*2.1. NH3-SCR and NH<sup>3</sup> Oxidation Activity*

Figure 2 presents the NH3-SCR activity and side product N2O concentration of catalysts before and after Na poisoning. Before Na poisoning, Cu/SSZ-13 with different crystal sizes present similar NH3-SCR activities. It can be observed that between 350–400 ◦C, SCR activity increases with increasing crystal sizes. In this temperature range, the increasing temperature induces the active center Cu2+ to migrate from the solvated form (CuII(NH3)n(H2O)m) to the molecular sieve framework (Z2CuII or ZCuIIOH) [33–35]. The change in reaction activity is mainly dominated by the number of isolated Cu ions. Such trend is consistent with the copper content in order: 2.3-Cu (1.44 wt %) > 0.8-Cu (1.38 wt %) > 0.4-Cu (1.05 wt %) (Table S1). Thereafter in the higher temperature region (>400 ◦C), all samples have decreased activities, which is caused by the side reaction NH<sup>3</sup> oxidation reaction. The NH<sup>3</sup> can be oxidized to N<sup>2</sup> by either NO<sup>x</sup> or O2. The competition between SCR reaction and NH<sup>3</sup> oxidation by O<sup>2</sup> at high temperatures (>350 ◦C) is widely reported [6]. The amount of N2O produced at a concentration of less than 11 ppm in the entire temperature window indicates that the catalysts have good N<sup>2</sup> selectivity (Figure 2c). NO<sup>x</sup> can be reduced to N2O or N<sup>2</sup> by NH3. Normally, 5–10 ppm of N2O production for the state-of-the-art Cu-based catalysts is usually observed in the literature [2,3]. After Na poisoning (Figure 2b), the three samples show completely different NH3-SCR reactivities, whose order is: 2.3-NaCu > 0.8-NaCu > 0.4-NaCu. The activity of 0.4-NaCu decreases most significantly, and the NO<sup>x</sup> conversion drops sharply from 98% to 30% at ~300 ◦C. Figure 2d shows the N2O generation curve with temperature ramping. Surprisingly, the maximum amount of N2O produced by 0.4-NaCu (~75 ppm) at 280 ◦C is 3 times that of 0.8-NaCu (~25 ppm) and 7 times that of 2.3-NaCu (~10 ppm). The results show that the geometric size of the molecular sieve greatly affects the NH3-SCR catalytic activity and N<sup>2</sup> selectivity of the Na-poisoned CuSSZ-13 catalysts. In short, the Cu/SSZ-13 catalyst with a larger crystal size has better Na resistance.

**Figure 2.** (**a**,**b**) NO<sup>x</sup> conversion and (**c**,**d**) N2O formation of Cu/SSZ-13 before and after Na poisoning. The gas feed contains 500 ppm NOx, 500 ppm NH<sup>3</sup> , 10% O<sup>2</sup> , 3% H2O, balanced N<sup>2</sup> . The gas hourly space velocity (GHSV) is 72,000 h−<sup>1</sup> .

As a side reaction of NH3-SCR, the NH<sup>3</sup> oxidation reaction was also tested (Figure 3). Before Na poisoning, the NH<sup>3</sup> oxidation performances of 0.4-Cu, 0.8-Cu and 2.3-Cu are almost the same. Temperature-dependent NO<sup>x</sup> and N2O evolutions are recorded as shown in Figure S1. Same trends for all nitrogen oxides are observed. After Na poisoning, the NH<sup>3</sup> oxidation performance of all samples is improved. The active center of NH<sup>3</sup> oxidation can be isolated Cu ions and CuO<sup>x</sup> clusters. In the previous report [36], NH<sup>3</sup> oxidation activities on CuO<sup>x</sup> clusters are much higher than Cu ions. Therefore, the improvement of NH<sup>3</sup> oxidation is attributed to CuO<sup>x</sup> formation in the catalysts. It is noted that 0.4-NaCu has the largest increase in activity, reaching ~100% conversion at 250 ◦C. In other words, Cu/SSZ-13 with a larger particle size has relatively low ammonia oxidation activity and higher resistance to Na poisoning. This is consistent with the results of NH3-SCR activity. More importantly, Figure S1 shows that there are two active centers in the oxidation process of NH<sup>3</sup> with temperature ramping. One active center is responsible for the formation of nitrogen oxides at 200–350 ◦C, and the other is responsible for above 350 ◦C. This trend of change is likely to be related to the migration of Cu with increasing temperature. As the crystal size increases, the former active center (might be CuII(NH3)n(H2O)<sup>m</sup> [37]) gradually decreases. 2.3-NaCu can hardly see the NO<sup>x</sup> volcanic curve around 300 ◦C. This observation will be further discussed later.

