Viscosity

4.2 T HERMOPHYSICAL PROPERTIES

4.2.2 Viscosity

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0 5 10 15 20 25 30

1.05 1.10 1.15 1.20 1.25 1.30

 (g.cm-3 )

Pressure (bar)

[C₂CN Bim]Br [C₂CN Hm]Br [C₂CN Oim]Br [C₂CN Bim]Cl [C₂CN Him]Cl [C₂CN Oim]Cl [C₂CN Bim]DOSS [C₂CN Him]DOSS [C₂CN Oim]DOSS [C₂CN Dim]DOSS [C₂CN Bim]DDS [C₂CN Him]DDS [C₂CN Oim]DDS [C₂CN Dim]DDS [C₂CN Him]SBA [C₂CN Oim]SBA [C₂CN Dim]SBA

Fig 4-48 Effect of pressure on the densities of [C2CN Cnim]Br, [C2CN Cnim]Cl, [C₂CN C_nim]DOSS, [C₂CN C_nim]DDS and [C₂CN C_nim]SBA ILs at 298.15 K

0 5 10 15 20 25 30

0.9 1.0 1.1 1.2 1.3 1.4

 (g.cm-3 )

Pressure (bar)

[C₂CN Bim]BS [C₂CN Him]BS [C₂CN Oim]BS [C₂CN Bim]TFMS [C₂CN Him]TFMS [C₂CN Oim]TFMS [C₂CN Ayim]DOSS [C₂CN Bzim]DOSS [C₂CN Heim]DOSS [P_8,8,8,14]Cl [P_8,8,8C₆P_8,8,8]Cl₂ [P_8,8,8C₁₀P_8,8,8]Cl₂ [P_6,6,6,14]DOSS [P_8,8,8,14]DOSS [P_8,8,8C₆P_8,8,8]DOSS₂ [P_8,8,8C₁₀P_8,8,8]DOSSl₂

Fig 4-49 Effect of pressure on the densities of [C2CN Cnim]BS, [C2CN Cnim]TFMS, [C2CN Ayim]DOSS,[C2CN Bzim]DOSS,[C2CN Heim]DOSS,[P6,6,6,14]DOSS [P_8,8,8,14]X and [P_8,8,8C_nP_8,8,8]X₂ ILs at 298.15 K.

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appears in many dimensionless groups used in mass- and heat-transfer correlations.

The applications that occur at high temperatures and/or pressures require reliable and accurate experimental data and mathematical models. This is especially pertinent for engineering applications as hydraulic fluids. ILs cover a wide range of viscosity [108].

The experimental viscosity values of the synthesized ILs are shown in Table A-15 to Table A-24 in Appendix A. High viscosity is a characteristic of most ILs. However the high thermal stability exhibited by ILs allows for applications at higher temperatures where the viscosity is reduced. Previous studies showed that the viscosity of ILs is largely controlled by hydrogen bonding, van der Waals forces, molecular weight and mobility [24]. The high viscosity for various ILs compared to molecular solvents was attributed to enhanced van der Waals forces relative to the hydrogen bonding [191].

The influence of anion on viscosity for the studied ILs is shown in Fig 4-51 to Fig 4-54. The measured viscosities are higher for the IL with DOSS anion among the sulfonate based anions, while it was the lowest for IL with TFMS anion. The ILs [C₂CN C_nim]TFMS shows the lowest viscosity of the [C₂CN C_nim]-based ILs investigated in this work. This can be explained by the incapability of the TFMS- anion to interact by hydrogen bonding and a randomized aggregation of ions caused by a low anionic basicity. More basic anions lead to tighter ion pairing of the cation with the anion, which also increases the intermolecular forces like hydrogen bonding [119]. Sulfonate groups can attract positively charged species to reduce the average transport of cations. The basicity of the anions incorporating sulfonate group varied depending on the alkyl chains and functional groups attached to the anion. As shown in Fig 4-50, The TFMS anion incorporate with withdrawing group (CF3) which result in decreasing the negative charge of the SO3-

group and hence decrease the basicity.

The DOSS anion incorporates with donating groups (alkyl chains) which increase the negative charge of the SO3-

group and hence increase the basicity. Moreover, the DOSS anions incorporates two alkyl chains while DDS incorporates one alkyl chain which results in higher basicity of the SO3-

group for DOSS anion compared to that for DDS anion [203].

