crovide names or formula as required.
If more than one name is possible,
provide both the I.U.P.A.C. name and the GUS/IC name:
K2S
potassium
sulphide
lithium phosphate
Li3P04
K2S04
potassium
sulphate
lead(II) perchlorate
Pb (Cl04)2
K2S03
potassium
sulphite
stannic chlorate
Sn(Cl03)4
Na3P04
sodium phosphate
antimony (V) sulphide
Sb28s
Ag2C03
silver carbonate
cobaltic
CO(N03)3
Mg(N03)2
magnesium
iron(III)
nitrate
copper(II)
Cu (Cl03)2
cupric chlorate
nickel(II)
NiS04
chlorate
nickelous
sulphate
sulphate
nitrate
carbonate
Fe2 (C03)3
bismuth (V) chloride
BiCls
sodium phosphite
Na3P03
mercury (II) cyanide
Hg (CN)2
iron (II) hypochlorite
Fe(ClO)2
Zn (ClO)2
zinc hypochlorite
carbon (IV) sulphide
CS2
V2 (C03)s
vanadium (V) carbonate
gold(III)
AU2 (804)3
Mn803
manganese (II) sulphite
phosphorous
iron(II)
plumbic periodate
Pb (104)4
ferrous chlorite
stannous
8n(OH)2
gold(III)
manganese (IV) oxide
Mn02
auric nitrate
gold(I)
Au2C03
Sc (N02)3
scandium
nitric oxide
N20S
CrS04
chromium (II) sulphate
iron(III)
sulphate
Fe2 (S04)3
Cr (S04)3
chromium (VI) sulphate
ammonium
phosphate
(NH4)3P04
Fe (Cl02)2
Au(N03)3
chlorite
nitrate
nitrite
sulphate
carbonate
hydroxide
carbonate
P2 (C03)3
Fill ir. he following table to show the oxy-anion
ls learned in class.
Be sure to show thL brmula
of each ion, the charge carried by each ion and the correct name for each ion. In the last row
along the bottom, show the three other polyatomic ions we have learned (formula charge and name) .
Cl041perchlorate
C032-
N031-
carbonate
nitrate
NO/-
nitrite
P043phosphate
P033phosphite
so/-
CIO/-
sulphate
chlorate
SO/sulphite
Cl021chlorite
Cl01hypochlorite
10/periodate
Br031bromate
10/iodate
2.
double displacement
potassium bromide
that results
in calcium
3.
decomposition
compound
6.
double displacement
phosphite
9.
decomposition of gallium hydroxide to form a common molecule
an ionic compound composed of only two elements
of sodium carbonate
between
osmium
produces
phosphate
and
a gas and an ionic
(VI) carbonate
and potassium
and
1.
Complete and balance each of the following equations.
These
equations are in the order of synthesis, decomposition,
single
replacement, double replacement and hydrocarbon combustion:
a)
cadmium chloride and ammonium
displacement reaction
b)
ferric oxide undergoes
fluorine gas
phosphate
undergo
a single replacement
a double
reactions
with
3.
What mass of potassium hydroxide is need to react with 22.2 g of
hydrogen sulphate according to the following equation?
What mass
of potassium sulphate will form.
4.
How many grams of toluene (C7Hs) are required to react with 25.0
L of oxygen at S.T.P. in a combustion reaction.
1.
For the double displacement reaction between sodium sulphate
and gallium(III) nitrate determine the mass of gallium(III)
sulphate that would form from the reaction of 50.0 g
gallium(III) nitrate
2.
For the combustion reaction of 100 L of butane gas (C4H10) at
S.T.P., what volume of carbon dioxide will form at S.T.P.
and what is the maximum mass of water that could be
collected
1 mol C4HlO
100Lx
-----x
100 L x
1 mol C4HlO
22.414 L C4HlO
22.414 L C4HlO
8 mol CO2
----x
2 mol C4HlO
22.414 L CO2
-----
1 mol CO2
x 10 mol H20 x 18.02 g H20
2 mol C4HIO
1 mol H20
- 400 L CO2
_
3.
For the reaction shown below, 50.0 g of hydrogen carbonate
is reacted with 35.0 g of BF3•
6.58 L of HF(g) is collected
at 750°C and 18.00 atm.
Use this information to determine
the percentage yield of this reaction.
Be sure to follow
the problem solving format used in class for questions of
this nature!
Beware the unbalance equation!
0.806 mol H2C03 x
2 mol BF3
I
3 mo H2C03
- 0.537 mol mol BF3 required
1 mol BF3
35.0 g BF3 x ---- 0.516 mol BF3 available - LIMITING
67.81 g BF3
0.516 mol BF3 x
0.516 mol BF3 x
3 mol H CO
2
2 mol BF3
6 mol HF
I
2 mo BF2
18.00 atm x 101.325 kPa
1 atm
3
-
0.774 mol H2C03 required
- 1.55 mol HF
nRT
p
kPax L
1.55 mol x 8.314 --
x 1023.15 K
Kxmol
1823.85 kPa
actual yield
% yield
= th eoretIca
. I . ld x 100 %
Yle
6.58 L
% yield
= 7.22 L x 100 %
4.
A 25.00 g impure sample of potassium carbonate is sufficiently
heat to completely decompose the potassium carbonate (into the
usual products for the decomposition of a carbonate).
The
residue mass (includes the impurity and the solid product from
the decomposition of potassium carbonate has a mass of 17.93 g.
Use this information to determine the % purity of the original
sample.
-
-
pure mass
.
x 100 %
Impure mass
22.2 g
25.0 g x 100 %
28.0 kg of ammonium nitrate is exploded through the above
decomposition
reaction.
If the final temperature of all three
gas phase products is 1815 DC and the explosion is confined to
a total volume of 5000 L, how many atmospheres of pressure will
be reached by this explosion.
28.0 kgx
1000 g
k
1 g
nRT
V
kPax L
1224.08 mol x 8.314 --
Kxmol
1 atm
4250.22 kPa x ---101.325 kPa
x 2088.15 K