Chemistry Stoichiometry Quiz

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Questions and Answers

How many moles of oxygen are required to produce 18 moles of water?

  • 12
  • 36
  • 9 (correct)
  • 18

How many moles of hydrogen gas are required to react with 5.5 moles of oxygen?

  • 3.5
  • 2.75
  • 5.5
  • 11 (correct)

What is the mole ratio of hydrogen gas to oxygen in the reaction?

  • 1:1
  • 2:1 (correct)
  • 3:1
  • 1:2

If 4 moles of water are produced, how many moles of hydrogen gas were consumed?

<p>2 (D)</p> Signup and view all the answers

If 10 grams of hydrogen gas are used in the reaction, how many grams of water will be produced?

<p>90 (A)</p> Signup and view all the answers

What is the molar mass of magnesium chloride (MgCl2)?

<p>95.21 g/mol (A)</p> Signup and view all the answers

How many grams are in 0.5 moles of sodium fluoride (NaF)?

<p>42 g (B)</p> Signup and view all the answers

How many moles are present in 150 grams of aluminum hydroxide (Al(OH)3)?

<p>1.9 moles (A)</p> Signup and view all the answers

What is the molar mass of copper(II) hydroxide, Cu(OH)2?

<p>97.55 g/mol (A)</p> Signup and view all the answers

If you have 2.0 moles of potassium sulfide (K2S), how many grams would you have?

<p>220 g (A)</p> Signup and view all the answers

What is the chemical formula of the reactant for the reaction shown in the question? (Select all that apply)

<p>Xe (B), F2 (D)</p> Signup and view all the answers

In calculation (b), what is the value "3.54 × 10−1 mol F2" representing?

<p>The number of moles of Fluorine used in the reaction (D)</p> Signup and view all the answers

What is the value 0.177 mol Xe(g) representing in the equation (b) for the reaction above?

<p>The number of moles of Xenon needed for the complete reaction (D)</p> Signup and view all the answers

In calculation (c), what is the mass of 4.35g F2 representing?

<p>The mass of Fluorine used in the reaction (A)</p> Signup and view all the answers

Based on the information in calculation (c), what is the mass of Xenon Tetrafluoride theoretically produced?

<p>11.9g (D)</p> Signup and view all the answers

What is the mass of Xenon theoretically produced in equation (d)?

<p>27.1g (D)</p> Signup and view all the answers

Which calculation represents the mass of the reactant (Xe) that would be needed to completely react with 15.7g of F2?

<p>calculation (d) (A)</p> Signup and view all the answers

Based on the information given, which of these components is the limiting reactant in the reaction between Xenon and Fluorine?

<p>It cannot be determined (C)</p> Signup and view all the answers

In the reaction between calcium fluoride and sulfuric acid, how many moles of calcium sulfate are produced when 10.0 g of calcium fluoride reacts with an excess of sulfuric acid?

<p>0.128 mol (C)</p> Signup and view all the answers

What is the limiting reactant in the reaction between 4.87 g of lithium nitride (Li3N) and 7.74 g of water (H2O)?

<p>Lithium Nitride (C)</p> Signup and view all the answers

In the reaction between aluminum and copper(II) chloride, how many moles of aluminum chloride (AlCl3) are produced when 0.25 g of aluminum reacts with an excess of copper(II) chloride?

<p>9.3 × 10−3 mol (D)</p> Signup and view all the answers

Which of the following reactants is in excess in the reaction between 33.76 g of zinc and 54.08 g of hydrochloric acid?

<p>Hydrochloric acid (C)</p> Signup and view all the answers

In the reaction between chlorine dioxide (ClO2) and water, what is the limiting reactant when 71.00 g of ClO2 reacts with 19.00 g of H2O?

<p>Chlorine Dioxide (B)</p> Signup and view all the answers

In the reaction between 10.0 g of calcium fluoride (CaF2) and 15.5 g of sulfuric acid (H2SO4), which reactant is in excess?

<p>Sulfuric Acid (C)</p> Signup and view all the answers

In the reaction CaCO3(s) + 2HCl(aq) → CaCl2(s) + CO2(g) + H2O(ℓ), what is the predicted yield of carbon dioxide if 15.7 g of CaCO3 reacts?

