quantities in chemical reactions review definitions $100 $200 $300 $400 $500 quantities balanced...

Quantities in Chemical Reactions

Review

Quantities in Chemical Reactions

Review

Definitions

$100 $100 $100 $100 $100 $100

$200 $200 $200 $200 $200

$300 $300 $300 $300 $300 $300

$400 $400 $400 $400 $400 $400

$500 $500 $500 $500 $500 $500

QuantitiesBalanced Chemical Equations

Additional Calculations

Team 1 Team 2 Team 3 Team 4

$200

Moles & Mass

Empirical Formulas

Definitions: $100Definitions: $100

Answer

A unit of measurement expressing amount of

a species

Definitions: $100Definitions: $100

MoleMole

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Definitions: $200Definitions: $200

Answer

The relationship between amounts of species in a reaction

Definitions: $200Definitions: $200

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StoichiometryStoichiometry

Definitions: $300Definitions: $300

Answer

The mass of one mole of a particular

chemical species

Definitions: $300Definitions: $300

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Atomic MassAtomic Mass

Definitions: $400Definitions: $400

Answer

1 mole of any gas occupies 22.4 L

Definitions: $400Definitions: $400

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STPSTP

Definitions: $500Definitions: $500

Answer

The number of particles in one mole

of a species

Definitions: $500Definitions: $500

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Avogadro’s NumberAvogadro’s Number

Moles & Mass: $100Moles & Mass: $100

Answer

Molar mass of (NH 4)2SO4

Moles & Mass: $100Moles & Mass: $100

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132.14 g/mol

Moles & Mass: $200Moles & Mass: $200

Answer

Number of atoms in 0.00511 mol of NaNO3

Moles & Mass: $200Moles & Mass: $200

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1.539 * 1023 atoms

Moles & Mass: $300Moles & Mass: $300

Answer

Number of grams in 2.3 x 10-4 moles of calcium

phosphate, Ca3(PO3)2?

Moles & Mass: $300Moles & Mass: $300

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0.116 grams

Scores

Proceed

Moles & Mass: $400Moles & Mass: $400

Answer

Using your knowledge of mole calculations and unit conversions,

determine how many atoms there are in 1 gallon of gasoline. Assume that the molecular formula for gasoline is

C6H14 and that the density of gasoline is approximately 0.85 grams/mL.

Note: there are 3785 mL per gallon.

Moles & Mass: $400Moles & Mass: $400

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5.29067 * 1023 atoms

Moles & Mass: $500Moles & Mass: $500

Answer

Number of molecules are there in 450 grams of

Na2SO4

Moles & Mass: $500Moles & Mass: $500

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1.91 * 1024 molecules

Quantities: $100Quantities: $100

Answer

CH4 + 3 O2 CO2 + 2 H2

Moles of CO2 produced if 26 g of CH4 is burned

Quantities: $100Quantities: $100

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16 moles16 moles

Quantities: $200Quantities: $200

Answer

CH4 + 3 O2 CO2 + 2 H2

Moles of CO2 produced if 67.2 L of CH4 is burned

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3 moles3 moles

Quantities: $300Quantities: $300

Answer

CaCO3(s) CO2(g) + CaO(s)

How many grams of calcium carbonate would you need to make 3.45 L of carbon dioxide

(assume STP)?

Quantities: $300Quantities: $300

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100/6 moles100/6 moles

Quantities: $400Quantities: $400

Answer

H2 gas can be produced by reacting CH4 with high

temperature steam. How many particles of H2 are produced when 158 g of CH4 reacts with steam?

CH4(g) + H2O(g) → CO(g) + 3 H2(g)

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180 * 1023 = 1.8 * 1025180 * 1023 = 1.8 * 1025

Quantities: $500Quantities: $500

Answer

The Haber process combines hydrogen (H2) with nitrogen (N2) to produce ammonia (NH3). At

STP, how many moles of ammonia can you produce, given

that you have 44.8 L of H2?

N2 (g) +3H2(g) → 2NH3(g)

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1.333 moles1.333 moles

Formulas: $100Formulas: $100

Answer

The empirical formulas, given the % composition for respective elements:

Fe = 63.53%, S = 36.47%

The empirical formulas, given the % composition for respective elements:

Fe = 63.53%, S = 36.47%

Formulas: $100Formulas: $100

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FeSFeS

Formulas: $200Formulas: $200

Answer

The empirical formulas, given the % composition for respective elements:

Na = 21.6%, Cl = 33.3%, O = 45.1%

The empirical formulas, given the % composition for respective elements:

Na = 21.6%, Cl = 33.3%, O = 45.1%

Formulas: $200Formulas: $200

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NaClO3NaClO3

Formulas: $300Formulas: $300

Answer

The empirical formulas, given the % composition for respective elements:

Cr = 26.52%, S = 24.52%, O = 48.96%

The empirical formulas, given the % composition for respective elements:

Cr = 26.52%, S = 24.52%, O = 48.96%

Formulas: $300Formulas: $300

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CrS3O6CrS3O6

Formulas: $400Formulas: $400

Answer

A compound of unknown identity is

made up of 40.1% sulfur and 59.9% oxygen (by

mass).

