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Consider the following two step reaction: TeO2 + 2 OH- = TeO32- + H20 TeO32- + …
Related Topics
Wize University Chemistry Textbook > Stoichiometry
Stoichiometry
6 Activities
Consider the following two step reaction:
TeO
2
+ 2 OH- = TeO
3
2-
+ H
2
0
TeO
3
2-
+ 2H
+
= H
2
TeO
3
What mass of H
2
TeO
3
is obtained from 74.2 g of TeO
2
, assuming 100 % yield?
74.1 g
82.6 g
67.6 g
72.6 g
I don't know
Check Submission
More Stoichiometry Questions:
Consider the reaction between hydrogen gas (
H
2
\rm H_2
H
2
) and carbon monoxide (
C
O
\rm CO
CO
) which produces methanol gas (
C
H
3
O
H
\rm CH_3OH
C
H
3
OH
).
2
H
2
(
g
)
+
C
O
(
g
)
→
C
H
3
O
H
(
g
)
\rm 2H_2(g)+CO(g)\rightarrow CH_3OH(g)
2
H
2
(
g
)
+
CO
(
g
)
→
C
H
3
OH
(
g
)
The scheme above represents the initial content of a flask before any reaction took place. Which of the schemes below would correspond to the content of this flask once the reaction has reached completion?
Precipitation
A 4.23 g sample of a mixture of BaCl
2
and Ba(NO
3
)
2
is treated with excess AgNO
3
(aq). The precipitate is filtered off and then dried. If the dry precipitate weighs
5.27 g, what is the percentage by mass of BaCl
2
in the original mixture?
Molar masses:
A piece of zinc is allowed to react with an excess quantity of sulfuric acid, and the hydrogen gas produced is collected in a gas burette by displacement of water. Neglecting the effect of the vapor pressure of water on the system, calculate how many milligram (mg) of zinc would generate 92.0 mL of the gas at a temperature of 25.0 °C and a pressure of 1.00 atm.
Stoichiometry: Mole Ratios
How many moles of H
2
and N
2
can be formed by the decomposition of 12.7mol of ammonia, NH
3
? Do not include units in your answer.
2
N
H
3
→
N
2
+
3
H
2
2NH_3\rightarrow N_2+3H_2
2
N
H
3
→
N
2
+
3
H
2
Stoichiometry: Limiting Reagent
What is the maximum mass of Ca(CN)
2
that can be obtained from 1.56 g of HCN and 2.58 g of Ca(OH)
2
? The balanced chemical equation is shown below.
2
H
C
N
(
a
q
)
+
C
a
(
O
H
)
2
(
a
q
)
→
C
a
(
C
N
)
2
(
a
q
)
+
2
H
2
O
(
ℓ
)
27.03
g
/
m
o
l
74.10
g
/
m
o
l
92.12
g
/
m
o
l
18.02
g
/
m
o
l
\def\arraystretch{1.5}\begin{array}{ccccccc} 2 HCN(aq) &+ &Ca(OH)_2(aq)&→& Ca(CN)_2(aq) &+& 2 H_2O(\ell) \\ 27.03g/mol && 74.10g/mol && 92.12g/mol&& 18.02g/mol \end{array}
2
H
C
N
(
a
q
)
27.03
g
/
m
o
l
+
C
a
(
O
H
)
2
(
a
q
)
74.10
g
/
m
o
l
→
C
a
(
C
N
)
2
(
a
q
)
92.12
g
/
m
o
l
+
2
H
2
O
(
ℓ
)
18.02
g
/
m
o
l
Stoichiometry
The thermite reaction is used for welding railroad rails. The reaction is:
F
e
3
O
3
(
s
)
+
2
A
l
(
s
)
→
3
F
e
(
s
)
+
A
l
2
O
3
(s)
{Fe}_3{O}_3({s})+2{Al(s)}\rightarrow 3{Fe(s)}+{Al}_2{O}_3\text{(s)}
F
e
3
O
3
(
s
)
+
2
A
l
(
s
)
→
3
F
e
(
s
)
+
A
l
2
O
3
(s)
If 25g of iron, Fe(s), are produced from a reaction how many grams of aluminum oxide are generated?
