ライフサイエンスコーパス: kJ

1 ) s(-1), DeltaH(double dagger) = 8.7 +/- 1.0 kJ mol(-1), DeltaS(double dagger) = -120 +/- 40 J mol(-1

2 lizes alpha-synuclein fibrils by 5.0 +/- 1.0 kJ mol(-1), thus increasing the supersaturation of monom

3 .0 +/- 2.5 kJ/mol, ACO2 IRE-RNA 35.0 +/- 2.0 kJ/mol.

4 s(-1), DeltaH(double dagger) = 17.6 +/- 3.0 kJ mol(-1), DeltaS(double dagger) = -143 +/- 11 J mol(-1

5 N), and calculated heat of formation (-421.0 kJ mol(-1)), combined with its calculated superior deton

6 s C=0.020+/-0.002 min(-1) and Ea,s=155+/-7.0 kJ/mol.

7 eltarG' approaches equilibrium (DeltarG' = 0 kJ/mol), exponentially more enzyme counterproductively c

8 eaction enthalpies amount to -27.10 +/- 0.05 kJ for TA and -29.30 +/- 0.05 kJ for TU.

9 27.10 +/- 0.05 kJ for TA and -29.30 +/- 0.05 kJ for TU.

10 itio energy, and 50% of those to within 0.05 kJ mol(-1).

11 tively, isosteric heat of adsorption = 40.05 kJ mol(-1)).

12 +/- 0.09 M(-1) and DeltaG of -19.2 +/- 0.06 kJ mol(-1) for COX-1.

13 ative DeltaCPdouble dagger) was -1.2 +/- 0.1 kJ mol(-1) K(-1) .

14 donor indole (DeltaH degrees = -7.3 +/- 0.1 kJ/mol, DeltaS degrees = -24 +/- 1 J/(mol.K)).

15 remarkably reduced from 95.7 kJ/mol to 12.1 kJ/mol (A2 model).

16 mately 1.4-fold (from D G H 2 O 21.8 to 16.1 kJ mol(-1) ).

17 netics and the activation energy (Ea = 246.1 kJ.mol(-1)) of the reaction were estimated using the so-

18 1 gN m(-2) d(-1) at an energy demand of 26.1 kJ gN(-1).

19 to detect a between-group difference of 4.1 kJ/kg/d at follow-up.

20 tively, and enthalpy change for K1 was -42.1 kJ.mol(-1).

21 at activation energies of 54.9 (TA) and 66.1 kJ.mol(-1) (TU) for the same temperature range, confirmi

22 nthalpy of adsorption (Deltahads = -73 +/- 1 kJ/mol), with a larger than expected entropic penalty fo

23 re sensitive indicators than vitamin C (82.1 kJ/mol).

24 ltaDeltaG(double dagger)sel, 233 K = 9 +/- 1 kJ/mol).

25 in activation energies Ea(D) - Ea(H) was 9.1 kJ.mol(-1).

26 deviations in the Gibbs free energy (about 1 kJ/mol) are significantly smaller than the "chemical acc

27 ely 38-fold but only altered DeltaGHet by <1 kJ mol(-1).

28 H-bonds were worth less than -1 kJ mol(-1) when the interacting groups were separated by

29 ats of adsorption (Qst) of -34(1) and -12(1) kJ/mol, respectively.

30 fully reversible O2 affinities (Qst = -47(1) kJ/mol at low loadings).

31 an Arrhenius activation energy of 111 +/- 10 kJ/mol, which is lower than that observed for molecular

32 asurement of NHC desorption energy (158+/-10 kJ mol(-1)) and confirmation that the NHC sits upright o

33 the *OH probe used), but a value of about 10 kJ mol(-1) for p-benzoquinone loss, which is consistent

34 eric heat of hydrogen adsorption is above 10 kJ mol(-1).

35 destabilizes the domain by approximately 10 kJ/mol, promoting its unfolding.

36 generated (4.6 +/- 0.4) x 10(9) cm(-3) at 10 kJ/m(3).

