 67.2$ liters at standard conditions.

Flashcard 77: Identify the unit for molar mass.

Answer: grams per mole (g/mol). Standard unit expressing mass per mole of substance.

Flashcard 78: What is the formula for molarity?

Answer: $\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}$ . Relates amount of solute to solution volume.

Flashcard 79: How is theoretical yield calculated?

Answer: Use stoichiometry from the balanced equation. Assumes complete reaction with limiting reactant consumed.

Flashcard 80: What is the excess reactant in $2H_2 + O_2 \rightarrow 2H_2O$ with 5 moles $H_2$ and 2 moles $O_2$ ?

Answer: $O_2$ . Remains after limiting reactant is completely consumed.

Flashcard 81: What is the excess reactant in $2H_2 + O_2 \rightarrow 2H_2O$ with 5 moles $H_2$ and 2 moles $O_2$ ?

Answer: $O_2$ . Remains after limiting reactant is completely consumed.

Flashcard 82: How do you calculate mass from moles?

Answer: $\text{mass (g)} = \text{moles} \times \text{molar mass (g/mol)}$ . Multiplies moles by molar mass to get mass in grams.

Flashcard 83: What is the molecular formula for a compound with empirical formula $CH_2O$ and molar mass 180 g/mol?

Answer: $C_6H_{12}O_6$ . $180 \div 30 = 6$ , so multiply $CH_2O$ by 6.

Flashcard 84: Determine the moles of $NaOH$ needed to neutralize 1 mole of $HCl$ .

Answer: 1 mole. $1:1$ mole ratio from balanced acid-base equation.

Flashcard 85: Determine the empirical formula for a compound with 50% sulfur and 50% oxygen by mass.

Answer: $SO_2$ . Equal mass percentages give 1:2 atomic ratio S:O.

Flashcard 86: Identify the limiting reactant in 4 moles $N_2$ and 10 moles $H_2$ for $N_2 + 3H_2 \rightarrow 2NH_3$ .

Answer: $H_2$ . Need 12 moles $H_2$ but only have 10; $H_2$ limits.

Flashcard 87: What is the formula for percent yield?

Answer: $\text{Percent yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100$ . Compares actual to theoretical yield as a percentage.

Flashcard 88: Determine the limiting reactant in $2H_2 + O_2 \rightarrow 2H_2O$ given 5 moles $H_2$ and 2 moles $O_2$ .

Answer: $H_2$ . Needs 2.5 moles $O_2$ , but only 2 available, so $H_2$ limits.

Flashcard 89: What is the formula to calculate the number of moles from mass?

Answer: $\text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}$ . Divides mass by molar mass to find amount in moles.

Flashcard 90: What is the stoichiometric coefficient for $H_2$ in $2H_2 + O_2 \rightarrow 2H_2O$ ?

Answer:

Coefficient shows 2 molecules react in balanced equation.

Flashcard 91: What is the formula for molarity?

Answer: $\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}$ . Relates amount of solute to solution volume.

Flashcard 92: What is the formula to calculate the number of particles from moles?

Answer: $\text{particles} = \text{moles} \times 6.022 \times 10^{23}$ . Multiplies moles by Avogadro's number for particle count.

Flashcard 93: How many grams of $O_2$ are needed to react with 4 moles of $C$ in $C + O_2 \rightarrow CO_2$ ?

Answer: 128 grams. $4 \times 32 = 128$ grams using 1:1 mole ratio.

Flashcard 94: What is the formula to calculate the number of moles from mass?

Answer: $\text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}$ . Divides mass by molar mass to find amount in moles.

Flashcard 95: How many moles of $H_2$ are needed to produce 2 moles of $NH_3$ in $N_2 + 3H_2 \rightarrow 2NH_3$ ?

Answer: 3 moles. 3:2 mole ratio from balanced equation coefficients.

Flashcard 96: What is empirical formula?

Answer: The simplest whole-number ratio of atoms. Shows simplest ratio without molecular complexity.

Flashcard 97: What is the percent yield if the theoretical yield is 100g and actual yield is 80g?

Answer: 80%. $\frac{80}{100} \times 100\% = 80\%$ efficiency.

Flashcard 98: Calculate the mass of 0.5 moles of $C_6H_{12}O_6$ .

Answer: 90 grams. $0.5 \times 180 = 90$ using glucose molar mass.

Flashcard 99: State Avogadro's number.