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Fig 4-50 Structures of DOSS, DDS, SBA, BS and TFMS anions

290 300 310 320 330 340 350 360

0 5000 10000 15000 20000

 (mPa.s)

T/K

[C₂CN Bim]Cl [C₂CN Bim]Br [C₂CN Bim]DOSS [C₂CN Bim]DDS [C₂CN Bim]BS [C₂CN Bim]TFMS

Fig 4-51 Viscosities as a function of temperature for [C2CN Bim]X

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290 300 310 320 330 340 350 360

0 2000 4000 6000 8000 10000 12000 14000 16000 18000 20000

 (mPa.s)

T/K

[C₂CN Him]Cl [C₂CN Him]Br [C₂CN Him]DOSS [C₂CN Him]DDS [C₂CN Him]SBA [C₂CN Him]BS [C₂CN Him]TFMS

Fig 4-52 Viscosities as a function of temperature for [C2CN Him]X

290 300 310 320 330 340 350 360

0 5000 10000 15000 20000

 (mPa.s)

T/K

[C₂CN Oim]Cl [C2CN Oim]Br [C₂CN Oim]DOSS [C2CN Oim]DDS [C₂CN Oim]SBA [C2CN Oim]BS [C₂CN Oim]TFMS

Fig 4-53 Viscosities as a function of temperature for [C2CN Oim]X

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290 300 310 320 330 340 350 360

0 2000 4000 6000 8000 10000 12000 14000 16000 18000 20000

 (mPa.s)

T/K

[C2CN Dim]Br [C₂CN Dim]DOSS [C2CN Dim]DDS [C₂CN Dim]SBA

Fig 4-54 Viscosities as a function of temperature for [C₂CN Dim]X

The increased volumes of the anions here (trifluoromethanesulfonate excepted) lead to higher viscosities through reductions in ion mobility [67]. In addition, the high viscosity can also be ascribed to increased electrostatic interactions between the cation and anion. The [C2CN Dim]DOSS IL showed highest viscosity since it possesses the largest anions with a values while [C2CN Bim]TFMS showed lowest viscosity.

The viscosity values of the synthesized imidazolium-based ILs are higher than those of the corresponding ILs without nitrile group, which could be due to the high electron mobility around the nitrile group [106].

The viscosity values increase as the alkyl chains increases as observed by Tokuda et al. [111]. Even though the viscosities are high, the effect of shear rate on viscosities was investigated. ILs is classified as either Newtonian fluid or a thixotropic fluid. For the present ILs the shear rate has no difference in the viscosity but longer alkyl chains, (e.g., [CnMim]BF4 where n  12) show non-Newtonian behavior [92]. The present ILs are classified as Newtonian fluid since n = 4, 6, 8, 10 (where n is the number of carbon atoms).

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The viscosities of these nitrile-functionalized ILs with sulfonate anions are much higher compared with the reported imidazolium-based nitrile-functionalized ILs. For [C₂CN MIm]BF₄, [C₃CN Mim]BF₄ and [C₄CN Mim]Cl the viscosities are 65.5, 352 and 5222 mPa.s respectively [41, 106]. Moreover, the viscosities of the present synthesized ILs are higher compared to the other pyridinium-based nitrile- functionalized ILs (for [C1CnCNPyr]NTf2 (n=1, 2, 3, 5 where n is the number of carbon atoms) the viscosities are in the range (345 to 540) cP) as reported by Nockeman and coworkers [201]. The imidazolium cations and sulfonate anions are joined together by a hydrogen bonding network [65] which resulted in increased viscosity. Low anion weight and low basicity (for less basic anion, the van der Waals forces dominates over the H-bonding due to better charge delocalization and this will reduce the viscosity of the IL) are necessary to obtain IL with low viscosity [191].

The viscosity increases with increasing molecular weight or alkyl chain [113] as shown in Fig 4-55. The high viscosities of the [P6,6,6,14]DOSS and [P8,8,8,14]DOSS ILs when compared to [P6,6, 6,14]NTf2 and [P6,6,6,14]OTf is due to the long alkyl chain of the DOSS anion. It is accomplished by increasing the electrostatic interaction between the cation and anion. Further the higher viscosity of the present phosphonium-based ILs when compared to [P_{2,2,2 ,8}]NTf₂ and [P_2,2,2,2]NTf₂ is attribute to the increased Van der Waals interactions of the long alkyl chains from both the phosphonium cations and the DOSS anion. The large volume of the DOSS anion causes low ion mobility and hence low viscosity [67].