Stoichiometry: Yield
What is the maximum amount of iodine gas (in moles) that can be formed if 1.00 mole of manganese (IV) oxide was allowed to react with 2.00 moles of hydroiodic acid to from manganese(II) iodide, iodine gas, and water?
Gases (Ideal) IIII
Today, most ammonia is produced by the Haber Process, which combines nitrogen from the air with hydrogen to produce ammonia gas. At 400
o
C and 2.00 atm, what volume of nitrogen gas is required to react completely with 50.0 L of hydrogen gas to produce ammonia gas?
Precipitation
Given the following reaction:
Na
2
SO
4
(s) + 2 C(s)
→
Na
2
S(s) + 2 CO
2
(g)
How many grams of carbon are required to produce 18.4 g Na
2
S(s)?
Limiting Reagent
What is the maximum mass of Ca(CN)
2
that can be obtained from 1.56 g of HCN and 2.58 g of Ca(OH)
2
? The balanced chemical equation is shown below. The molar masses are given in gmol
−1
. (Choose the closest answer.)
2 HCN(aq) + Ca(OH)
2
(aq)
→
Ca(CN)
2
(aq) + 2 H
2
O(l)
27.03 74.10 92.12 18.02
Precipitation
A 4.23 g sample of a mixture of BaCl
2
and Ba(NO
3
)
2
is treated with excess AgNO
3
(aq). The precipitate is filtered off and then dried. If the dry precipitate weighs
5.27 g, what is the percentage by mass of BaCl
2
in the original mixture?
Molar masses:
Stoichiometry
How many moles of H
2
and N
2
can be formed by the decomposition of 12.7 mol of ammonia, NH
3
?
When coal is burned, sulfur that is present within coal is converted to sulfur dioxide
(SO)
2
{\small \text{(SO)}_2}
(SO)
2
. This results in the acid ran phenomenon.
S(s)
+
O
2
(g)
→
SO
2
(g)
\text{S(s)}+\text{O}_2\text{(g)}\rightarrow\text{SO}_2\text{(g)}
S(s)
+
O
2
(g)
→
SO
2
(g)
If 3.75 kg of S are reacted with oxygen, calculate the volume of
SO
2
{\small \text{SO}_2}
SO
2
gas (in L) formed at 25.0
°
C
{\small \degree\text{C}}
°
C
and 1.10 atm.
The following gaseous reaction takes place at 473 K and 101.3 kPa:
N
2
(
g
)
+
O
2
(
g
)
→
N
O
2
(
g
)
N_{2(g)}+O_{2(g)}\to NO_{2(g)}
N
2
(
g
)
+
O
2
(
g
)
→
N
O
2
(
g
)
If 80.0 g of 0
2
are available to react, how many litres of N
2
will be required to completely consume the oxygen supply?
Br
2
and F
2
can react to form BrF
5
(g) according to the following unbalanced reaction: R=0.08206atmL/molK
B
r
2
(
g
)
+
F
2
(
g
)
→
B
r
F
5
(
g
)
Br_{2\left(g\right)}+\ F_{2\left(g\right)}\to BrF_{5\left(g\right)}
B
r
2
(
g
)
+
F
2
(
g
)
→
B
r
F
5
(
g
)
How many litres of BrF
5
can be produced at 43 °C and 1.0 atm if 18 mols of F
2
are reacted with an excess quantity of Br
2
?
Stoichiometry 3
What mass of C
5
H
12
produces 9.033
⋅
\cdot
⋅
10
22
CO
2
molecules upon complete combustion?
What volume of 3.16 M H
3
PO
4
solution is necessary to react with 27 mL of 0.18 M Mg(OH)
2
?
Consider the two following reactions:
CS
2
+ 3Cl
2
→ CCl
4
(l)+ S
2
Cl
2
(l) 60% yield
3 CCl
4
(l) + 2 SbF
3
(s) → 3 CCl
2
F
2
(g) + 2SbCl
3
(s) 80% yield
Redox Reactions and Calculation Using the Mole Method
Cu
2+
reacts with Na
2
S
2
O
3
by the following reaction:
Cu
2+
+ I
−
+ S
2
O
3
2−
→ CuI (s) + S
4
O
6
2−
A 4.115 g sample containing CuSO
4
and excess KI is treated with 32.55 mL of 0.2214 M Na
2
S
2
O
3
solution to titrate Cu
2+
. What is the % CuSO
4
in the sample?