Answer: $6.022 \times 10^{23}$ . The number of particles in one mole of any substance.

Flashcard 100: What is the formula for molarity?

Answer: $\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}$ . Relates amount of solute to solution volume.

AP Chemistry Flashcards: Stoichiometry

Stoichiometry

What this deck covers

How to use these flashcards

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Flashcard 1: What is the first step in a stoichiometry problem?

Flashcard 2: What is the formula to calculate the number of particles from moles?

Flashcard 3: How many moles of H2H_2H2​ are needed to produce 2 moles of NH3NH_3NH3​ in N2+3H2→2NH3N_2 + 3H_2 \rightarrow 2NH_3N2​+3H2​→2NH3​?

Flashcard 4: Calculate the percent composition of oxygen in H2OH_2OH2​O.

Flashcard 5: Find the molar mass of CO2CO_2CO2​.

Flashcard 6: Identify the unit for molar mass.

Flashcard 7: Which unit is used to express concentration in stoichiometry?

Flashcard 8: What is the formula for percent yield?

Flashcard 9: Calculate the percent composition of oxygen in H2OH_2OH2​O.

Flashcard 10: Calculate the molarity of a solution with 10 moles in 5 L.

Flashcard 11: Identify the limiting reactant in 4 moles N2N_2N2​ and 10 moles H2H_2H2​ for N2+3H2→2NH3N_2 + 3H_2 \rightarrow 2NH_3N2​+3H2​→2NH3​.

Flashcard 12: What is the stoichiometric coefficient for H2H_2H2​ in 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O2H2​+O2​→2H2​O?

Flashcard 13: What is the molar mass of H2SO4H_2SO_4H2​SO4​?

Flashcard 14: Which unit is used to express concentration in stoichiometry?

Flashcard 15: What is the molecular formula for a compound with empirical formula CH2OCH_2OCH2​O and molar mass 180 g/mol?

Flashcard 16: What is the molecular formula for a compound with empirical formula CH2OCH_2OCH2​O and molar mass 180 g/mol?

Flashcard 17: What is the concentration of a solution with 5 moles of solute in 2 L of solution?

Flashcard 18: What is the first step in a stoichiometry problem?

Flashcard 19: Determine the empirical formula for a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen.

Flashcard 20: What is the excess reactant in 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O2H2​+O2​→2H2​O with 5 moles H2H_2H2​ and 2 moles O2O_2O2​?

Flashcard 21: Determine the limiting reactant in 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O2H2​+O2​→2H2​O given 5 moles H2H_2H2​ and 2 moles O2O_2O2​.

Flashcard 22: How is actual yield different from theoretical yield?

Flashcard 23: How is theoretical yield calculated?

Flashcard 24: What is the formula to calculate the number of particles from moles?

Flashcard 25: Find the moles of H2OH_2OH2​O in 36 grams.

Flashcard 26: What is the stoichiometric coefficient for H2H_2H2​ in 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O2H2​+O2​→2H2​O?

Flashcard 27: Identify the limiting reactant in 4 moles N2N_2N2​ and 10 moles H2H_2H2​ for N2+3H2→2NH3N_2 + 3H_2 \rightarrow 2NH_3N2​+3H2​→2NH3​.

Flashcard 28: How do you calculate mass from moles?

Flashcard 29: Find the volume of gas at STP for 1 mole.

Flashcard 30: What is the percent yield if the theoretical yield is 100g and actual yield is 80g?

Flashcard 31: Calculate the number of molecules in 2 moles of H2H_2H2​.

Flashcard 32: What is the molar mass of H2SO4H_2SO_4H2​SO4​?

Flashcard 33: Convert 3 moles of NaClNaClNaCl to grams.

Flashcard 34: Calculate the percent composition of oxygen in H2OH_2OH2​O.

Flashcard 35: How do you calculate mass from moles?

Flashcard 36: What is the stoichiometric coefficient for H2H_2H2​ in 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O2H2​+O2​→2H2​O?

Flashcard 37: Determine the empirical formula for a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen.

Flashcard 38: Determine the moles of NaOHNaOHNaOH needed to neutralize 111 mole of HClHClHCl.

Flashcard 39: Determine the limiting reactant in 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O2H2​+O2​→2H2​O given 5 moles H2H_2H2​ and 2 moles O2O_2O2​.

Flashcard 40: Define molar mass.