Increasing the alkyl chain length has two contradictory effects: increase the electron donation into the cationic centre which decreases the electrostatic interaction between the cation and anion and hence viscosity is reduced. However increases the alkyl chain length also causes the Van der Waal‘s interactions to increase and viscosity to increase.

The viscosity values of the present DCILs are much higher and is comparable to phosphonium-based monocationic ILs (Fig 4-55); the viscosities of [P6,6,6,14]NTf2], [P8,8,8,,8]NTf2 and [P8,8,8,8] dithiomalenitrile is 450, 418 and 5590 mPa.s respectively [114].The viscosity values increases asthe spacer alkyl chain length increases and the

116

result is in agreement with that observed by Tokuda et al.[111]. The high viscosity of the DCILs was attributed to an increase in van der Waals forces, hydrogen bonding between cationic protons and anionic halides and the symmetry of the cations and anions [92].

290 300 310 320 330 340 350 360

0 5000 10000 15000 20000

 (mPa.s)

T/K

[C₂CN Bim]DOSS [C₂CN Him]DOSS [C₂CN Oim]DOSS [C₂CN Dim]DOSS [C₂CN Ayim]DOSS [C₂CN BZim]DOSS [C₂CN Heim]DOSS [P_6,6,6,14]DOSS [P_8,8,8,14]DOSS [P_8,8,8C₆P_8,8,8]DOSS₂ [P_8,8,8C₁₀P_8,8,8]DOSS₂

Fig 4-55 Viscosities for the DOSS-based ILs as a function of temperature

The influence of temperature on viscosity for the studied ILs is shown in Fig 4-51 to Fig 4-55. As can be observed, a rise in temperature caused a significant reduction in the viscosities of the synthesized ILs. An increase in temperature diminishes the strength of interactions between the cation and anion and should result in a lower viscosity [191]. These results sugget that slow mass-transfer processes occurr in ILs at room temperatures due to high viscosity of ILs will become accelerated at elevated temperatures.

As can be observed, a rise in temperature caused a significant reduction in the viscosities of the present synthesized ILs. However, as shown in Fig 4-55 and in Table A-15 to Table A-24 in Appendix A, the viscosity values of the ILs show functional group and alkyl chain length dependency [119], and an addition of

117

functional group or increasing alkyl chain length has been found to give higher viscosity value.

Variation of the viscosity with temperature provides information on the structure of the ILs [133]. The temperature dependence of viscosity was studied for all of the synthesized ILs over the temperature range 293.15-353.15 K and the plots (Fig 4-56 to Fig 4-60) were fitted with the logarithmic form of the Arrhenius equation ( 4-4).

RT E_



ln _

ln 4-4

where  is the viscosity,  is the viscosity at infinite temperature, E activation energy for viscous flow, R is universal gas constant and T is temperature in Kelvin.

The activation energies for viscous flow (E_) and the viscosities at infinite temperature (_) were calculated from the slopes and intercepts (respectively) of the Arrhenius plots (Fig 4-56 to Fig 4-60). Table A-25 shows the Arrhenius parameters obtained from the Arrhenius plots together with the standard deviations (SD). The standard deviations were calculated using equation ‎4-2.

0.0028 0.0029 0.0030 0.0031 0.0032 0.0033 0.0034 5

6 7 8 9 10

ln (mPa.s-1 )

1/T(K^-1)

[C2CN Bim]Br C2CN Him]Br C2CN Oim]Br [C₂CN Dim]Br [C2CN Bim]Cl [C2CN Him]Cl [C2CN Oim]Cl

Fig 4-56 Arrhenius plot of viscosity for [C2CN Cnm]Brand [C2CN Cnm]Cl ILs

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0.0028 0.0029 0.0030 0.0031 0.0032 0.0033 0.0034 0.0035 4

5 6 7 8 9 10

ln (mPa.s-1)

1/T(K^-1)