Sulfur, S
8
, reacts with O
2
at high temperature to produce SO
2
. If 160 molecules of O
2
are used up:
a. How many molecules of sulfur react?
b. How many molecules of SO
2
form?
What mass of KClO
3
is required to produce proper amount of O
2
needed to achieve complete combustion of 78.88 g CH
4
?
2 KClO
3
→
2 KCl + 3 O
2
Gas Stoichiometry
The oxidation of phosphine is shown below:
2 PH
3
(g) + 3 O
2
(g) → P
2
O
3
(s) + 3 H
2
O(g)
What volume of O
2
(g), measured at 101 kPa and 50
o
C, is consumed in the formation of 20.0 g of P
2
O
3
by this reaction?
Mole method
What is the maximum number of moles of CCl
2
F
2
that can be obtained from 6.5 mol SbF
3
and 5.2 mol CCl
4
?
3 CCl
4
+ 2 SbF
3
→ 3 CCl
2
F
2
+ 2 SbCl
3
Gas Stoichiometry
A 1.8 g mixture of KClO
3
and KCl was heated until the complete decomposition of KClO
3
. The released O
2
has a volume of 405 mL at 25
⁰
C and 745 Torr. What was the percent of KClO
3
present in the mixture?
Calculating Molarity from Mass
In a reaction described by the equation below (unbalanced), excess calcium carbonate is added to 70.0 mL of hydrochloric acid. The theoretical yield of this reaction produces 20.0 g of carbon dioxide. Assuming the reaction proceeds with 100% yield and the volume of the solution does not change upon addition of solid, calculate the molairty, in mol/L, of the hydrochloric acid solution. The units for your answer should be in M or mol/L, but no units are required in your answer.
C
a
C
O
3
(
s
)
+
H
C
l
(
a
q
)
→
C
a
C
l
2
(
a
q
)
+
C
O
2
(
g
)
+
H
2
O
(
l
)
CaCO_3\ \left(s\right)\ \ \ \ +\ \ \ \ HCl\ \left(aq\right)\ \ \ \ \rightarrow\ \ \ \ CaCl_2\ \left(aq\right)\ \ \ \ +\ \ \ \ CO_2\ \left(g\right)\ \ \ \ +\ \ \ \ H_2O\ \left(l\right)
C
a
C
O
3
(
s
)
+
H
C
l
(
a
q
)
→
C
a
C
l
2
(
a
q
)
+
C
O
2
(
g
)
+
H
2
O
(
l
)
Chemical Reactions: Limiting Reagent
Based on the unbalanced chemical reaction below:
N
a
N
O
2
(
s
)
+
O
2
(
g
)
→
N
a
N
O
3
(
s
)
NaNO_2\ \left(s\right)\ \ \ \ +\ \ \ \ O_2\ \left(g\right)\ \ \ \ \rightarrow\ \ \ \ NaNO_3\ \left(s\right)
N
a
N
O
2
(
s
)
+
O
2
(
g
)
→
N
a
N
O
3
(
s
)
a)
Calculate the mass of sodium nitrate if 10.25 g of sodium nitrite is reacted with 7.55 g of oxygen gas.
Chemical Reactions: Limiting Reagent & Percent Yield Practice
Iron oxidizes when exposed to oxygen to form iron oxide according to the following equation:
Fe + O2 →Fe2O3
352g of pure iron is exposed to 12.0 mols of O2, and after a period of time 46.7 g of iron oxide (rust) is collected.
What volume of hydrogen (STP) is produced by dissolving one-half mole of aluminum in sulfuric acid?
2
A
l
(
s
)
+
3
H
2
S
O
4
(
a
q
)
→
A
l
2
(
S
O
4
)
3
(
a
q
)
+
3
H
2
(
g
)
2Al_{(s)}+3H_2SO_{4(aq)} \to Al_2(SO_4)_{3(aq)}+3H_{2(g)}
2
A
l
(
s
)
+
3
H
2
S
O
4
(
a
q
)
→
A
l
2
(
S
O
4
)
3
(
a
q
)
+
3
H
2
(
g
)
Br
2
and F
2
can react to form BrF
5
(g) according to the following unbalanced reaction:
B
r
2
(
g
)
+
F
2
(
g
)
→
B
r
F
5
(
g
)
Br_{2\left(g\right)}+\ F_{2\left(g\right)}\to BrF_{5\left(g\right)}
B
r
2
(
g
)
+
F
2
(
g
)
→
B
r
F
5
(
g
)
How many litres of BrF
5
can be produced at 43 °C and 1.0 atm if 18 mols of F
2
are reacted with an excess quantity of Br
2
?