Flashcard 41: State Avogadro's number.

Flashcard 42: Find the volume of gas at STP for 1 mole.

Flashcard 43: What is the first step in a stoichiometry problem?

Flashcard 44: What is the molecular formula for a compound with empirical formula CH2OCH_2OCH2​O and molar mass 180 g/mol?

Flashcard 45: Calculate the mass of 0.5 moles of C6H12O6C_6H_{12}O_6C6​H12​O6​.

Flashcard 46: How is theoretical yield calculated?

Flashcard 47: What is the concentration of a solution with 5 moles of solute in 2 L of solution?

Flashcard 48: Identify the unit for molar mass.

Flashcard 49: Find the moles of H2OH_2OH2​O in 36 grams.

Flashcard 50: What is the excess reactant in 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O2H2​+O2​→2H2​O with 5 moles H2H_2H2​ and 2 moles O2O_2O2​?

Flashcard 51: How do you calculate mass from moles?

Flashcard 52: Determine the moles of NaOHNaOHNaOH needed to neutralize 1 mole of HClHClHCl.

Flashcard 53: Convert 0.25 moles of MgMgMg to atoms.

Flashcard 54: Calculate the number of molecules in 2 moles of H2H_2H2​.

Flashcard 55: What is empirical formula?

Flashcard 56: What is the percent yield if the theoretical yield is 100g and actual yield is 80g?

Flashcard 57: Which unit is used to express concentration in stoichiometry?

Flashcard 58: Find the moles of H2OH_2OH2​O in 36 grams.

Flashcard 59: What is the formula for molarity?

Flashcard 60: Convert 3 moles of NaClNaClNaCl to grams.

Flashcard 61: Calculate the volume at STP for 0.5 moles of gas.

Flashcard 62: Find the molar mass of CO2CO_2CO2​.

Flashcard 63: Convert 3 moles of NaClNaClNaCl to grams.

Flashcard 64: Calculate the mass of 0.5 moles of C6H12O6C_6H_{12}O_6C6​H12​O6​.

Flashcard 65: What is the formula to calculate the number of moles from mass?

Flashcard 66: What is empirical formula?

Flashcard 67: Determine the limiting reactant in 2H2+O2→2H2O2H_2 + O_2 \rightarrow 2H_2O2H2​+O2​→2H2​O given 5 moles H2H_2H2​ and 2 moles O2O_2O2​.

Flashcard 68: What is the concentration of a solution with 5 moles of solute in 2 L of solution?

Flashcard 69: Calculate the mass of 0.5 moles of C6H12O6C_6H_{12}O_6C6​H12​O6​.

Flashcard 70: How is actual yield different from theoretical yield?

Flashcard 71: How many moles of H2H_2H2​ are needed to produce 2 moles of NH3NH_3NH3​ in N2+3H2→2NH3N_2 + 3H_2 \rightarrow 2NH_3N2​+3H2​→2NH3​?

Flashcard 72: How is theoretical yield calculated?

Flashcard 73: Identify the unit for molar mass.

Flashcard 74: Find the volume of gas at STP for 1 mole.

Flashcard 75: Determine the empirical formula for a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen.

Flashcard 3: How many moles of $H_2$ are needed to produce 2 moles of $NH_3$ in $N_2 + 3H_2 \rightarrow 2NH_3$ ?

Flashcard 4: Calculate the percent composition of oxygen in $H_2O$ .

Flashcard 5: Find the molar mass of $CO_2$ .

Flashcard 9: Calculate the percent composition of oxygen in $H_2O$ .

Flashcard 11: Identify the limiting reactant in 4 moles $N_2$ and 10 moles $H_2$ for $N_2 + 3H_2 \rightarrow 2NH_3$ .

Flashcard 12: What is the stoichiometric coefficient for $H_2$ in $2H_2 + O_2 \rightarrow 2H_2O$ ?

Flashcard 13: What is the molar mass of $H_2SO_4$ ?

Flashcard 15: What is the molecular formula for a compound with empirical formula $CH_2O$ and molar mass 180 g/mol?

Flashcard 16: What is the molecular formula for a compound with empirical formula $CH_2O$ and molar mass 180 g/mol?

Flashcard 20: What is the excess reactant in $2H_2 + O_2 \rightarrow 2H_2O$ with 5 moles $H_2$ and 2 moles $O_2$ ?