37 extraordinary Hall effect, is reduced by 10 kJ/m(3) by tensile strain out-of-plane epsilon(z) = 9 x

38 eltaHf,298K = (325 +/- 8) kJ mol(-1), ca. 10 kJ mol(-1) below the previous value.

39 energy barrier for 15-lipoxygenation was 10 kJ/mol higher than for 12-lipoxygenation.

40 with energy barriers of approximately 10-100 kJ mol(-1) depending on d.

41 ducts, with Ng binding energies of 80 to 100 kJ mol(-1) , contain B-Ng bonds with a substantial degre

42 were 0.0047 and 0.0023 s(-1), and 87 and 104 kJ/mol, respectively.

43 table anti conformer 6anti is DeltaG() = 104 kJ mol(-1) at 298 K.

44 onsistent with a high activation energy, 106 kJ/mol) that increases Mn(II) affinity.

45 formate (HCOObi,ad) plus (H2O-OH)ad was 106 kJ/mol at 3/8 ML and 150 K.

46 The activation energy is 94, 106, and 112 kJ/mol for MNPZ, NDELA, and NHeGly, respectively.

47 nius barriers that are lower for dimers (114 kJ/mol at 750 K) than for monomers (124 kJ/mol).

48 sociated, with the calculated barrier of 116 kJ mol(-1) and the overall energy gain of 72 kJ mol(-1).

49 azobenzene more than doubles from 58 to 120 kJ mol(-1), and the material also maintains robust cycla

50 y consumption of 483 kWh per ton of Cl2 (124 kJ molCl2 (-1) ) which is about 50-55 % of state-of-the-

51 (114 kJ/mol at 750 K) than for monomers (124 kJ/mol).

52 ergy (Ea) requirements ranged from 51 to 125 kJ mol(-1), with wood-derived PyOM having the highest Ea

53 energies in the range of -202 kJ/mol to -127 kJ/mol.

54 teric interaction energy of approximately 13 kJ mol(-1), which is comparable to that of the binding o

55 d the affinity for HIP-CoA (DeltaDeltaG = 13 kJ mol(-1)) is consistent with the loss of three hydroge

56 activation energies of the process span 135 kJ/mol to 226 kJ/mol, and 188 kJ/mol to 268 kJ/mol, for

57 tivation energies were ranged from 51 to 135 kJ mol(-1) for ascorbic acid and from 49 to 99 kJ mol(-1

58 Activation energies ranged from 22 to 136 kJ mol(-1), HMF formation being the most temperature sen

59 G = -9 +/- 20 kJ.mol(-1), DeltaH = 64 +/- 14 kJ.mol(-1), and DeltaS= 247 +/- 50 J.mol(-1).K(-1).

60 = -20 +/- 19 kJ.mol(-1), DeltaH = -75 +/- 14 kJ.mol(-1), and DeltaS= -188 +/- 48 J.mol(-1).K(-1) for

61 (DeltaH()) for H2O formation increase by 14 kJ mol(-1) when Pd cluster diameters increase from 0.7 t

62 95% CI, -284 to 395 kJ) at 12 months and 143 kJ (95% CI, -241 to 526 kJ) at 24 months.

63 ) and NaClO4 (alpha = 400, DeltaGalpha = -15 kJ mol(-1)) in 4:1 dichloromethane-acetonitrile.

64 f TSMT that differ in energy by more than 15 kJ mol(-1).

