pollution-free. Gases at ... of organic solvents exist that offer an extended potential range for waste oxidation ... hi,h-value chemical feedstocks from waste biomass [20], little .... A Pine. Instrument. RDE4 potentiostat was used for voltage sweep ...... the limiting current for a reversible reaction controlled only by mass transfer is.
December FINAL for
the
Period
REPORT
January
ELECTROCHEMICAL
December
1987
INCINERATION
Prepared L.
0 ,J
1989
OF WASTES
by
Kaba, G.D. Hitchens, and J.O'M. Bockris Surface Electrochemistry Laboratory Texas A&M University College
Station,
Texas
Prepared
77843,
U.S.A.
for
A/,¢ _z_-
(NASA-CR-12.5317) I_CINCRATION OF 19tl/ l]ec. IQg'_
1989
!:L _-C T _,uC H_ _ I CAL :_A?,T[S Fin_,I pe_,ort, (T_:_x_s A_,M Univ.)
/77p
_91-!$15_ J_.,n. -_:_ _ C _CL I )_
ELECTROCHEMICAL
L.
Kaba,
INCINERATION
G.D.
Surface
Hitchens,
OF
J.O'M.
Electrochemistry
Department
of
College
Bockris
Laboratory
Chemistry,
Texas
Station,
WASTES
Texas
A6_
778A3,
University U.S.A.
INTRODUCTION
The
disposal
increasing
public
wastes
into
years,
it
On
other
the
housing
New
the
has
developments
are
that
situation,
dissipatin_
oxides
of
low
to
the
site
in
and
converted
is
desirable.
the
combustion
of
in
environment
and
a
space
carbon
which
waste
monoxide
be
used
the
state
as
sea
to
during
for
is
chemicals is
undesirable
and
the
offer
the
to
due
the
by
be to
gases
several
any
NO
are
utilize
recycled. the
In
difficulties
presence
[5,6].
advantages
of
[3,4].
wastes
to
inevitable
effluent
absence
can
new
and
desireable
that
20
for
operate
posed
reject
last
and
and
of
[1,2].
chemicals
problems
it
to
the
cities
build
acceptable
where
a matter
unacceptable
to
The
is
permissible
but,
systems
expensive
in
and
raw
environmentally
into
techniques
may
of
vehicles
wastes
its
regarded
drainage
is
space
_iectrochemical
of
Here
in
including
and
CO
in
the
the
_ases.
l#ork papers,
and
convert
heat
zem9eratures
evolve_
farms
is
will
nitrogen
particular.
this
in
was
sink
cumbersome
at
demanding
treatments
that
waste
Gases
it
infinite
clear
whereby
waste
Earlier,
apparently
sewage
particuiarlv
organic
concern.
hand,
pollution-free
of
domestic
become
technology
zhis
of
done
and
early
hitherto
the
present
stages
of
in
this
report
area is
a potentially
an
has
been
attempt
valuable
restricted to
give
a
technology.
to more
technological fundamental
basis
THEELECTROCHEMISTRY OF ORGANIC OXIDATIONTO CO2 Aqueoussolutions
have an electrode potential
window in which substances
can be oxidized without competition from oxygen evolution up to about 1.6 V on the normal hydrogen scale in acid solution oxidation potentials
at 25°C. Correspondingly,
of someorganic compoundsfound in humanwaste and
chemicals derived from biomass are shown in Table i. therefore,
to carry out a complete oxidation
of all
It should be possible, the components in fecal
wastes, including urea, to CO2 in aqueous solution.
Correspondingly,
of organic solvents exist that offer an extended potential
2), although the reduced conductivity presence of suitable
salts)
available
a number
range for waste
oxidation without competition from the oxygen evolution reaction
anodic potential
the
(see Table
in such system (even in the
would have to be taken into account [i0];
the most
used in the present work was 1.9 V versus the Normal Hydrogen
Electrode (NHE). On the solution,
there
systems
at
[i1,12]; wastes
it would
lithium The
in
view
of
material
is
650°C
may
a
be
at
of
650°C
of
with
bubbled
to
O°C,
during present,
oxidation
from
[131,
the
reactions,
the
waste
who
is
but
dissolution
the
of
known
in
of
into
in
the
about
[14],
Cu,
the
a
of
90%
the
the typical
potential. are
important
the
yield
temperature
was
of of
lowering
oxidation
it
conditions
oxidation presence
aqueous
carbonate
similar
reactions
when
CO 2 on
Kolbe-like
coal
or
application
that
in
molten
thermal
oxidation
found
incomplete
these
of
oxygen
reduction
little
under
without of
is
them
degree
mixture
Horri
wastes
oxidation
coefficients
work
of
introducing
considerable
carbonate
At
oxidation
anodic
a
the
formed
the
using
that
temperature
of
if
possibility
and
occur
obtained.