**Figure 3.** NH<sup>3</sup> oxidation activity of Cu/SSZ-13 (**a**) before and (**b**) after Na poisoning. The gas feed contains 500 ppm NH<sup>3</sup> , 10% O<sup>2</sup> and balanced N<sup>2</sup> . The gas hourly space velocity (GHSV) is 72,000 h−<sup>1</sup> .

Combined with the results of NH3-SCR activities, it is interesting to find that Na poisoned Cu/SSZ-13 with a smaller crystal size has a more serious decline in SCR activity and N<sup>2</sup> selectivity. Such reaction tread cannot be separable from the structure of the catalysts caused by different crystal growth paths. Therefore, the characterization of the texture properties and the active center were conducted.

#### *2.2. Texture Properties*

The crystal structure was characterized by X-ray diffraction experiments. All catalysts show uniform CHA-type X-ray diffraction patterns (9.7◦ , 13.1◦ , 16.3◦ , 18.0◦ , 20.9◦ , 25.4◦ , 26.3◦ , 31.1◦ ), as shown in Figure S2. No characteristic peaks corresponding to CuO (35.6, 38.8◦ ) or Na2O (36.2, 46.1◦ ) are observed, which suggests ICP (Table S1) determined ~1.4 wt % Cu and ~2 wt % Na (if Na poisoned) are well dispersed and the particle size of them are under the detection limit. Our previous work reported poisoned Na can induce desiliconization and form "H2Si2O5" crystal phase (21.8◦ ) [38]. As shown in Figure 4, it shows that the larger the crystal size of the molecular sieve is, the easier it is to desiliconize. However, the structural desiliconization occurs on the H/SSZ-13 but not Cu/SSZ-13, which shows that Cu ions play a role in protecting the Si framework. The nature of SSZ-13 determines the acid sites (Si-OH-Al) formation in the zeolites. Na poisoned samples presented the "H2Si2O5" crystal phase (21.8◦ ), which indicates desiliconization occurs. When Cu was loaded, such desiliconization was much weakened. The results show that

desiliconization is likely to happen on the acid sites. Si-O(CuIIOH)-Al or Al-O-CuII-O-Si-O-Al sites can be kept after Na poisoning.

**Figure 4.** 20–23◦ XRD patterns of Na-poisoned (**a**) H/SSZ-13 supports and (**b**) Cu/SSZ-13 catalysts.

The N<sup>2</sup> adsorption and desorption experiments are used to characterize the pore structure of the catalysts. As shown in Table 1, the BET specific surface area of both SSZ-13 and CuSSZ-13 is greater than 800 m2/g. However, the support SSZ-13 is easily damaged by Na poisoning, and the specific surface area is greatly reduced. This is consistent with the XRD results. The desiliconization is believed to cause such variation on the specific surface area. In contrast, the tolerance of Cu/SSZ-13 to Na is much improved. The pore distribution was also analyzed and found that the pore structure is rarely damaged by Na poisoning (Figure S3).


**Table 1.** BET Specific surface area of samples.

The framework coordination structure of the catalyst was also characterized by NMR technology. Normalized <sup>27</sup>Al and <sup>29</sup>Si NMR spectra show that the coordination of Si and Al has little change before and after Na poisoning, independent of the crystal size of Cu/SSZ-13 (Figure S4). All samples present framework tetrahedral Al at 60 ppm. Corresponding feature of Si at −109, −103, and −99 ppm are attributed to Si(4Si, 0Al), Si(3Si, 1Al), and Si(2Si, 2Al), respectively.