Stoichiometry: Limiting reagents
Ammonia, NH
3
, and borane, BH
3
, react to form a Lewis adduct, ammonia borane as shown below.
N
H
3
(
s
o
l
)
+
B
H
3
(
s
o
l
)
→
N
H
3
B
H
3
(
s
)
NH_{3(sol)} + BH_{3(sol)} \rightarrow NH_3BH_{3(s)}
N
H
3
(
so
l
)
+
B
H
3
(
so
l
)
→
N
H
3
B
H
3
(
s
)
If 24 mL of a 0.74 M solution of ammonia is mixed with 12 mL of a 1.8 M solution of borane what is the maximum mass of ammonia borane that can be produced?
Stoichiometry: Mass Percentage
How many grams of PCl
3
are needed to produce 10g of POCl
3
using an excess of hydrogen peroxide assuming a typical reaction yield of 78%?
P
C
l
3
+
H
2
O
2
→
P
O
C
l
3
+
H
2
O
PCl_3+H_2O_2\rightarrow POCl_3+H_2O
P
C
l
3
+
H
2
O
2
→
P
O
C
l
3
+
H
2
O
Stoichiometry: Percent yield
Consider the following unbalanced reaction:
C
4
H
8
O
2
+
O
2
→
C
O
2
+
H
2
O
\rm C_4H_8O_2 +O_2 \to CO_2 + H_2O
C
4
H
8
O
2
+
O
2
→
C
O
2
+
H
2
O
If 36.00 g of
C
4
H
8
O
2
\rm C_4H_8O_2
C
4
H
8
O
2
is burned, what mass of water would be collected if the reaction yield was 76%?
Chemical Reactions: Limiting Reagent
15mL of a 1.2M solution of HCl reacts with 22mL of a 1.4M solution of NaOH. How many moles of NaOH are left after the reaction is complete?
H
C
l
(
a
q
)
+
N
a
O
H
(
a
q
)
→
H
2
O
(
l
)
+
N
a
C
l
(
a
q
)
HCl_{(aq)}+NaOH_{(aq)}\rightarrow H_2O_{(l)}+ NaCl_{(aq)}
H
C
l
(
a
q
)
+
N
a
O
H
(
a
q
)
→
H
2
O
(
l
)
+
N
a
C
l
(
a
q
)
Stoichiometry: Mass of product calculation
16.0 mL of Hg (mp = -38.8
o
C, density = 13.56 g/mL) reacts with Fluorine gas and the reaction goes to completion as shown below in the unbalanced chemical reaction.
H
g
(
l
)
+
F
2
(
g
)
→
H
g
F
2
(
s
)
Hg_{(l)}+F_{2(g)}\rightarrow HgF_{2(s)}
H
g
(
l
)
+
F
2
(
g
)
→
H
g
F
2
(
s
)
Once the reaction has gone to completion, what mass of Mercury Fluoride, HgF
2
, is produced?
Chemical Reactions: Hydrate Question
A 15.67 g sample of a hydrate of magnesium carbonate (MgCO
3
) was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?
Practice: Mass Percentage
A compound containing sodium, chlorine, and oxygen is 25.42% sodium by mass. A 3.25 g sample gives 4.33 x 10
22
atoms of oxygen. What is the empirical formula?
Hint: This is a tricky problem but start by writing the variables that you know.....what can you solve for?
If you're still not sure, my hint is to start with O! We can calculate moles of O, then mass of O, then % mass of O! What should we do next??
Stoichiometry: Percent Yield
A compound with the formula
C
7
H
8
O
3
\text{C}_7\text{H}_8\text{O}_3
C
7
H
8
O
3
is burned to completion in excess
O
2
\text{O}_2
O
2
. If 18.0g of the organic compound was consumed in the reaction, how many grams of
H
2
O
\text{H}_2\text{O}
H
2
O
will be collected if the yield was 85%?