organic
hand,
potassium
temperature was
ocher
of
coefficient
reactions
found
methane
that,
of
(dE/dT)
- 4xlO"3 V/°C and (dl/dT) of coal product, it
" 0.i mA/°C. From considerations
seemedthat - an expected range for the oxidation of
wastes would be around 1.0-1.5 V (vs _E), significantly
of the oxidation
thus, not enough to decomposewater
on platinum.
The electrode materials
for waste oxidation
in aqueous solutions
should
be inexpensive, remain un-oxidized under the highly anodic conditions an oxide) and be a poor electrocatalyst
for oxygen evolution.
often used for organic oxidations since it a battery material) This field
(i.e.
be
Lead dioxide is
is highly conducting (it
is used as
and has a high overvoltage for oxygen evolution
[15,16].
is open to new oxide electrodes that have cometo be used in recent
years [17].
._nongthese are the perovskites
[18], where the addition of 20-
30%barium oxide to the materials such as lanthanum nickelate
allows a
conductin_ oxide to be used as an electrode which is stable to oxygen attack. In addition,
Ebonex (Ti407) may be used which is an extremely stable anodic or
cathodic material
in acid environments [19].
AlthouBh, electrochemical hi,h-value available
oxidations are an important meansof obtaining
chemical feedstocks from waste biomass [20], little on the complete oxidation of carbonaceous material
information to CO2.
is
Bockris
et al El_ showed that carbohydrates are completely oxidized to CO2 during electrol"sis,
initially,
the electrolysis
carbohydrates.' such as sucrose, cellobiose
was performed on simple (_.D-glucose dimer) and glucose, in
&0%H3?C i or f_: NaOHat temperatures of 80-I00°C. (52 cm2) :_as used as the anode. The reactivity increasinB complexity.
Nevertheless,
A platinized
platinum gauze
decreased for molecules of
it was found that cellulose
broken down to CO2 with a current efficiency
could be
of around 100%and only 2
faradays were involved in the evolution of I mol of CO2 perhaps because of
preliminary studied
on
The
anodic
platinum
in
generation
of
utilized
based
on
oxidants
of
of
for
urine
the
generation CI"
organic
and
used
from
an
humans
activated
and
was
lost.
although
the
No
electrochemical
method
Delphi
Inc
Research
redox
of
couples
_;aste
effluenc
which
material
which
of
such
contained
this
and
showed
that
to
of
activated
of
treating
electrochemical
the of
50
mA/cm
of
the
has
been
monoxide
or
urine
strong
chlorine
and
were
An
developed
holding
into
of
_he
odor
available,
"indirect"
used
tank.
chips
oxides
be
recently
were
fecal
of
could
products
electrodes
wood
a
2", furthermore,
detected.
a waste
and
mixture
100%
planar
generation
waste
CI 2 was
approach, to
of
were
close
generation
mixtures
that
the
the
and
using
been
as
Also,
the
electrolysis
OCI')
OCI',
manure
carbon
systems
of
treatment
cattle
no
studies
has
production
02
circulated
as
These
HOCI
the
the
approach
support
(CI 2,
estimates
C02,
In
life
chlorine
a current
waste
[8]. were
regenerative
This
about
the
quantitative
of
bring
solution.
electrodes,
using
evolution
themselves
by
include
Through
clarified
indirectly
by
means
platinum
achieved
removed
agent.
[10,25].
decolorized
be
features
on
the
[9,23,24].
could
be
which
in
in
effective
chlorine
quickly
urine
can
agents
activated
bleaching
as
mixtures
material
material
disinfectant
waste
waste
of
been
[22].
oxidizing
in
Additional
been
NaOH
Oxidation reactions of casein have
purification
electrodes.
has
IN
carbonaceous
from
the
reactions.
electrolysis
oxidation
of
hydrolysis
by
to
The
regenerate
conversion
a pollution-free
nitrogen
was
achieved.