65 74.150 kJ mol(-1), 111.174 kJ mol(-1) and 93.311 kJ mol(-1) of

66 thalene increases exponentially from 9 to 16 kJ/mol ( approximately 1.6-2.9 log units of sorption coe

67 and N2 was computed to be endothermic by 169 kJ/mol, which is energetically more favorable than forma

68 etric work capacity during contraction (2.17 kJ kg(-1)), which is over 50 times that of the same weig

69 rogen abstraction (15-lipoxygenation) was 17 kJ/mol lower than for arachidonic acid 12-lipoxygenation

70 74.150 kJ mol(-1), 111.174 kJ mol(-1) and 93.311 kJ mol(-1) of activation energy va

71 ue (DeltaE) for PyOM was between 4.0 and 175 kJ mol(-1); with manure-derived PyOM having the highest

72 G of the reaction ranged between -21 and -18 kJ mol(-1).

73 ding of NaI (alpha = 1300, DeltaGalpha = -18 kJ mol(-1)) and NaClO4 (alpha = 400, DeltaGalpha = -15 k

74 equently has a very small HOMO-LUMO gap (187 kJ mol(-1)).

75 ocess span 135 kJ/mol to 226 kJ/mol, and 188 kJ/mol to 268 kJ/mol, for neat and recycled PE, respecti

76 /aq) + H2O, we determine DeltaG = -20 +/- 19 kJ.mol(-1), DeltaH = -75 +/- 14 kJ.mol(-1), and DeltaS=

77 scopy showed an enthalpy of activation of 19 kJ mol(-1) and a approximately 2.5-fold kinetic isotope

78 yst for the HER-HOR in acids is 0.2 eV or 19 kJ mol(-1).

79 to an arene is favored by approximately 1.2 kJ mol(-1).

80 cement of -10.9, -22.0, -22.9, 2.09, and 1.2 kJ/mol for glyoxal monohydrate and -3.1, -10.3, -7.91, 6

81 grees C=1.58+/-0.02 min(-1) and Ea=161+/-2.2 kJ/mol.

82 s of CO adsorption ranging from 52.7 to 27.2 kJ/mol along the series Ni > Co > Fe > Mg > Mn > Zn, fol

83 rgy of stabilization (DeltaG(0)) of 32 +/- 2 kJ.mol(-1) For holoBcII, a first non-cooperative transit

84 on was suggested by DeltaDeltaGo values >4.2 kJ/mol obtained from double mutant cycle analysis.

85 elements at 25 degrees C is -1,970.0 +/- 4.2 kJ/mol.

86 n energies for k1 and k-1 were 3.04 and 45.2 kJ.mol(-1), respectively, and enthalpy change for K1 was

87 BA (55.9 kJ/mol) and 2-FM-Lys+2-FM-Arg (58.2 kJ/mol) were shown to be slightly more sensitive indicat

88 th a cone conformation, DeltaG(), being 63.2 kJ mol(-1).

89 e acceptors) changes by only approximately 2 kJ mol(-1) across the AnO2(2+) series, indicating that t

90 es and can contribute up to approximately -2 kJ/mol to the interaction.

91 2) ) with peak energy and power density of 2 kJ m(-2) (6.2 MJ m(-3) or 1.7 mWh cm(-3) ) and 150 kW m(

92 -10 +/- 29 kJ.mol(-1), DeltaH = -139 +/- 20 kJ.mol(-1), and DeltaS= -435 +/- 70 J.mol(-1).K(-1) for

93 protonation, we determine DeltaG = -9 +/- 20 kJ.mol(-1), DeltaH = 64 +/- 14 kJ.mol(-1), and DeltaS= 2

94 the solid-state reaction by approximately 20 kJ mol(-1), allowing the reaction to be achieved closer

95 key reaction is quite low ( approximately 20 kJ/mol), which is far less than the dissociation energy

96 y of these interactions was approximately 20 kJ/mol, suggesting involvement of hydrophobic interactio

97 an isosteric heat of adsorption as low as 20 kJ mol(-1) for carbon dioxide, which could bring a disti

98 ntails binding energies in the range of -202 kJ/mol to -127 kJ/mol.

99 and/or an additional energy criterion of 210 kJ).

100 ergies of the process span 135 kJ/mol to 226 kJ/mol, and 188 kJ/mol to 268 kJ/mol, for neat and recyc

101 hed remanence (1.16 T) giving a BHmax of 230 kJ m(-3).

102 -min infusion of isotonic glucose (15 g, 235 kJ) or saline to the duodenum or ileum.