Formulas: $400Formulas: $400

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SO3SO3

Formulas : $500Formulas : $500

Answer

The empirical formulas, given the % composition for respective elements:

C = 63.1%, H = 11.92%, F = 24.97%

The empirical formulas, given the % composition for respective elements:

C = 63.1%, H = 11.92%, F = 24.97%

Formulas: $500Formulas: $500

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C5H12F

Balanced Chemical Equations: $100Balanced Chemical Equations: $100

Answer

__CHCl3  +  __Cl2 → __CCl4  +  __HCl __CHCl3  +  __Cl2 → __CCl4  +  __HCl 

Balanced Chemical Equations: $100Balanced Chemical Equations: $100

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Already balanced

CHCl3  +  Cl2 →  CCl4  +  HCl 

Already balanced

CHCl3  +  Cl2 →  CCl4  +  HCl 

Balanced Chemical Equations: $200Balanced Chemical Equations: $200

Answer

__SnO2 + __H2 → __Sn + __H2O__SnO2 + __H2 → __Sn + __H2O

Balanced Chemical Equations: $200Balanced Chemical Equations: $200

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SnO2 + 2H2 → Sn + 2H2OSnO2 + 2H2 → Sn + 2H2O

Balanced Chemical Equations: $300Balanced Chemical Equations: $300

Answer

__KOH + __H3PO4→__K3PO4 + __H2O__KOH + __H3PO4→__K3PO4 + __H2O

Balanced Chemical Equations: $300Balanced Chemical Equations: $300

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3 KOH + H3PO4→ K3PO4 + 3 H2O3 KOH + H3PO4→ K3PO4 + 3 H2O

Balanced Chemical Equations: $400Balanced Chemical Equations: $400

Answer

__KNO3 + __H2CO3→__K2CO3 + __HNO3__KNO3 + __H2CO3→__K2CO3 + __HNO3

Balanced Chemical Equations: $400Balanced Chemical Equations: $400

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2 KNO3 + H2CO3 → K2CO3 + 2 HNO32 KNO3 + H2CO3 → K2CO3 + 2 HNO3

Balanced Chemical Equations: $500Balanced Chemical Equations: $500

Answer

__ CaCl2 + __ Na3PO4 → __ Ca3(PO4)2 + __ NaCl

__ CaCl2 + __ Na3PO4 → __ Ca3(PO4)2 + __ NaCl

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3 CaCl2 + 2 Na3PO4 → Ca3(PO4)2 + 6 NaCl

3 CaCl2 + 2 Na3PO4 → Ca3(PO4)2 + 6 NaCl

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Answer

How many grams of H2 are produced if there are 18

grams of H2O?

CH4(g) + H2O(g) → CO(g) + 3 H2(g)

How many grams of H2 are produced if there are 18

grams of H2O?

CH4(g) + H2O(g) → CO(g) + 3 H2(g)

Additional Calculations: $100Additional Calculations: $100

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3 grams3 grams

Additional Calculations: $200Additional Calculations: $200

Answer

Na2S(aq) + AgNO3(aq) → Ag2S(s) + NaNO3(aq)

How many grams of Ag2S can be produced from 7.88 grams of AgNO3 and excess Na2S?

Na2S(aq) + AgNO3(aq) → Ag2S(s) + NaNO3(aq)

How many grams of Ag2S can be produced from 7.88 grams of AgNO3 and excess Na2S?

Additional Calculations: $200Additional Calculations: $200

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5.74 grams5.74 grams

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Answer

CuSO4 + Zn → ZnSO4 + Cu

How many grams of copper are produced from 2.9 grams

of zinc consumed with excess CuSO4 in this

reaction?

CuSO4 + Zn → ZnSO4 + Cu

How many grams of copper are produced from 2.9 grams

of zinc consumed with excess CuSO4 in this

reaction?

Additional Calculations: $300Additional Calculations: $300

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2.8 grams2.8 grams

Additional Calculations: $400Additional Calculations: $400

Answer

Limiting reagent when there is 8 grams of CH4

and 18 grams of H2O

CH4(g) + H2O(g) → CO(g) + 3 H2(g)

Limiting reagent when there is 8 grams of CH4

and 18 grams of H2O

CH4(g) + H2O(g) → CO(g) + 3 H2(g)

Additional Calculations: $400Additional Calculations: $400

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CH4(g)CH4(g)

Additional Calculations: $500Additional Calculations: $500

Answer

4.00 g of the gas was produced in a flask

containing 24.8 g of the reactant. Determine the

percent yield of the student's reaction.

4.00 g of the gas was produced in a flask

containing 24.8 g of the reactant. Determine the

percent yield of the student's reaction.

Additional Calculations: $500Additional Calculations: $500

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30.3%30.3%

Titration CalculationTitration Calculation

Proceed

Answer

3 NH4NO3 + Na3PO4 (NH4)3PO4 + 3 NaNO3

a) With 30 g of NH4NO3 and 50 g of Na3PO4, identify the limiting reagent.

b) What is the maximum amount of each product that can be formed?

3 NH4NO3 + Na3PO4 (NH4)3PO4 + 3 NaNO3

a) With 30 g of NH4NO3 and 50 g of Na3PO4, identify the limiting reagent.

b) What is the maximum amount of each product that can be formed?

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NH4NO3NH4NO3

a) Identify the limiting reagent

nNH4NO3

 nNa3PO4 =

0.375 mol NH4NO3 produces 0.125 mol of (NH4)3PO4

0.305 mol of Na3PO4 produces 0.305 mol of (NH4)3PO4

NH4NO3 is the limiting reagent b) What is the maximum amount of each product that can be formed?

Since NH4NO3 is the limiting reagent, only 0.125 mol of (NH4)3PO4 and 0.375 mol of NaNO3 can be produced.