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Quantities in Chemical Reactions
Review
Quantities in Chemical Reactions
Review
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Definitions
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QuantitiesBalanced Chemical Equations
Additional Calculations
Team 1 Team 2 Team 3 Team 4
$200
Moles & Mass
Empirical Formulas
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Definitions: $100Definitions: $100
Answer
A unit of measurement expressing amount of
a species
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Definitions: $100Definitions: $100
MoleMole
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Definitions: $200Definitions: $200
Answer
The relationship between amounts of species in a reaction
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StoichiometryStoichiometry
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Answer
The mass of one mole of a particular
chemical species
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Atomic MassAtomic Mass
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Answer
1 mole of any gas occupies 22.4 L
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STPSTP
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Answer
The number of particles in one mole
of a species
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Avogadro’s NumberAvogadro’s Number
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Moles & Mass: $100Moles & Mass: $100
Answer
Molar mass of (NH 4)2SO4
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132.14 g/mol
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Moles & Mass: $200Moles & Mass: $200
Answer
Number of atoms in 0.00511 mol of NaNO3
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1.539 * 1023 atoms
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Moles & Mass: $300Moles & Mass: $300
Answer
Number of grams in 2.3 x 10-4 moles of calcium
phosphate, Ca3(PO3)2?
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0.116 grams
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Scores
Proceed
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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.
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5.29067 * 1023 atoms
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Moles & Mass: $500Moles & Mass: $500
Answer
Number of molecules are there in 450 grams of
Na2SO4
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1.91 * 1024 molecules
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Answer
CH4 + 3 O2 CO2 + 2 H2
Moles of CO2 produced if 26 g of CH4 is burned
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16 moles16 moles
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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
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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)?
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100/6 moles100/6 moles
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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
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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
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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%
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FeSFeS
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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%
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NaClO3NaClO3
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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%
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CrS3O6CrS3O6
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Answer
A compound of unknown identity is
made up of 40.1% sulfur and 59.9% oxygen (by
mass).
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SO3SO3
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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%
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C5H12F
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Answer
__CHCl3 + __Cl2 → __CCl4 + __HCl __CHCl3 + __Cl2 → __CCl4 + __HCl
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Already balanced
CHCl3 + Cl2 → CCl4 + HCl
Already balanced
CHCl3 + Cl2 → CCl4 + HCl
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Answer
__SnO2 + __H2 → __Sn + __H2O__SnO2 + __H2 → __Sn + __H2O
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SnO2 + 2H2 → Sn + 2H2OSnO2 + 2H2 → Sn + 2H2O
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Answer
__KOH + __H3PO4→__K3PO4 + __H2O__KOH + __H3PO4→__K3PO4 + __H2O
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3 KOH + H3PO4→ K3PO4 + 3 H2O3 KOH + H3PO4→ K3PO4 + 3 H2O
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Answer
__KNO3 + __H2CO3→__K2CO3 + __HNO3__KNO3 + __H2CO3→__K2CO3 + __HNO3
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2 KNO3 + H2CO3 → K2CO3 + 2 HNO32 KNO3 + H2CO3 → K2CO3 + 2 HNO3
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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)
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3 grams3 grams
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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?
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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?
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2.8 grams2.8 grams
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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)
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CH4(g)CH4(g)
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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.
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30.3%30.3%
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Titration CalculationTitration Calculation
Proceed
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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
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a) Identify the limiting reagent
nNH4NO3
nNa3PO4 =
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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.