In dilute nitric acid, HNO
3
, copper metal dissolves according to the following equation. How many grams of HNO
3
are needed to dissolve 11.45 g of Cu according to this equation?
3
C
u
+
8
H
N
O
3
→
3
C
u
(
N
O
3
)
2
+
2
N
O
+
4
H
2
O
3Cu+8HNO_3→3Cu(NO_3)_2+2NO+4H_2O
3
C
u
+
8
H
N
O
3
→
3
C
u
(
N
O
3
)
2
+
2
N
O
+
4
H
2
O
When coal is burned, sulfur that is present within coal is converted to sulfur dioxide (SO
2
). This results in the acid rain phenomenon. If 3.75 kg of S are reacted with oxygen, calculate the volume of SO
2
gas (in L) formed at 25.0 °C and 1.10 atm.
The potassium salt of benzoic acid, potassium benzoate (KC
7
H
5
O
2
, MM=160 g/mol) can be made by the action of potassium permanganate on toluene (C
7
H
8
, MM=92 g/mol). If the yield of potassium benzoate cannot realistically be expected to be more than 71%, what is the minimum number of grams of toluene needed to produce 11.5 g of potassium benzoate?
C
7
H
8
+
2
K
M
n
O
4
→
K
C
7
H
5
O
2
+
2
M
n
O
2
+
K
O
H
+
H
2
O
C_7 H_8+2KMnO_4→KC_7 H_5 O_2+2MnO_2+KOH+H_2 O
C
7
H
8
+
2
K
M
n
O
4
→
K
C
7
H
5
O
2
+
2
M
n
O
2
+
K
O
H
+
H
2
O
Stoichiometry: Percent Yield
How many grams of PCl
3
are needed to produce 10g of OPCl
3
using an excess of hydrogen peroxide assuming a typical reaction yield of 78%?
PCl
3
+
H
2
O
2
→
OPCl
3
+
H
2
O
Stoichiometry
The thermite reaction is used for welding railroad rails. The reaction is:
Fe
3
O
3
(
s
)
+
2
Al(s)
→
3
Fe(s)
+
Al
2
O
3
(s)
\text{Fe}_3\text{O}_3\text({s})+2\text{Al(s)}\rightarrow 3\text{Fe(s)}+\text{Al}_2\text{O}_3\text{(s)}
Fe
3
O
3
(
s
)
+
2
Al(s)
→
3
Fe(s)
+
Al
2
O
3
(s)
If 25. grams of iron, Fe(s), are produced from a reaction how many grams of aluminum oxide are generated?
Chemical Reactions: Limiting Reagent & Percent Yield Practice
Iron oxidizes when exposed to oxygen to form iron oxide according to the following equation:
Fe + O
2
→Fe
2
O
3
352g of pure iron is exposed to 12.0 mols of O
2
, and after a period of time 46.7 g of iron oxide (rust) is collected.
Stoichiometry and Ideal Gas Law Practice
The combustion of methanol (CH
3
OH) is shown below. If 16g of methanol is burned in oxygen, what volume of CO
2
is produced if the pressure is 101.3kPa, T=25C, and R=8.314kPaL/molK? Round to the nearest whole number.
CH
3
OH + O
2
--> CO
2
+ H
2
O
Is the equation balanced?
No
A piece of zinc is allowed to react with an excess quantity of sulfuric acid, and the hydrogen gas produced is collected in a gas burette by displacement of water. Neglecting the effect of the vapor pressure of water on the system, calculate how many milligram (mg) of zinc would generate 92.0 mL of the gas at a temperature of 25.0 °C and a pressure of 1.00 atm.
Consider the reaction between hydrogen gas (
H
2
\rm H_2
H
2
) and carbon monoxide (
C
O
\rm CO
CO
) which produces methanol gas (
C
H
3
O
H
\rm CH_3OH
C
H
3
OH
).
2
H
2
(
g
)
+
C
O
(
g
)
→
C
H
3
O
H
(
g
)
\rm 2H_2(g)+CO(g)\rightarrow CH_3OH(g)
2
H
2
(
g
)
+
CO
(
g
)
→
C
H
3
OH
(
g
)
The scheme above represents the initial content of a flask before any reaction took place. Which of the schemes below would correspond to the content of this flask once the reaction has reached completion?