The
of
use
use
potentials
of
various
of
new
without
flow
electrocatalysts,
interference
systems
to
of
increase
organic
solvents
oxygen,
wider
the
contact
to
increase
temperature
time
and
the
ranges,
eventually
range
the
carbonate
and
investigation.
other
molten
salts,
belong
to
a later
stage
of
the
METHODOLOGY
Electrochemica_
¢e11_
Two
kinds
of
The
cell
shown
electrolytes
the
counter
of
the
cell
sparging
the
gases
magnetic
follower
packed
with
solution.
a
The
thermometer
After
each
500°C
in
washed
For
experiments
added
from
electrolyte
the
electrolyte a00
was ml.
designed
so
lead
The
that
dioxide
was
Pine
and
stirred
it
on
Instrument
and the
with
working
rod
placed
3 cm
[9];
a hot
a
cc's.
Both
the
the
top
of
cell
in
with
the
nitrogen
gas
finally
was
waste
was
400
means
of
was
by
a
a
tube
hydroxide
was
a
hv
monitored
ground-glass
_reatment
_ashed
in
with
of
cell
used
was
25
cm
off-gases
biomass
a magnetic were
of
counter
the
urine
(Figure
2).
Argon
was
collected
as
high. were
and
follower.
The
either
a platinum
volume
of
electrode
was
the
used
(in
an
sulfuric
The
used
the
cell
to
of
foil
cell
in
on
both
potentiostat
was
used
for
voltage
an
sparge
described
volume
absence
had
CO 2
above.
The
electrolyte (I00
both
cm2),
sides,
cases,
plate.
RDE4
glass
a barium
using
products,
and
ground
temperature
_le_ned
cc's,
working
through
to
acid
water.
mixtures
was
the
which
a
carried
2.
in
stirring
was
and
cell
organic
as
additional
compartment
most
Pt
200
anodic
electrodes
occupied
compartment
the
distilled
_:ork
was
trap
glass
the
I and
anodic
and
eliminate
a U-tube
of
plate,
the
involving
all
Figures
a hot
experiment,
with
in
the
outlet
a water
into
for
and
The
through
fitted
shown
supplied
rpm.
on
of
of
through
rested
electrolyte,
used
electrolyte
6,000
to
are
compartment
the
finally
diameter
was
continuously
air
internal
and
volume
fitted
from
cell
and
A
used.
wool,
acid
cell
i,
at
at
a
Figure
was
oven
_as
in
cathodic
glass
The
joint.
of
used,
were
The
Aooaratus
were
electrodes
joints.
using
cells
were
volume
and
sweep
the
or
experiments below.
and Current
recorded
_aste
on
waste
of
sewage
its
and
contents
from
these
obtained
in
obtained
from
consistency
and
the
I_
weight.
All
For
the
was
weiBhed
sulfuric
_ave
_:as
made
described
time
curves
were
704AB).
a
strong
monitored
waste
involving
treated
sonicator
q Bm
O_ C
C3 q
C_'_
_V J
O_ _//t"
i
in=
I
_s
0
0.6
0.8
.tr
_/LT
I
1
1.0
1.2
J
i
1.4
1.6
Potential/V (NHE)
FL_=e
L5 :
Cu==enc.Eo=en=ial
cuz-ves for
dlfferen_
concen=ra:Lons
g/1LCec.
O
ra=e
i
=v/s.
I0 g/iL:er). T -
150"C.
of
oxide=ion
=ase£n
(_
Potential
of
case£n
_/!i=e=; l_=ics 0.5 -
Ln L2 _ H2SO_ for _
_ g/liter;
2 v (N_K).
_ Scan
6
4 -e-FIG.
16
OJ
E _me
_o
2
r_
L-L.-
•
•
O
0
!
1
2
4
Casein
FL_u=e
t6:
Effecu densi=y
of a=
concen=ra=ion in
eieccrode-po=enclal
OF POOF:
_
6
8
concentrationlg
casein 150"C
i
"_ ....... ,,'
j
10
=he
anodic
12 M H2SO _ from
=he
volcameuric
0.5
- 2.0 v
12
liter-1
on
limit
I
(NHE).