<p>6.90 g (B)</p> Signup and view all the answers

In the reaction between 4.87 g of lithium nitride (Li3N) and 7.74 g of water (H2O), how many moles of ammonia (NH3) are produced if the limiting reactant is completely consumed?

<p>0.140 mol (C)</p> Signup and view all the answers

What is the experimental yield of carbon dioxide if the predicted yield is 6.90 g and the percentage yield is 81.5%?

<p>5.62 g (B)</p> Signup and view all the answers

What does the percentage yield represent?

<p>The ratio of the actual amount of product obtained to the theoretical amount of product that can be formed, expressed as a percentage (D)</p> Signup and view all the answers

What is the theoretical yield of aluminum chloride (AlCl3) in moles, when 0.25 g of aluminum reacts with 0.51 g of copper(II) chloride (CuCl2)?

<p>0.0025 mol (D)</p> Signup and view all the answers

If the experimental yield of a reaction is less than the predicted yield, what are some possible reasons?

<p>All of the above (D)</p> Signup and view all the answers

What is the formula for calculating the percentage yield of a reaction?

<p>(Experimental yield / Predicted yield) x 100% (C)</p> Signup and view all the answers

What is the theoretical yield of iron(III) hydroxide in grams when 10.0 g of iron(III) sulfate reacts with excess sodium hydroxide?

<p>5.35 (C)</p> Signup and view all the answers

What is the limiting reagent in the reaction between iron(III) sulfate and sodium hydroxide as given in the content?

<p>Iron (III) sulfate (A)</p> Signup and view all the answers

What is the percentage yield of bromine if 20.0 g of bromic acid react with excess hydrobromic acid and produce 47.3 g of bromine?

<p>63.6% (A)</p> Signup and view all the answers

What is the predicted yield of lead(II) chromate in grams if 12.5 g of lead(II) chloride react with excess sodium chromate?

<p>14.5 g (A)</p> Signup and view all the answers

What is the correct balanced chemical equation for the reaction between bromic acid (HBrO3) and hydrobromic acid (HBr)?

<p>HBrO3(aq) + 5HBr(aq) → 3H2O(ℓ) + 3Br2(aq) (D)</p> Signup and view all the answers

What is the correct balanced chemical equation for the reaction between lead(II) chloride (PbCl2) and sodium chromate (Na2CrO4)?

<p>PbCl2(s) + Na2CrO4(aq) → PbCrO4(s) + 2NaCl(aq) (D)</p> Signup and view all the answers

Calculate the percentage yield of the bromine if the experimental yield of bromine is 47.3 g, and the theoretical yield is 74.4 g?

<p>63.6% (B)</p> Signup and view all the answers

Identify the product formed when lead(II) chloride reacts with sodium chromate.

<p>Lead(II) chromate (B)</p> Signup and view all the answers

Flashcards

Moles in 15 grams of lithium

There are 2.2 moles in 15 grams of lithium.

Grams in 2.4 moles of sulfur

2.4 moles of sulfur equals 77 grams for S(s) or 6.2 x 10^2 grams for S8(s).

Moles in 22 grams of argon

There are 0.55 moles in 22 grams of argon.

Grams in 88.1 moles of magnesium

88.1 moles of magnesium equals 2.14 x 10^3 grams.

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Molecular weight of H2O

The molecular weight of water (H2O) is 18.02 g/mol.

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Percentage Yield

The ratio of actual yield to predicted yield, multiplied by 100%.

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Experimental Yield

The actual amount of product obtained from a reaction.

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Predicted Yield

The calculated amount of product expected from a reaction based on stoichiometry.

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Calculating % Yield

To find % yield, divide experimental yield by predicted yield and multiply by 100.

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Expected Yield Example

If 15.7 g of CaCO3 yields 6.90 g of CO2, that's your expected yield.

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Iron(III) sulfate limiting reagent

Iron(III) sulfate is the limiting reagent in the reaction.

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Expected mass of Fe(OH)3

The predicted mass of iron(III) hydroxide produced is 5.35g.

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Experimental yield example

For 1.72g of product from a 9.10g predicted yield, % yield = 18.9%.

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Molar mass of HBrO3

The molar mass of HBrO3 is 128.91 g/mol.

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Predicted yield of Br2

The predicted yield of bromine (Br2) from 20g HBrO3 is 74.4g.