The results of structural characterizations (XRD, BET, NMR) consistently indicate that even though Na poisoning may destroy the structure of the SSZ-13 supports, the loading of Cu greatly improves the tolerance to Na poisoning. The texture properties of Cu/SSZ-13 with different crystal sizes have little variation between each other.

#### *2.3. Cu Distribution*

Figure 5 presents hydrogen temperature-programmed reduction (H2-TPR) profiles of CuSSZ-13 catalysts with different crystal sizes before and after Na poisoning. According to previous reports, it is generally believed that the H<sup>2</sup> reduction peak at 200 ◦C and 400 ◦C are attributed to the reduction of the eight-membered ring (8MR) Cu2+ ions and six-membered ring (8MR) Cu2+ ions to Cu<sup>+</sup> , respectively. The reduction peak above 500 ◦C is the reduction of Cu<sup>+</sup> to Cu<sup>0</sup> [12,39]. As shown in Figure 5a, an H<sup>2</sup> reduction peak

dominates at ~181 ◦C, while the one at ~400 ◦C is not significant. For Cu/SSZ-13 with Si/Al of ~25, Cu2+ is mostly in the form of Z[CuIIOH] (Z represents the negatively charged framework site), rather than Z2CuII, because the probability of having two Al atoms in a six-membered ring (6MR) at the same time is relatively small. <sup>29</sup>Si NMR results also show that Si (3Si, 1Al) species dominate the framework structure (Figure S4). However, an unexpected result is that the larger the crystal size, the fewer Cu species can be reduced. This is in contradiction with the result that the total Cu content of 0.4-Cu, 0.8-Cu, and 2.3-Cu detected by ICP is 1.05 wt %, 1.38 wt %, and 1.44 wt %, respectively. Note that UV–vis characterization (Figure 6) confirms the ICP results, in which the charge transfer of O2- to Cu2+ at 200 nm bands follows an order: 0.4-Cu < 0.8-Cu < 2.3-Cu. Why does the amount of reducible Cu decrease with increasing crystal size? What needs to be certain is that the kinetic radius of H<sup>2</sup> is small enough to pass through the molecular sieve and reach the Cu ion surface. Therefore, it is reasonable to believe that more stable Cu ions in the larger-sized Cu/SSZ-13 make them less reducible. Meanwhile, with the increasing crystal sizes, the shifting to a higher reduction temperature of Cu<sup>+</sup> to Cu<sup>0</sup> is observed. It also indicated that the interaction between Cu ions and supports becomes stronger for the Cu/SSZ-13 with a larger crystal size. After Na poisoning, the reduction peaks shift to lower temperatures, which was previously observed in the literature [13,40]. The peak at 150 ◦C is attributed to the reduction of Z[CuIIOH] to Cu<sup>+</sup> , and the sharp one at 220 ◦C is attributed to the reduction of CuO to Cu<sup>0</sup> . Here we classify the reducing species at ~220 ◦C as CuO, because UV–vis characterizes the formation of a large amount of CuO shown in Figure 6. The amount of produced CuO is proportional to the increase in NH<sup>3</sup> oxidation reaction activity. Besides, the amount of reducible Cu of different samples is still the same as that of fresh samples. The reason why the increase in the particle size leads to the stronger interaction between Cu and the supports is still unclear.

**Figure 5.** H<sup>2</sup> -TPR profiles of Cu/SSZ-13 with different crystal sizes (**a**) before and (**b**) after Na poisoning.

