Figure 1. The moles of condensed nitrate against temperature in a
ternary system of RNC-sulfuric
acid-nitric
acid
at
fixed initial water vapor
of
0.07848 mol (equivalent to 60% RH at 263.15 K and 101325 Pa in 1
m3). All curves have the same initial moles of
HNO3, H2SO4 and the RNC
as
1.11151×10−9,
2.03777×10−11and
8.86895×10−8,
respectively. The legend on the right indicates which RNC is present in
each trace. (a) includes all RNCs in Group I (defined in Table 1) and
MEA (as comparison) and (b) includes all RNCs in Group II and ammonia
(as comparison).
To further elucidate the reason for such significant difference inTc values among amines, the properties of several
amines with distinctively different functional groups were compared
(Table 1). Neither gaseous basicity (GB), aqueous basicity
(Kb ) or the volatility of an RNC or its nitrate
salt (psat and Kp ,
respectively) seems to directly determine the Tcof an RNC. For example, DMA and MEA have similar GB values yet
distinctively different Tc . When compared with
PZ, TMA have a similar Kb yet aTc that is ~ 28 K lower. PZ has a
much higher GB than MEA but their Tc values are
comparable. AN and MEA have similar saturation vapor pressures at room
temperature yet distinctive different Tc , ruling
out any direct contribution on Tc from the
volatility of the amine. The solid/gas dissociation constants of the
nitrates of alkylamines are about 10 times lower than that of ammonium
nitrate yet they exhibit comparable Tc ,
suggesting that saturation condensation of nitrate salts alone may not
explain the difference in Tc for Group I and II
RNCs. Furthermore, the molar mass of IBA is about 50% more than that of
MEA, but their Tc values are essentially the
same, suggesting that Van der Waals forces do not contribute
significantly here. It appears that the electron affinity of the
functional groups on the amines has little effect on theTc . For example, the nitro group in AN-N and the
methyl group in AN-M are electron withdrawing and electron donating
groups, respectively. However, both RNCs showed little contribution to
NA condensation at above 260 K.
One distinctive observation is that amines with only alkyl (e.g., MA) or
aromatic (e.g., AN) substitutions showed much lowerTc than those with hydroxyl (–OH) groups (e.g.,
MEA). Furthermore, IBA and PZ, showed Tc values
comparable to that of MEA, with the former having a similar chemical
structure as MEA, while the latter having a second amine group (–NH–)
in the ring (Table 1). Since MEA and PZ do not share the same functional
groups, their high Tc values could not be
explained alone by the presence of –OH groups in the chemical
structure.
Based on these observations, it is proposed that the ability of RNCs to
form additional hydrogen bonds plays a critical role on how RNCs may
facilitate the condensation of NA on nanoparticles. Generally, theTcvalue will increase significantly when a RNC can form more hydrogen
bonds. MEA, PZ and IBA, with one additional hydroxyl or amine group than
monoamines, have Tc values of ~
300 K. DAE, DGA and DIPA with two additional hydrogen bonds, showedTc values as high as 323 K (Table 1), allowing NA
to condense above room temperature.
Another factor that may affect the Tc is
hydrophobicity. AN and AN-M both contain an aromatic ring which is more
hydrophobic than a methyl group. The decreasing solubility of amines in
water results in less NA condensed and dissolved in the particle,
greatly diminishing the condensation of NA compared with MA. In the case
of AN-O, the –OH attached to the aromatic ring can form additional
hydrogen bonds, which seems to offset the negative effect of the
non-polar aromatic ring and increase the Tc to
289K (+15 °C).
To evaluate the Kelvin curvature effect [Zhang et al, 2012] on the
condensation of RNC and NA, the saturation vapor pressurepsat of MEA was increased by factors of 10 and
102; the corresponding Tcvalues decreased to 296 K and 288 K, respectively. This analysis
suggests the significant impact of particle size on the condensation of
NA in the presence of RNCs.
Although Figure 1 and Table 1 well demonstrate the enhancement of NA
condensation by the presence of amines, ambient concentration of amines
is normally much lower than 1900 pptv, nor would amines exist in the
atmosphere without a relatively high concentration of ammonia. In
reality, the ambient concentration of amines is usually 1–2 orders of
magnitude lower than that of ammonia, although the amine:ammonia mol
ratio could be higher near industries emitting amines, such as near a
power-plant using CCS technology. As a result, a chemical system of
ammonia, MEA, SA and NA with varying MEA:ammonia mol ratios was
investigated. Figure 2a illustrates the change of theTc value of an ASN system with varying amount of
the ammonia replaced with MEA. The enhancement of the NA condensation by
MEA is noticeable even at as low as 0.1 mol % (~ 2
pptv). It appears that as the mole fraction of MEA increases, theTc increases following an excellent linear
relationship (R2 = 0.99 and Figure S2):
Tc =9.1615×[−log(MEA%)]+305.33 (1)
where MEA% is the MEA mole fraction in total RNCs (mol %).
In additional to the structures and concentrations of amines, amount of
total water is another factor that may impact the condensation of NA.
Our further investigation (Figure S3) suggested that increase in the
total water vapor in the system leads to an increase inTc of the system, hence facilitating the
condensation of NA. However, the enhancement is not as strong as other
effects such as additional hydrogen bonding or hydrophobicity. A similar
trend was observed by Chee et al. [2019] when they studied the
nanoparticle formation and growth in a DMA-NA system.
(a)