Flashcard 21: Determine the limiting reactant in $2H_2 + O_2 \rightarrow 2H_2O$ given 5 moles $H_2$ and 2 moles $O_2$ .

Flashcard 25: Find the moles of $H_2O$ in 36 grams.

Flashcard 26: What is the stoichiometric coefficient for $H_2$ in $2H_2 + O_2 \rightarrow 2H_2O$ ?

Flashcard 27: Identify the limiting reactant in 4 moles $N_2$ and 10 moles $H_2$ for $N_2 + 3H_2 \rightarrow 2NH_3$ .

Flashcard 31: Calculate the number of molecules in 2 moles of $H_2$ .

Flashcard 32: What is the molar mass of $H_2SO_4$ ?

Flashcard 33: Convert 3 moles of $NaCl$ to grams.

Flashcard 34: Calculate the percent composition of oxygen in $H_2O$ .

Flashcard 36: What is the stoichiometric coefficient for $H_2$ in $2H_2 + O_2 \rightarrow 2H_2O$ ?

Flashcard 38: Determine the moles of $NaOH$ needed to neutralize $1$ mole of $HCl$ .

Flashcard 39: Determine the limiting reactant in $2H_2 + O_2 \rightarrow 2H_2O$ given 5 moles $H_2$ and 2 moles $O_2$ .

Flashcard 44: What is the molecular formula for a compound with empirical formula $CH_2O$ and molar mass 180 g/mol?

Flashcard 45: Calculate the mass of 0.5 moles of $C_6H_{12}O_6$ .

Flashcard 49: Find the moles of $H_2O$ in 36 grams.

Flashcard 50: What is the excess reactant in $2H_2 + O_2 \rightarrow 2H_2O$ with 5 moles $H_2$ and 2 moles $O_2$ ?

Flashcard 52: Determine the moles of $NaOH$ needed to neutralize 1 mole of $HCl$ .

Flashcard 53: Convert 0.25 moles of $Mg$ to atoms.

Flashcard 54: Calculate the number of molecules in 2 moles of $H_2$ .

Flashcard 58: Find the moles of $H_2O$ in 36 grams.

Flashcard 60: Convert 3 moles of $NaCl$ to grams.

Flashcard 62: Find the molar mass of $CO_2$ .

Flashcard 63: Convert 3 moles of $NaCl$ to grams.

Flashcard 64: Calculate the mass of 0.5 moles of $C_6H_{12}O_6$ .

Flashcard 67: Determine the limiting reactant in $2H_2 + O_2 \rightarrow 2H_2O$ given 5 moles $H_2$ and 2 moles $O_2$ .

Flashcard 69: Calculate the mass of 0.5 moles of $C_6H_{12}O_6$ .

Flashcard 71: How many moles of $H_2$ are needed to produce 2 moles of $NH_3$ in $N_2 + 3H_2 \rightarrow 2NH_3$ ?

Flashcard 80: What is the excess reactant in $2H_2 + O_2 \rightarrow 2H_2O$ with 5 moles $H_2$ and 2 moles $O_2$ ?

Flashcard 81: What is the excess reactant in $2H_2 + O_2 \rightarrow 2H_2O$ with 5 moles $H_2$ and 2 moles $O_2$ ?

Flashcard 83: What is the molecular formula for a compound with empirical formula $CH_2O$ and molar mass 180 g/mol?

Flashcard 84: Determine the moles of $NaOH$ needed to neutralize 1 mole of $HCl$ .

Flashcard 86: Identify the limiting reactant in 4 moles $N_2$ and 10 moles $H_2$ for $N_2 + 3H_2 \rightarrow 2NH_3$ .

Flashcard 88: Determine the limiting reactant in $2H_2 + O_2 \rightarrow 2H_2O$ given 5 moles $H_2$ and 2 moles $O_2$ .

Flashcard 90: What is the stoichiometric coefficient for $H_2$ in $2H_2 + O_2 \rightarrow 2H_2O$ ?

Flashcard 93: How many grams of $O_2$ are needed to react with 4 moles of $C$ in $C + O_2 \rightarrow CO_2$ ?

Flashcard 95: How many moles of $H_2$ are needed to produce 2 moles of $NH_3$ in $N_2 + 3H_2 \rightarrow 2NH_3$ ?

Flashcard 98: Calculate the mass of 0.5 moles of $C_6H_{12}O_6$ .