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Molar mass of PbCrO4

The molar mass of lead(II) chromate (PbCrO4) is 323.20 g/mol.

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Yield of PbCrO4

The predicted yield of lead(II) chromate is 14.5g from 12.5g PbCl2.

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CaF2 reaction with H2SO4

CaF2 reacts with H2SO4 to produce CaSO4 and HF.

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Limiting Reactant

A reactant that gets consumed first, limiting product formation.

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Moles of CaF2 from grams

Converting grams of CaF2 to moles involves dividing by molar mass (78.08 g/mol).

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Moles of H2SO4 from grams

Convert grams of H2SO4 to moles using its molar mass (98.09 g/mol).

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Li3N reaction with H2O

Li3N reacts with water to create LiOH and NH3.

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Moles of Li3N from grams

Convert grams of Li3N into moles using its molar mass (34.83 g/mol).

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Copper(II) chloride as limiting

In the reaction, copper(II) chloride is the reactant that limits the production of AlCl3.

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Excess reactants

Reactant that remains after the limiting reactant is fully consumed.

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Reaction of Xenon with Fluorine

Xe(g) + 2F2(g) → XeF4(g) shows a chemical reaction between xenon and fluorine to form xenon tetrafluoride.

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Mole Ratio in Reaction (XeF4)

For every 2 moles of F2, 1 mole of Xe is needed to produce XeF4.

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Calculation of Moles of Xe from F2

nXe = 3.54 × 10−1 mol F2 × (1 mol Xe / 2 mol F2) results in 0.177 mol Xe.

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Mass of XeF4 Formation

mXeF4 = 4.35 g F2 × (1 mol F2 / 38.00 g) × (1 mol XeF4 / 2 mol F2) × 207.29 g/mol = 11.9 g XeF4.

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Calculating Mass of Xe

mXe = 15.7 g F2 × (1 mol F2 / 38.00 g) × (1 mol Xe / 2 mol F2) × 131.29 g/mol = 27.1 g Xe.

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Identifying Limiting Reactant

In the reaction ZnO + C → Zn + CO, ZnO is the limiting reactant because it produces less product in comparison to C.

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Glucose and Oxygen Reaction

C6H12O6 + 6O2 → 6CO2 + 6H2O shows glucose as the limiting reactant due to lower available moles compared to O2.

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Limiting Reactant in C3H6 and NO Reaction

In the reaction 4C3H6 + 6NO → 4C3H3N + 6H2O + N2, C3H6 is the limiting reactant due to production constraints.

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Ammonia production ratio

In the reaction N2 + 3 H2 → 2 NH3, for every 1 mole of N2, 3 moles of H2 are required to produce 2 moles of NH3.

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SO2 to SO3 ratio

The reaction 2 SO2 + O2 → 2 SO3 shows a 1:2 ratio of O2 to SO3 production.

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PCl5 formation

In PCl3 + Cl2 → PCl5, the ratio of PCl3 to Cl2 is 1:1 for producing PCl5.

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NH3 to N2 ratio

In the equation 4 NH3 + 3 O2 → 2 N2 + 6 H2O, the ratio is 4 moles of NH3 to produce 2 moles of N2.

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Water from oxygen calculation

For the equation 2 H2 + O2 → 2 H2O, 5 moles of O2 yield 10 moles of H2O due to a 1:2 relationship.

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Study Notes

Naming Ions

  • Positive ions are named by the element name followed by "ion"
  • Negative ions are named by changing the element ending to "-ide" and followed by "ion"
  • Group 1 forms 1+ ions
  • Group 2 forms 2+ ions
  • Group 13 forms 3+ ions
  • Group 15 forms 3- ions
  • Group 16 forms 2- ions
  • Group 17 forms 1- ions

Naming Ions with Variable Charges

  • Iron(II) and Iron(III) are named using Roman numerals following "Iron" in parentheses
  • Stock system uses Roman numerals
  • Stock system names for Fe2+, Fe3+ and other ions with variable charges are Iron(II), Iron(III)

Polyatomic Ions

  • Sulfate ion: SO42-
  • Nitrate ion: NO3-
  • Hydrogen carbonate ion: HCO3-
  • Bisulfite ion: HSO3-
  • Carbonate ion: CO32-
  • Hydroxide ion: OH-

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