Chemistry Reference
In-Depth Information
(c) How many moles of NaOH will be present after the
reaction?
(d) How many moles of
10.111
Calculate the number of moles of
SO
2
that will be
2
produced by the reaction of 1.00 mol of
SO
with
3
H
.
2.76 mol of
10.112
Calculate the number of moles of
Na
will be present in the fi-
nal solution?
(e) Does your answer to part (d) confirm that
CO
2
that will be
HCO
3
produced by the reaction of 2.20 mol of
with
Na
is a
H
.
1.80 mol of
10.113 Calculate the mass of that will be produced by
the reaction of 0.550 mol of
spectator ion?
10.107 How many moles of carbonate ion can be converted to
carbon dioxide and water with 4.42 mol
10.108 Calculate the mass of solid that can be produced
by the reaction of 0.300 mol of with excess .
10.109 How many moles of sulfite ion can be converted to sul-
fur dioxide and water with 0.650 mol
10.110
Calculate the number of moles of each ion in the final
solution after 1.75 mol of aqueous
CO
2
2
CO
with 1.25 mol
H
?
3
H
.
of
10.114
Calculate the mass of
Ag
2
S
BaSO
4
that can be produced by
S
2
Ag
2
the reaction of 0.234 mol of
SO
with 0.125 mol
4
Ba
2
.
of
10.115 Calculate the mass of that can be produced by
the reaction of 0.105 mol of
H
?
PbI
2
Pb
2
with 0.400 mol
BaCl
2
and 2.70 mol
of I
.
of aqueous
AgNO
3
are mixed.
General Problems
10.116
List the steps necessary to do each of the following
stoichiometry problems:
(a) Calculate the number of moles of aluminum metal
required to prepare 6.11 mol of solid
(b) Calculate the number of grams of
10.121
How many moles of
H
2
can be prepared using 0.500 mol
of silver and excess
10.122 What mass of barium carbonate can be produced by
treatment in aqueous solution of 31.2 g of sodium hy-
drogen carbonate with 30.0 g of barium nitrate?
is also produced.)
10.123
Heating of solid sodium hydrogen carbonate is one step
in the industrial process for production of washing
soda—sodium carbonate. Carbon dioxide and water are
also produced. Calculate the mass of solid produced
when a 2.11-kg sample of sodium hydrogen carbonate
is heated.
10.124 (a) After 2.06 g of solid is heated for a brief
time, 1.18 g of KCl has been produced. What mass
of has been produced?
(b) What mass of remained undecomposed?
10.125
(a) A 1.221-g sample of a mixture of and
was heated for a brief time, after which
0.998 g of solid remained. Write the balanced equa-
tion for the reaction, indicating which of the sub-
stances is the catalyst and including the states of all
reactants and products.
(b) How many grams of oxygen were produced?
(c) How many grams of decomposed?
(d) How many grams of KCl were produced?
(e) What is the minimum mass of
H
3
PO
4
?
Al
2
O
3
.
(CO
2
Ca(OH)
2
(s)
re-
quired to prepare 0.885 mol of
Ca(ClO
4
)
2
(aq)
by
reaction with
(c) Calculate the number of grams of that can be
prepared from 6.16 g of CO(g) and 3.60 g of
10.117
Calculate the number of moles of each substance ex-
cept water in solution after 3.11 mol of NaOH(aq) is
added to 3.82 mol of
HClO
4
(aq).
CO
2
(g)
O
2
(g).
HC
2
H
3
O
2
(aq).
Why was water
excluded?
10.118
In each case, calculate the mass of the product other
than water:
(a) 75.0 g of sulfuric acid is treated with sufficient
aqueous potassium hydroxide so that the acid is
completely neutralized
(b) 75.0 g of aqueous sodium hydroxide is treated with
excess chloric acid
(c) 75.0 g of solid magnesium oxide is treated with
excess hydrochloric acid
(d) 75.0 g of gaseous dinitrogen trioxide is treated with
excess aqueous sodium hydroxide
10.119 Rewrite Problem 10.33 as a single-step problem.
10.120
(a) Write three stepwise equations for the reaction
of NaOH and using only 1 mol of NaOH
in each step. (b) If we add 1.50 mol of NaOH to
1.00
KClO
3
O
2
KClO
3
KClO
3
(s)
MnO
2
(s)
KClO
3
KClO
3
that was
present originally?
10.126 After 0.0800 mol of solid has been heated for a
period of time, 0.0188 mol remains. Calculate the mass
of each product.
H
3
PO
4
,
KClO
3
mol of
NaH
2
PO
4
,
how many moles of
Na
2
HPO
4
and
Na
3
PO
4
will be present at the end of
all reaction?
