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Batteries 2022, 8, 108 4 of 16 FiFgiugruere1.1.SEMmicrograph((a)),,XRDppaatttetrenrn(b()b,)R,aRmamanasnpespctercutmru(mc),(Nc),2 aNdsoardpstoiorpn–tidoens–odrpestiornpitsion- 2 istohtehremrm(d()da)nadndpoproeresizsiezdeidstirsitbriubtuiotino(ne)(eo)fotfhtehheahrdarcdacrbaorbnounsuedseidnitnhitshsistusdtuyd.y. Theconductivitiesoftheelectrolyte(1moldm−3NaClO in1:1EC/DEC)arecalcu- The conductivities of the electrolyte (1 mol dm−3 NaClO4 in 1:1 EC/DEC) are calcu- laltaetdedbbyy[3[13]1:]: κ = L/RA (1) 𝜅 𝐿⁄𝑅𝐴 (1) where κ is conductivity, L is distance between electrodes, A is electrode area and R is resis- where κ is conductivity, L is distance between electrodes, A is electrode area and R is re- tance. As the working and counter electrodes are in a fixed position, L/A is constant and sistance. As the working and counter electrodes are in a fixed position, L/A is constant and can be obtained by testing standard KCl solutions (Figure S1). For this experimental setup, can be obtained by testing standard KCl solutions (Figure S1). For this experimental setup, L/A was calculated to be 317 m−1. The measured electrolyte conductivities are displayed in Figure 2 and increase with temperature as expected [32]. The conductivity at 80 ◦C is approximately three times that at 10 ◦C (Table S1) linked to increasing Na+/ClO4− dissoci- ation and decreasing electrolyte viscosity [33]. Holding electrolytes around 20 ◦C overnight results in some colourless crystals being precipitated, possibly due to EC precipitation (Figure S2). That could result in lower electrolyte conductivity at a lower temperature than that shown in Figure 2.PDF Image | Temperature Dependence of Hard Carbon Sodium Half-Cells
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