#### *2.4. Acidic Distribution*

In the beginning, the target of designing the Cu/SSZ-13 with different crystal sizes is to tune the surface acid sites. The spatial acidic distribution of Cu/SSZ-13 was revealed by comparing the surface acid sites and bulky acid sites. Figure S5 shows the ammonia temperature-programmed desorption (NH3-TPD) profiles. NH<sup>3</sup> molecules are small enough to penetrate the SSZ-13 zeolites and therefore can be used to characterize the bulky acid sites. The results show that Cu/SSZ-13 catalysts with different crystal sizes own a similar amount of bulky acid sites. Even Na-poisoned samples have a similar total acid amount, which is mainly dominated by weakly adsorbed acids.

**Figure 6.** UV–vis spectra of the Cu/SSZ-13 with different crystal sizes.

Diethylamine is a probe molecule often used to investigate the surface acidity of microporous molecular sieves. Its kinetic diameter (4.5 Å) is larger than the pore size of the SSZ-13 molecular sieve (3.8 Å), which ensures that it can only bind to the acidic sites on the outer surface of the crystal. As shown in Figure 7a, only 0.4-Cu sample can adsorb diethylamine molecules. The results of diethylamine TPD for H/SSZ-13 catalysts in Figure 7c show that the smaller the crystal size, the more surface acid sites. It can be inferred that Cu is more present on the surface with a small crystal size, and as the crystal size increases, Cu is distributed in the subsurface or core, i.e., little diethylamine adsorption on the surface of 0.8-Na and 2.3-Na. For the Na-poisoned samples, two desorption peaks of diethylamine can be observed at ~200 ◦C and 300 ◦C in Figure 7b,d. Comparing the results of H/SSZ-13 and NaH/SSZ-13, it can be found that partial Na ions can substitute Brønsted acid sites and adsorb diethylamine on the surface of the molecular sieve. It is reasonable that there is almost no diethylamine adsorbing on the 2.3-NaH, because its surface acid sites are limited. Besides, with the decrease of the crystal size and the more acid sites on the surface, replaced Na ions remains on the outer surface. The acidic characteristics of the outer surface of Na-poisoned Cu/SSZ-13 are also in line with expectations. The Na substitution of Cu and the formation of CuO clusters are the basic characteristic of CuSSZ-13 alkali metal poisoning [25]. The newly generated acid sites on the outer surface of 0.8-Na and 2.3-Na are attributed to the formation of CuO clusters, which is consistent with the trends of CuO determined by UV–vis and ammonia oxidation activity.

The acidity of the outer surface of the catalyst was also quantitatively tested by pyridine infrared technology. Pyridine is a molecule with a larger kinetic radius of 5.7 Å, which can only interact with the acid sites on the outer surface of Cu/SSZ-13. According to previous studies [41–43], The IR bands at 1450 and 1593 cm−<sup>1</sup> are attributed to the chemisorbed pyridine on the Lewis acid sites of the zeolites. The IR band at 1483 cm−<sup>1</sup> is assigned to the pyridine bonded on both Lewis and Brønsted acid sites. The IR band at 1630 cm−<sup>1</sup> is attributed to the Brønsted acid sites. As shown in Figure 8, the results show that the smaller the crystal size is, the more Brønsted acid and Lewis acid are on the surface. Although there is a certain deviation on surface quantification from the diethylamine-TPD, the trend is highly consistent.

**Figure 7.** Diethylamine-TPD profiles of Cu/SSZ-13 (**a**,**b**) and H/SSZ-13 (**c**,**d**) before and after Na poisoning.

**Figure 8.** Pyridine-chemisorbed IR spectra of (a) H/SSZ-13 and (b) Cu/SSZ-13 with different crystal sizes before Na poisoning.

In addition to chemical adsorption methods, we expect to visually investigate the spatial distribution of Cu ions on SSZ-13. Combined with cross-section polishing technology, the Cu/SSZ-13 is cut and the Cu content is analyzed by EDS. As shown in Figure 9, point EDS analysis was conducted from the center to the edge of the Cu/SSZ-13 cross-section for four individual crystals. The detected Cu content is summarized in Table 2. The energy spectra are attached to the supporting information (Figure S6). The results show that the distribution of Cu in the molecular sieve forms a decreasing gradient from the center to the edge. Note that it is hard to detect Cu on the surface and subsurface. Such a feature provides sufficient outer surface space to buffer the corrosion of Na, thereby protecting the Cu ions in the core.