A 2.56 g sample of ZnSO4
⋅
7H2O is heated to dryness. Determine the anhydrous mass remaining after all the water has been driven off. (provide an answer with 2 decimal places and correct unit)
Stoichiometry: Molar mass and Avogadro's Number
How many hydrogen atoms are in exactly 2 g of hydrazinium sulfate, N
2
H
6
SO
4
?
Ideal Gas Law: Stoichiometry
What volume of hydrogen (STP) is produced by dissolving one-half mole of aluminum in sulfuric acid?
2
A
l
(
s
)
+
3
H
2
S
O
4
(
a
q
)
→
A
l
2
(
S
O
4
)
3
(
a
q
)
+
3
H
2
(
g
)
2Al(s)+3H_2SO_4(aq)→Al_2(SO_4)_3(aq)+3H_2(g)
2
A
l
(
s
)
+
3
H
2
S
O
4
(
a
q
)
→
A
l
2
(
S
O
4
)
3
(
a
q
)
+
3
H
2
(
g
)
A piece of zinc is allowed to react with an excess quantity of sulfuric acid, and the hydrogen gas produced is collected in a gas burette by displacement of water. Neglecting the effect of the vapor pressure of water on the system, calculate how many milligram (mg) of zinc would generate 92.0 mL of the gas at a temperature of 25.0 °C and a pressure of 1.00 atm.
Gas Laws: Practice
A student decides to do a more controlled version of the hydrogen balloon explosion. The
unbalanced
chemical equation for this reaction is shown below:
H
2
(
g
)
+
O
2
(
g
)
→
H
2
O
(
g
)
H_2(g)+O_2(g)→H_2O(g)
H
2
(
g
)
+
O
2
(
g
)
→
H
2
O
(
g
)
(a)
Write the
balanced
chemical equation for this reaction.
Chemical Reactions: Limiting Reagent
Potassium carbonate, K
2
CO
3
, will react with acetic acid, CH
3
CO
2
H, to produce carbon dioxide gas, as per the following unbalanced reaction:
K
2
C
O
3
(
s
)
+
C
H
3
C
O
2
H
(
a
q
)
→
K
C
H
3
C
O
2
(
a
q
)
+
C
O
2
(
g
)
+
H
2
O
(
l
)
K_2CO_3(s)+CH_3CO_2H(aq)\rightarrow KCH_3CO_2(aq)+CO_2(g)+H_2O(l)
K
2
C
O
3
(
s
)
+
C
H
3
C
O
2
H
(
a
q
)
→
K
C
H
3
C
O
2
(
a
q
)
+
C
O
2
(
g
)
+
H
2
O
(
l
)
If 4 moles of K
2
CO
3
reacted with an excess of CH
3
CO
2
H, how many moles of CH
3
CO
2
H reacted?
Stoichiometry
Br
2
and F
2
can react to form BrF
5
(g) according to the following unbalanced reaction: R=0.08206atmL/molK
B
r
2
(
g
)
+
F
2
(
g
)
→
B
r
F
5
(
g
)
Br_{2\left(g\right)}+\ F_{2\left(g\right)}\to BrF_{5\left(g\right)}
B
r
2
(
g
)
+
F
2
(
g
)
→
B
r
F
5
(
g
)
How many litres of BrF
5
can be produced at 43 °C and 1.0 atm if 18 mols of F
2
are reacted with an excess quantity of Br
2
?
Stoichiometry
The following gaseous reaction takes place at 473 K and 101.3 kPa:
N
2
(
g
)
+
O
2
(
g
)
→
N
O
2
(
g
)
N_{2(g)}+O_{2(g)}\to NO_{2(g)}
N
2
(
g
)
+
O
2
(
g
)
→
N
O
2
(
g
)
If 80.0 g of 0
2
are available to react, how many litres of N
2
will be required to completely consume the oxygen supply?
Like Spring 2019 Exam 2
At 100
o
C and 1.00 atm, what volume of nitrogen gas is required to react completely with 10.0 L of hydrogen gas to produce ammonia gas?