Limi=ing
Scan
current
behavior rage
l=v/s.
at pc
¢q
.p
i
E t.. "4r f om
U3
'lr
m
r_ J
J
k., t__
4
"t
.I¢ I
m
r-
0
i
0.6
0.8
I
i
1.0
1.2
PotentiaW
Figure
17
Currenc-pocenuial different
curves
=emporacures.
for exidaulon ( •
I
1.6
(NHE)
of casein
25"C; "_ 80"C; _
limits 0.5 - 2 v (N'HE). Scan race i mv/s. g/flier.
I
1.4
in 12 M H250_
150"C).
a=
Pocen=iai
Casein ¢onconcraulon
14
-2.6-
-2.8 -
Owl !
E
-_.0
-
-3.2
-
0
u
m em W
c o
log
i/Acre'2
40
o 30-
_._
20-
o 10-
0 !
•
0.0
,
2.5
b
_
5.0
7.5
Time
Elec=rochem¢cai H2$0 _ u.sing _/ltcer.
OF
?C_>,_ +..,:-:,:._-._ l'Y
l
i
10.0
12.5
15.0
of electrolysis
produce!on a P=
i
i
eiec:rode
of
CO2 dt_lcing
a=
150"C.
J
17.5
i
t
20.0
22.,5
(hours)
case£n
CaJle£n
electrolysis
concen=r&=¢on
_n 1_
12
"0
C_ t
8-
0
Potentiai/V
Figure
21"
Effec= density
of a_
eiec=rode.
yeas= 150"C
concen=racion in
Poten=ial
( •
2.5
g/li=er:
_!7.5
and
35
g/li=er).
12 M
SO_
limi=s
on from 0.5
5 g/liuer:
_
(NHE)
:he =he
anodic
!mzi:ing
vol_ammecric
2 v
(NHE).
Scan
7.5
g/liuer:Ol2.5
current behavior raue
ac
i mv/s.
g/li=er:
P:
_
A A
w
5-
4
/
== i tno
° ..e
/
/
° U V
;
10
3
Yeast
Effec= :enszcy
of yeas= a=
eiecurode.
150"C
Pocen=iai
!
30
concentrationlg
concen=ra=ion in
J
20
12 M SO4 limius
on from 0.5
=he
anodic
liter- 1
iLmi=ing
=he vol:amme=ric 2.0 v
(NHE),
curren=
behavior Scan
race
ac
P:.
i mv/s.
7
0.6
0.8
1.0
1.2
1.4
Potential/V
Figure
23:
Currenc-Po£en_ial differen_
curves
=8mgera=ures.
¢oncen=ra=ion
i_
g/l_:er.
for
( •
1.8
(NHE)
oxida=ion
Potential
1.8
of
lim_s
2S'C;
+
yeas_
0.5 80"C;
in
- 2.0 _
12 H H2SO a a_ v
(N_E).
120"C;
O
Yeast 1SO'C).
:.C
-2.0
@
-2.5 -
CJ
E -3.0
-3.5
i I
2.0
i
2.2
2.4
2.6
1/T=K
Fi-u.':_
"'
;aria=ion -_mDera=ure.
of
:he Yea/_
,+ .
limi:in
I curren_
concen=ra:ion
i
i
2.8
I
3.0
3.2
103
dlniit-y 23.4
as
g/li_er.
func:ion
of
t
3.4
Q
1.6-,
UJ
Z >
/
I
iI
C 0
ft.
08
..
]"
6
d
-5
-4
log
.--!_r_
25 :
Curren=/Po=enr-£al
< A),
for
yeas=
in
i/Acre- 2
reia:ionship
a=
12
Yeas:
M
H2SO_.
-3
80"C
(0),
120"C
=oncen=ra=£on
([_),
23._
150"C
g/li:er.
6O A
cO
¢/3
_.¢
c_J
0
0 w
m
0 k-
4
6
Time
.--L-u:_..=
"-'"
Elec:rochemical H2$0 _ _/licer.
°
using
a
8
12
14
16
18
of electrolysis (hours)
pro_uc:ion P_
10
eiec:rode
of CO 2 duping a_
150"C.
yeas:
Yeas_
elec:roLysis
concen_r&_ion
in 1_
!2
2.0
A
UJ
:3: Z > n oiBm
q) W
O
I
-2
log
- i _',:.:: •
Z-
Curren=/pocen=ial cellulose
([]),
reia=ionship casein
(/_),
i/Acre- 2
at and
!50"C yeast
for (0)
oieic in
acid 12
M
(0) H2SO4.