103 ffective enthalpy of vaporization of 117-237 kJ mol(-1).

104 Activation energy was found to be 28.24 kJ mol(-1).

105 t Hoff analysis, yielding DeltaG(assn) = -24 kJ mol(-1) and an activation energy DeltaG(double dagger

106 J/2.5 h) and resting energy expenditure (243 kJ/d) and an anorexigenic appetite-sensation profile.Pro

107 plication of a PEF treatment (2 kV/cm; 11.25 kJ/kg) to the olive paste significantly increased the ex

108 imated a reaction activation energy of 14.25 kJ/mol and a temperature coefficient Q10 of 1.22 to corr

109 prompting).Mean energy (difference: -567.25 kJ; 95% CI: -697.95, -436.55 kJ; P < 0.001), saturated f

110 eakage was relatively low ( approximately 25 kJ/mol) and the yield of alkanals (10-18%) was higher th

111 a low activation barrier to conduction of 25 kJ mol(-1) .

112 kJ/mol to 226 kJ/mol, and 188 kJ/mol to 268 kJ/mol, for neat and recycled PE, respectively, and the

113 melting at 167-170 degrees C (DeltaHfus = 27 kJ.mol(-1)).

114 ize 2000 distorted geometries to within 0.28 kJ mol(-1) of the corresponding ab initio energy, and 50

115 s found to have an activation barrier of 280 kJ/mol, in contrast to 82 kJ/mol for the slowest step in

116 s thermochemistry yields DeltaG = -10 +/- 29 kJ.mol(-1), DeltaH = -139 +/- 20 kJ.mol(-1), and DeltaS=

117 rea: the change in DeltaG for binding is 0.3 kJ mol(-1) A(-2), corresponding to 5 kJ mol(-1) for each

118 1), and DeltaG(double dagger) = 43.8 +/- 0.3 kJ mol(-1) at 293 K).

119 to 1a in carbon tetrachloride (-23.5 +/- 0.3 kJ mol(-1)) interlocks our study with Laurence's scale o

120 Pa, relatively small amounts of energy (<0.3 kJ/g) are absorbed by the compression of these MOFs.

121 aH degrees = -10.9 +/- 0.4 and -11.8 +/- 0.3 kJ/mol; DeltaS degrees = -38 +/- 2 and -34 +/- 2 J/(mol.

122 +/- 1.10 x 10(4) M(-1) and DeltaG of -100.3 kJ mol(-1) in comparison to a Ka 0.41 x 10(3) +/- 0.09 M

123 was observed at pH 2.5: DeltaDeltaGF >/=11.3 kJ mol(-1) .

124 nd exchange having barriers of 17.8 and 19.3 kJ/mol for cyclopentene and cyclohexene, respectively.

125 ter change, namely lowering DeltaGCIA by 2.3 kJ mol(-1) relative to its wild-type value.

126 eF as weak ligand for binding (DeltaH = -2.3 kJ/mol; -TDeltaS = -19.5 kJ/mol) but not as substrate fo

127 culated to have a heat of formation of 398.3 kJ mol(-1) .

128 cluster 4H(2-) (232 +/- 4 kJ mol(-1), -46.3 kJ mol(-1)) the latter is found to react significantly f

129 y of 50 A m(-2) and an energy demand of 56.3 kJ gN(-1).

130 width of 0.68 nm, DeltaFperm(TcO4(-)) = -6.3 kJ mol(-1), compared to DeltaFperm(SO4(2-)) = +22.4 kJ m

131 was no relationship between W' (19.4 +/- 6.3 kJ) and muscle fibre type.

132 ng energy of CO2 to benzyl thiolate of -66.3 kJ mol(-1), consistent with the experimental observation

133 strongly exothermic process (DeltaH = -80.3 kJ/mol; -TDeltaS = 37.9 kJ/mol, Kd = 39 nm) whereby the

134 reaction, and values of DeltaG() = 91 +/- 3 kJ.mol(-1), DeltaH() = 84 +/- 9 kJ.mol(-1), and DeltaS()

135 0(10) cm(-3) at a specific energy input of 3 kJ/m(3), and the portable device generated (4.6 +/- 0.4)

136 surface nucleation is found to be 144 +/- 30 kJ/mol, very similar to that for interface nucleation.