[C₂CN Bim]DOSS C2CN Him]DOSS C₂CN Oim]DOSS [C2CN Dim]DOSS [C₂CN Bim]DDS [C2CN Him]DDS [C₂CN Oim]DDS [C₂CN Dim]DDS

Fig 4-57 Arrhenius plot of viscosity for [C₂CN C_nm]DOSSand [C₂CN C_nm]DDS ILs

0.0028 0.0029 0.0030 0.0031 0.0032 0.0033 0.0034 0.0035 3

4 5 6 7 8 9 10

ln  (mPa.s-1)

1/T(K^-1)

[C₂CN Him]SBA [C₂CN Oim]SBA [C₂CN Dim]SBA [C₂CN Bim]TFMS [C₂CN Him]TFMS [C₂CN Oim]TFMS

Fig 4-58 Arrhenius plot of viscosity for [C2CN Cnm]SBAand [C2CN Cnm]TFMS ILs

0.0028 0.0029 0.0030 0.0031 0.0032 0.0033 0.0034 0.0035 4

5 6 7 8 9 10

ln (mPa.s-1)

1/T(K^-1)

[C₂CN Bim]BS [C₂CN Him]BS [C₂CN Oim]BS [C₂CN Ayim]DOSS [C₂CN Bzim]DOSS [C₂CN Heim]DOSS

Fig 4-59 Arrhenius plot of viscosity for [C2CN Cnm]BSand dual functionalized ILs

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0.0028 0.0029 0.0030 0.0031 0.0032 0.0033 0.0034 0.0035 4.5

5.0 5.5 6.0 6.5 7.0 7.5 8.0 8.5 9.0 9.5 10.0

ln (mPa.s-1 )

1/T(K^-1)

[P_8,8,8,14]Cl [P8,8,8C

6[P

8,8,8]Cl

2

[P_8,8,8C₁₀[P_8,8,8]Cl₂ [P_6,6,6,14]DOSS [P_8,8,8,14]DOSS [P_8,8,8C₆[P_8,8,8]DOSS₂ [P_8,8,8C₁₀[P_8,8,8]DOSS₂

Fig 4-60 Arrhenius plot of viscosity for phosphonium-based ILs

The activation energy for viscous flow (E_) gives an estimation of the level of energy required by the ions to move freely inside the IL. The value of E can be correlated with structural information about the ILs. The larger the value of E, the harder it is for the ions to move freely inside the IL. That might be due to either physical size or more numerous or stronger interactions in the IL (and hence more order) [109]. The viscosity at infinite temperature () is an indication of the magnitude of the constitutive ions structures effect on the viscosity of the ILs [109, 133]. At infinite temperature, interactions which contribute to viscosity at room temperature in ILs are no longer effective and the viscosity (η∞) is governed only by the geometric structure of the ions in the IL. So the value of η∞ is representative of a structural contribution of the ions to the viscosity [109].

The activation energies (E_) are higher for the dual functionalized imidazolium- based ILs while it was the lowest for phosphonium-based ILs. The activation energy is higher for the dual functionalized ILs than for the nitrile functionalized IL, suggesting that for the constitutive ions of the dual functionalized ILs is more difficult to pass each other in comparison with the nitrile functionalized. The energy barrier for the dual functionalized ILs ions, which must be surpassed, could become higher as a result of attaching two functionalized chains to the imidazolium cation. The present ILs showed lower activation energies compared to that for other ILs reported by Sánchez, et al. [133], (the activation energies of [Bmim]BF₄ and [Amim]BF₄ are (33.53 and 49.18)10³ KJ.mol^-1). Furthermore, these ILs except [C2CN Cnim]TFMS

120

show higher activation energies compared to [Bmmim]BF₄, [Bmim]PF₆ and [Bmim]CF₃SO₃ ILs that have activation energies in the range of 21-26.17 KJ.mol^-1 [109].

The viscosities at infinite temperatures (η∞) are higher for the phosphonium-based ILs followed by the nitrile functionalized IL while it was the lowest for the dual functionalized imidazolium-based ILs. These results suggest that the structural contribution of the phosphonium-based ILs ions to the viscosity is greater than the other studied ILs. This might be due to the large number of alkyl chains of the phosphonium-based ILs. It is accomplished by increasing the electrostatic interaction between the cation and anion and also the Van der Waal‘s interactions between the alkyl chains.