**Figure 9.** Point EDS analysis of 2.3-Cu sample.



It is time to recall the changes in NH<sup>3</sup> oxidation performance of Cu/SSZ-13 with different crystal sizes before and after Na poisoning. According to our analysis, the side reaction of NH<sup>3</sup> oxidation of Na-poisoned Cu/SSZ-13 with larger crystal size is not significantly improved (Figure 3), and the number of active centers around 300 ◦C decreases with the increase of crystal sizes (Figure S1). This is rationalized by the difference in spatial acidity distribution. On the one hand, the smaller the crystal size, the more acidic the surface of Cu/SSZ-13 is, and the proportion of Cu ions on the surface is greater. This results in the surface Cu ions being susceptible to the Na corrosion to generate CuO species. On the other hand, the Cu ions distributed in the large crystal-sized molecular sieve have extremely strong stability. The interaction between Cu and framework O can be characterized by H2-TPR. Because the interaction of Cu and O reflects how difficult the Cu2+ can be reduced (or O2<sup>−</sup> can be split). From the H2-TPR results, with increasing crystal sizes more Cu interacts with the framework O so strongly that it cannot be reduced by H2. The chemical bond between the core Cu ions and framework O might be strong enough that NH<sup>3</sup> or H2O cannot solvate Cu ions, which explains why the CuII(NH3)n(H2O)<sup>m</sup> species are less distributed in the large-sized Cu/SSZ-13. This inference is based on the fact that the active center of NH<sup>3</sup> oxidation will change with increasing temperature. Chemically, isolated Cu (II) in the six-member ring of SSZ-13 is the active center. It can be solvated by H2O and NH<sup>3</sup> molecules to form so-called hydrated or ammoniated Cu (II) species (CuII(NH3)n(H2O)m). Gao et al. reported that the activation energy of Cu/SSZ-13 in the low-temperature region (200–260 ◦C) and the high-temperature region (400–460 ◦C) of the NH<sup>3</sup> oxidation reaction are 64.1 kJ/mol and 150 kJ/mol, respectively [39]. Therefore, it is reasonable to believe that the reaction path is different in the two different temperature ranges, and the active center transforms from solvable CuII(NH3)n(H2O)<sup>m</sup> to framework-anchored ZCuIIOH as the temperature crosses ~300 ◦C.

#### **3. Materials and Methods**

#### *3.1. Catalysts Preparation*

Na/SSZ-13 (Si/Al = 25) was home-made according to previous reports [2,44,45]. The crystal size of SSZ-13 was controlled by adding different amounts of seed crystals [46]. During the hydrothermal synthesis process, other conditions remain the same, such as crystallization temperature (160 ◦C), crystallization time (72 h), silicon source (silica sol, Jiyida Co. Ltd., Qingdao, China), aluminum source (pseudo-boehmite, Chinalco, Zibo, China), template agent (1-Adamantanamine, Sigma-Aldrich, Beijing, China), etc. The templating agent was removed from as-prepared Na/SSZ-13 by calcinating at 650 ◦C for 4 h. Cu/SSZ-13 was obtained by the aqueous ion-exchange method. Briefly, following Na/SSZ-13 with the template removed, NH4/SSZ-13 was obtained by twice ion-exchanging with 0.1M NH4NO3. Then NH4/SSZ-13 was ion-exchanged by 0.1M Cu(NO3)<sup>2</sup> to prepare

Cu/SSZ-13. H/SSZ-13 was also prepared by calcinating NH4/SSZ-13 at 550 ◦C for 4 h. The samples were denoted by 'x-Cu' and 'x-H' to respectively represent Cu/SSZ-13 catalysts and H/SSZ-13 supports with different crystal sizes, where x is the crystal size (µm).