/ .--.....t
6 ;..J_er" 9.38 g.,_er" 18.72 g.,ter"
--.e-
23.4 g.,ter"
3.5 _j m
/
< _m am em
/
>" 2.5-
4me .el
c-
w
F I
i
i
"
0.5
l_otential/V
Currenm-po=entlai
Fixate 28 :
waste
_-;.
,. "_
curve
(NHE)
for :he oxicht=ion of
in 12 M H2SO _ on P_ for different
?o:enulal
:,,
1.5
1
limits 0.5 1.8 v (NME).
ar:ificial
concen_raclons
Scan rate I mv/s.
fecal
of waste. T - 150"C.
Figure
29
A v
10
20
30
Dry waste concentration/g
Fibre
29:
Effec= density P=.
of aU
elec=rode.
dry wasue 150"C
in
concen=ra=ion 12 M H2SO _,
Po_en=ial
limits
A _
on
from 0.5
4o liter"
=he
anodlc
uhe volu_eurlc - 1.8 v
(NHE).
limi=ing
current
behavior Scan
ra_e
at i
_V/S.
_'* '*-""':
QUALITY"
-S
A
< =
-/
Z.
;
2.4 1/T'K
OF
PO0;_
Variation
of :he
ano_ic
zemoera=ure
on P_.
Wasue
QUALITY
Z
,
2.6
!
2.8
w
1#
iimi=in 8 curren= concen_ra=ion
dez%siry
23._
as
g/li=er.
a fu_%c=ion
of
_
9
OJ
/
_em
w ,m
.,q
u_ /
E3 / dm,e
/
2-,
® /
/ C_
Potential/V (NHE)
.=i_=e
31;
Curren= au
pocan_ial
dlfferenu
Ar:ifical !20"C;
curves
_a_perauures
was_a
for on
concencra=ion
oxida=ion
9_.
of
Pouanuial
23._
g/li=er.
ar=Ificial limi=s (_
fecal
wasue
0.5
2.0 v
(N_E].
25"C;
4, 80"C;
*
O150"C).
'-',_' _ ", _'-'!', QUALITY
-e.-2 '-,e-
, IO'_M S , 10"_M
Pe !
E J
/ /
emm .me
C
u
L_
D
1.0
" 1.5
PotentiaVV
_urren_-Pouen_iai im 12 M H2S0 _ usin$ _a"+.
:" ....."""'_;
i_AGE IS
OF F_CO._; QU/_,LITY
curves
for oxida=ion
a P_ eiec_:ode
Sweep raue _ mv/s.
(NHE)
of ar=ificial
for dlfferen_
fecal waste
concencra=ions
of
A
0
0 Imb
0 0 0 C 0 tomb
m
Gram
0
0 0
5
10
15
Time of electrolysis
?i_-_re 33:
CO 2 production P= electrode
a=
dur_n_ 150"C.
20
(hours_
biomass
eieccroiysLs
in
12 H H2SO _ using
Biomass
concencra=on
14.OA
g/lizer.
a
-T--"
"
13
C_ q
/ I
o_
@
r_ I J
10
0
20
30
40
Time of electrolysis
?L_e
_
Total _ix_ure
nltro_on of
concencranion Currenu
conuen_
aruifical 15.3
I - 800
MA.
variation
fecal
wasuo
3 g/liter.
wig and
7O
(hours)
eloc=rolysis
uring
Platinum
60
50
at
time
60"C.
electrod_
of a
Dry waste
aria
I00
sq.
cm.
25O A
0
200 -
150
i 100
ii
10
0
20
30
443
50
8t3
-
Time of electrolysis (hours)
C02
produc:!on
PbO 2 electrode g/li=er.
durin_ at
Curren=
60"C
ar:ificial Ar=ificial
I - 800
MA.
fecal fecal
waste wasue
electrolysis concen=ra=ion
using 12.2
a 2
7
6
\
k,w W ,m m
5 \
©
\ \ \
3
m
i
0
10
20
30
Time
Fizure
47'
Toual
of
organic
arulficial
]7"C)
aiecurodes
(
carbon
facal
60"C).
area
variauion
was=e
Dry
i00
of
sq.
and
was=e
cm.
4O
50
electrolysis
wi=h
urine
=wo
Currmn=
13.5
I
-
=ime
differen=
co.cenurauion
800
7C
(hours)
eiecurolysis
a=
60
MA.
