Name:___________
Period:_____
Date:________________
Here is the equation to use for the first three problems:
N2 + 3 H2 ---> 2 NH3
1. If we have 2.00 mol of N 2 reacting with 4.00 mol H 2 , identify the limiting reagent and how many moles
of NH 3 will be produced.
2. Suppose 6.00 mol of H 2 reacted with 2.5 mol nitrogen. How many moles of ammonia would be
produced?
3. If 4 mol of NH 3 are actually produced in the scenario from problem 2, what is the percent yield of this
reaction?
Here's the equation to use for the next four problems:
2 H2 + O2 ---> 2 H2O
1. How many moles of H 2 O are produced when 5.00 moles of oxygen and 7 moles of H 2 are used?
2. If 3 moles of H 2 and .7 mol of O 2 are mixed which will be the limiting reagent? How much H 2 O would
be produced?
3. If only 1.2 mol of H 2 O are produced in the scenario from problem 2, what is the percent yield of this
reaction?
4. Suppose 4.00 grams of H 2 and 6.00 grams of O 2 are mixed, how many moles of water would be
produced?
Name:___________
Period:_____
Date:________________
Here is the equation to use for the first three problems:
2 NaOH + CaBr2 ---> 2 NaBr + Ca(OH)2
1. If we have 4.00 mol of NaOH reacting with 5.00 mol CaBr 2 , identify the limiting reagent and how many
moles of Ca(OH) 2 will be produced.
2. Suppose 7.00 mol of NaOH reacted with 2.5 mol CaBr 2 . How many moles of NaBr would be produced?
3. If 4 mol of NaBr are actually produced in the scenario from problem 2, what is the percent yield of this
reaction?
Here's the equation to use for the next four problems:
Na2S + 2 HCl ---> 2 NaCl + H2S
1. How many moles of H 2 S are produced when 5.00 moles of Na 2 S and 7 moles of HCl are used?
2. If 3 moles of HCl and .7 mol of Na 2 S are mixed which will be the limiting reagent? How much NaCl
would be produced?
3. If only 1.2 mol of NaCl are produced in the scenario from problem 2, what is the percent yield of this
reaction?
4. Suppose 4.00 grams of HCl and 6.00 grams of Na 2 S are mixed, how many moles of H 2 S would be
produced?
Name:
(J
Date: _ _ _ _ _ __
Period:
Here is the equation to use for the first three problems:
1. If we have 2.00 mol ofN2 reacting with 4.00 mol H2, identify the limiting reagent and how many moles
ofNH3 will be produced.
~.00 ... I H, •
1r,! M~J cc
3 .._., H'l.
~;?Mal NU
C
3
H,.L?"
=:_,;
2. Suppose 6.00 mol of H2 reacted with 2.5 mol nitrogen. How many moles of ammonia would be
produced?
3. If 4 mol ofNH3 are actually produced in the scenario from problem 2, what is the percent yield ofthis
reaction?
<-i ,-..o( r,J 11-,
- - - -1.. llO J60t,
@
'-IM<>INH}
Here's the equation to use for the next four problems:
1. How many moles ofH20 are produced when 5.00 moles of oxygen and 7 moles of H2 are used?
s.oo M.:.I e>..
2. ,.,...1 "i.0
----;;..,c
- : /0 ,..o\ i.l .,0
1
I ,...1 o.,_
7, dJ Mol U'l.
lt
z,.,. 0 f ,4._0 .,._ ~,....( ~
2-1~
~
2. If 3 moles of H2 and .7 mol of 0 2 are mixed which will be the limiting reagent? How much H20 would
be produced?
3. If only 1.2 mol ofH20 are produced in the scenario from problem 2, what is the percent yield of this
reaction?
4. Suppose 4.00 grams ofH2 and 6.00 grams of 0 2 are mixed, how many moles of water would be
produced?
~. oo.:! 1-f~ "
, ...... 1I{.._
)(.
Z..02jl41.
~.oo, ol.
l(
,...,.,(()'l.
::'>? .00-0.
~
1MDl fllc)
l"""ri.41...
1_ f'\O(
tf1 0
1...., I I).
--
I .'I 'r" NI ~h.O
Name:
K. G,-)
Period:
Date:- - - - - - -
Here is the equation to use for the first three problems:
2 NaOH + CaBr2 ---> 2 NaBr + Ca(OH)2
1. If we have 4.00 mol ofNaOH reacting with 5.00 mol CaBr2, identify the limiting reagent and how many
moles of Ca(OH)2 will be produced.
4 .00 '""'oL Ne.OH X
S.00 MO\ Co.Br,
J,... \C... (o~ =
)i.. ,.,. .
z.,....olN ~..i
-
\.-..lu. Br~
\
Ce..(o"\
~o.0'4
L; ..... d3
~\
---=------------
5 Mo\ Cc... Brz.
\..,,o\Co.lOlf\ -
"IC
0
-
2. Suppose 7.00 mol ofNaOH reacted with 2.5 mol CaBr2. How many moles ofNaBr would be produced?
7.CJO""ol ~o..O~
'leo\ No..~r ::: 7""" 0 \ l\lo. Br
l(
'l..,..ol
1.. S l"'\ol
Co. ~z.
tJo.OH
~ .J- Mal tJ ..k.
~
-=-
,~,c...Brl.
Co.. BrL L \
tJ.,. g,..
Mo I
IV\ ;
+0
3. If 4 mol ofNaBr are actually produced in the scenario from problem 2, what is the percent yield of this
reaction?
Here's the equation to use for the next four problems:
1. How many moles ofH2S are produced when 5.00 moles ofNa2S and 7 moles ofHCl are used?
7.
Mol
JtCl
"
I....,\ ~15 -- '-, .':) ,,.,. 0 j
t,11.;i
~i.-:>-_.-_._'-=-~~
2,...1 11 C.l
2. If 3 moles ofHCl and .7 mol ofNa2S are mixed which will be the limiting reagent? How much NaCl
would be produced?
3
J.\(.L
_i"\ol
__
_ ,.
s
----'JI.
. '""o\
IJQ'l.
21'\ol
fJo.Ll ::.
z......,1~L
l. MA\ tJ.,.u
I
1••
-~~
':
3.-..ol tJo,el
~I4
.
I
,I ll
. .
#'Jo..
MO "'"'
L)
S L,-.rJ
L
3. If only 1.2 mol of NaCl are produced in the scenario from problem 2, what is the percent yield of this
reaction?
4. Suppose 4.00 grams ofHCl and 6.00 grams ofNa2S are mixed, how many moles ofH2S would be
produced?
1./.005 ~ . ,
:,
,,.
l,.005
(""°\I\U K
Lfl. \l<.l
3G,
tJo.l.,~ >'-
. J
\-.11\.S _ ~
2 ...-., ll-4 C.l - ~.054'\
,_... I ~......s
7'l.ClS'~r-lo.z..~
Mol
1-42.S
/
x 1-1 ff,S
1....,1JJ..1.S
= C.Q7GPI Mol Jl1.,5