To simulate the alkali metal poisoning process, a combination of equal volume impregnation and high-temperature hydrothermal aging was carried out. In detail, it was impregnated with NaNO<sup>3</sup> on the samples and aged for 12 h at 600 ◦C under 10 vol % steam. 'x-NaCu' and 'x-NaH' were used to represent Na-poisoned samples.

#### *3.2. Characterization*

The morphology of the sample was pictured on a field emission electron microscopy (Regulus 8100, HITACHI, Tokyo, Japan) at 3 kV.

The powder X-ray diffraction (XRD) patterns of the catalysts were detected using a Rigaku Smartlab XRD (Tokyo, Japan) with Cu Kα radiation source. The X-ray emission tube was run at 40 kV and 40 mA. The diffraction angle (2 θ) range of 5–50◦ was chosen to identify the crystal phases.

The BET surface area was measured with a physisorption analyzer (ASAP 2460, Micromeritics) at 77K. Before testing, the samples were vacuumed under 300 ◦C for 3 h.

The NMR spectra were recorded using a JEOL JNM-ECZ600R spectrometer (Tokyo, Japan). The <sup>29</sup>Si and <sup>27</sup>Al NMR were carried out at a field strength of 14.1 T with a total scanning of 1200 and 300 times, relaxation delay of 10s and 2s, respectively. The tube diameter of 4 mm and 8 mm was chosen for testing <sup>27</sup>Al and <sup>29</sup>Si, respectively.

Hydrogen temperature-programmed reduction (H2-TPR) was carried out in a Micromeritics AutoChem 2920 II system (Micromeritics). The catalysts were pretreated under 5% O2/N<sup>2</sup> at 500 ◦C for 30 min. The H2-TPR profile was recorded from ambient to 900 ◦C at a rate of 10 ◦C/min.

UV–vis spectra were collected in a SHIMADZU UV-2600 (Kyoto, Japan) equipped with an integrating sphere assembly. The sample powder was pressed into a cake in the button groove at ambient. A pressed cake of BaSO<sup>4</sup> was used as the reference.

Diethylamine temperature-programmed desorption measurement was conducted using a plug flow microreactor. The diethylamine was detected using an online Fourier transmission infrared spectrometer (MultiGas 6030, MKS). The sample was pretreated under 5% O2/N<sup>2</sup> at 500 ◦C for 30 min, followed by diethylamine saturation at 100 ◦C. The weakly adsorbed diethylamine was purged by N<sup>2</sup> and then the sample was heated to 550 ◦C at a rate of 10 ◦C/min.

Operando pyridine titration experiment was monitored by a diffuse reflection infrared Fourier transform spectrometer (DRIFTS) (Nicolet 6700, Thermo). The sample was pretreated at 500 ◦C for 30 min under 5% O2/N2. Then it was cooled to 250 ◦C under N<sup>2</sup> and the background spectrum was collected. The in-situ time-resolved spectra were recorded when the N<sup>2</sup> carrier with pyridine mixed gas pass through the sample.

## *3.3. Catalytic Evaluation*

The standard NH3-SCR activity was tested with a plug flow microreactor. The powder sample was supported by quartz wool on both sides. Typically, 0.1 g catalyst was mixed with 0.9 g quartz sand to uniformly disperse catalysts powder. The simulated gas contains 500 ppm NH3, 500 ppm NO, 10% O2, 3% H2O and balanced N2. The gas hourly space velocity (GHSV) is 72,000 h−<sup>1</sup> . The NO<sup>x</sup> conversion was calculated as below,

$$\mathrm{NO\_{x}\%} = \frac{[\mathrm{NO\_{x}}]\_{\mathrm{in}} - [\mathrm{NO\_{x}}]\_{\mathrm{out}}}{[\mathrm{NO\_{x}}]\_{\mathrm{in}}} \times 100\% \tag{1}$$