3
of
a
mixuure
=emperauures
g/liuer.
P=
(
12
8 t__ W e_ I
6
o 0 k-
0 0
i
I
j
10
20
30
40
I
I
50
60
Time of electrolysis
Figure
_.8 :
Total
of
organic
ar=ificial
waste
carbon
fecal
concentration
variation
was=e 13.3
wi=h 3
wi_h
urine
g/liuer.
I
60"C
Current
80
90
(hours)
electrolysis
a=
I
70
on I -
time
PbO 2 800
of
a mixture
elec=rode. HA.
Dry
--NO
I HCO_ EQ.
POINT
_./
USABLE
I
8
"-2
pH UNITS
IN 50-+5
ml
(PHENOLPHTHALEIN) 6
4
If_wCO2 EQ. POINT
_!
--
----BREAK
OF
t _
2
1 0
I ,
20
40
I
I
I
60
80
100
MILLILITER Figure
.',9-.
Ti_ra$ion
_
IN 100 -+5 ml
(.RO.CRESOLpH UNITS ,ET.,L RED) --2 120
0.04 N TITRANT
curves
forS_
;aOH (curve a) and HCl (curve h).
cc
50cc
of
of
.04M
.04M
R2CO 3 with
Na2CO 3 with
.04H .04M
HCO 3 EQ. POINT CO2, HCO;----_ BUFFER
"
REGION_
.
1.o
J
I
0.5 _._/_._ 'f CO...'" ". ///.'." ////
/_//_,_"/ "/'_"" /' "'
2
0
11
/HCO_'.
I
_BUFFER
!
I
...-._,,
REGION
. I
V::::::_:-HCOZ, -,:';::::_._'_.."-_\.CO_-.\"-
""(" :/. _ii._._" :"_:'"::';:'"":'"'"'"":':':':':'""
4
CO 3
6
8
_'\\\\_"
10
12
specles
as
14
pH Figure
50
Fractions
of
carbona=e
a
fun¢=lom
of
pH.
• .
J'
\
_.
-
........
_, "
r'-
,..,,_
" -.',:;E'.IS
i_OOi','OUAL/TY
Eo
Urea
-0.738(a
GLucose
-0.36
)
Formaue Manni:ol
+O.02(a
Succina_e
+O.ll(a)
Glu=amine
+O.ll(a
)
Bu=araldehyde
+O.ll(a
) (Kp)
Adenine Acid
$accnaromvc_s
cerevi_
Peak
or half
wave
(a)
Caiculaced
(b)
0.LM
(c)
Aqueous
(d)
2M H2SO A on
(e)
0.LM
from
NaOH
(E_)
potentials AGof
on
Pla=inum.
buffer
(pH
are
values
5.7)
on
signified given
in Ref
[_"
i.
40.
graphi=e.
phosphate
"
_
platinum.
buffer
(pH
7.0)
on
graphite.
32 "
by
-0.432
[38]
+l.O(b)
[22_
)
Casein
Uric
Ref
EP/2
or _/2
+1.25(c
)
C3B7
+0.86(d
)
[3s!
+0.98(e
)
[39!
repec:iveiy.
Solvent
Acetic
Anodic
Elec=roiyce
acid
Limit
NaOAc
+2.0
Acetone
(nSu)4NCl04
+i.6
Acetonitrile
LiClO 4
+2.5
Acetonitrile
(Et)4NBF
Dimethylformamide
(nBu)4NClO
4
+1.6
Hethviene
(nBu)ANCl0
a
+1.8
Nitrobenzene
(nPr)ANCI0
_
+1.6
Nitrcmechane
Mg(ClO_)
Propyiene
chloride
carbona=e
+3,2
4
2
+2.2
E=ANCIO
A
+1.7
P vridine
EtANCIO
A
+3.3
Suifoiane
EtANCIO
_
+3.0
Te_ranv_rofuran
Et_NCIO
A
+1.6
33
Contents
_asce
Component
Cellulose
Casein Oleic
acid
of Art!flcial
Fecal
Weight
Waste
(kg)
% Of
Total
Dry
0.60
33%
0.43
25%
0 12
7%
0 17
10%
0 37
20%
KCI
0.04
2%
_;aCl
0 04
2%
3aCi_
0 03
i%
_a_er
2
Weigh=
S
34
ii ,__,_