The NH<sup>3</sup> oxidation activity was also investigated individually. The experiment setup is the same as that for the NH3-SCR activity measurement. 500 ppm NH3, 10% O<sup>2</sup> and balanced N<sup>2</sup> were used. The NH<sup>3</sup> conversion was calculated as below,

$$\text{NH}\_3\text{ }\%= \frac{[\text{NH}\_3]\_{\text{in}} - [\text{NH}\_3]\_{\text{out}}}{[\text{NH}\_3]\_{\text{in}}} \times 100\% \tag{2}$$

The reagents and products were monitored by an online FTIR spectrometer (Multigas 6030, MKS). For each sample, the activity test included pre-treatment and steady-state activity testing. For example, the catalysts were firstly oxidized under 10% O2/N<sup>2</sup> at 500 ◦C for 1 h. The ready catalyst was then fed with mixed gases of standard NH3-SCR or NH<sup>3</sup> oxidation. The steady-state data were collected from 500 ◦C to 100 ◦C in an interval of 50 ◦C.

#### **4. Conclusions**

Cu/SSZ-13 catalysts with similar Cu loadings and different crystal sizes (0.4–2.3 µm) were controllably synthesized. Although the pore structure of H/SSZ-13 with a large crystal size is susceptible to Na poisoning, the loading of Cu ions has a strong protective effect on the structure. It was found that increasing the crystal size of Cu/SSZ-13 catalysts can effectively improve the Na resistance. Large crystal size is conducive to the distribution of acidic sites on the subsurface or inner core of the molecular sieve. The Cu ions distributed in the deep layer have strong redox stability and are not easily solvated by NH<sup>3</sup> or H2O molecules. The richer Cu ions on the outer surface of Cu/SSZ-13 with smaller particle size is more susceptible to Na ion exchange to generate more CuO species. The decrease of Cu ions and the increase of CuO clusters are the main reasons for the decrease of NH3-SCR activity and the increase of side reaction NH<sup>3</sup> oxidation activity. The results are helpful to guide industrial applications in heavy-duty diesel engines after treatment by improving the alkali metal tolerance of commercial Cu/SSZ-13 catalysts for NH3-SCR reaction.

**Supplementary Materials:** The following are available online at https://www.mdpi.com/article/ 10.3390/catal11080979/s1, Figure S1: NO<sup>x</sup> and N2O concentration evolution in the NH<sup>3</sup> oxidation; Figure S2. XRD patterns of Cu/SSZ-13 (a) before and (b) after Na poisoning; Figure S3. The micropore distribution of Cu/SSZ-13 (a) before and (b) after Na poisoning; Figure S4. (a–b) <sup>27</sup>Al NMR spectra and (c–d) <sup>29</sup>Si NMR spectra of CuSSZ-13 before and after Na poisoning; Figure S5. NH<sup>3</sup> -TPD profiles of Cu/SSZ-13 with different crystal sizes (a) before and (b) after Na poisoning; Figure S6. Point EDS spectra corresponding to the results in Figure 9, Table S1. Element composition of Cu/SSZ-13 and Na-poisoned counterparts with different crystal sizes.

**Author Contributions:** Conceptualization, Z.C. and M.S.; Methodology, C.W.; Validation, Z.C., J.W. (Jianqiang Wang), and J.W. (Jun Wang); Formal analysis, Z.C.; Investigation, Z.C.; Writing—original draft preparation, Z.C.; Writing—review and editing, J.W. (Jianqiang Wang) and C.W.; Supervision, M.S. and G.S.; Project administration, J.W. (Jun Wang) and G.S.; Funding acquisition, J.W. (Jun Wang). All authors have read and agreed to the published version of the manuscript.

**Funding:** This research was funded by Foundation for Innovative Research Groups of the National Natural Science Foundation of China, grant number 51921004; Major Science and Technology Programs of Yunnan, grant number 202002AB080001-1; National Natural Science Foundation for Youth of China, grant number 21908207 and Postdoctoral Research Foundation of China, grant number 2020M670659; Shanxi Province Science Foundation for Youths, grant number 201901D211224.

**Acknowledgments:** We are grateful to all our funders.

**Conflicts of Interest:** The authors declare no conflict of interest.

#### **References**


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