137 on resulted in higher DIT ( approximately 30 kJ/2.5 h) and resting energy expenditure (243 kJ/d) and

138 ted Gibbs free energy as in the order of -30 kJ/mol and DHFR/TS molar ratio pointing to binding of 6

139 actions of ethyl nitrosoacrylate are over 30 kJ/mol lower than those that would be required for the c

140 diffuseness is emphasized, while Smax = 300 kJ/(K.m(3)) is obtained for Pb0.8Ba0.2ZrO3.

141 , Purple Haze and Nutri Red processed at 303 kJ/kg completely increased Caco-2 cells resistance towar

142 growth (scope for growth) from 0.59 to -0.31 kJ crab d(-1) in crabs fed with 1% plastic.

143 of formic acid (TOF = 1718 h(-1) and Ea = 31 kJ/mol) and one-pot reactions of formic acid, 2-nitrophe

144 a heat of CO adsorption (DeltaH(ads)) of -31 kJ mol(-1) for Au(0) and -64 kJ mol(-1) for Au(delta+) a

145 50 kJ mol(-1), 111.174 kJ mol(-1) and 93.311 kJ mol(-1) of activation energy values were found for L(

146 The heat of adsorption was below 32 kJ mol(-1) and the temperature of onset of intense therm

147 At the strongly binding Cu(I) sites (32 kJ mol(-1)) nuclear quantum effects result in higher ads

148 ly compound with a substantial lower GB (321 kJ/mol less) than 2,4-dimethyl-3-oxazoline.

149 umic Substances Society ranged from 16 to 34 kJ mol(-1).

150 The activation energy (35 kJ/mol) for dimerization is almost identical to this ent

151 onded pi-complex at Bronsted acid sites, -36 kJ/mol.

152 t 294 K and activation energy Ea = 64 +/- 37 kJ/mol.

153 with glucose-to-duodenum [-22%, -988 +/- 379 kJ (mean +/- SEM), Tukey's post hoc, P < 0.05]; and incr

154 xyquinoline and quinolone forms is 27 and 38 kJ mol(-1), for 5Me-HQE and 7Me-OQE, respectively.

155 ely 4 x 10(6) M(-1), DeltaG approximately 38 kJ/mol).

156 increasing temperature (activation energy=38 kJ/mol).

157 ng a DeltaG(double dagger) of 45, 39, and 39 kJ/mol, respectively.

158 nergy intake were 55 kJ (95% CI, -284 to 395 kJ) at 12 months and 143 kJ (95% CI, -241 to 526 kJ) at

159 less favorable relative to AH (-14.6 +/- 0.4 kJ/mol) when considering a simple additive model.

160 trations, with DeltaG(0) value of 65 +/- 1.4 kJ.mol(-1) These combined data highlight the importance

161 ieved accuracy (estimated uncertainty +/-1.4 kJ/mol), the ab initio energies become useful benchmarks

162 ps and an activation energy of 12.6 +/- 1.4 kJ/mol.

163 t of adsorption can also be tuned from -16.4 kJ/mol for CPM-200-Sc/Mg to -79.6 kJ/mol for CPM-200-V/M

164 ergies from experiments, with errors of -2-4 kJ using solvation method SMD in conjunction with hybrid

165 -1), compared to DeltaFperm(SO4(2-)) = +22.4 kJ mol(-1).

166 tion free energy (BDFE) of 5H(2-) (230 +/- 4 kJ mol(-1)) and the free energy DeltaG degrees PCET for

167 for the homoleptic cluster 4H(2-) (232 +/- 4 kJ mol(-1), -46.3 kJ mol(-1)) the latter is found to rea

168 the energy absorption typically reaches 3-4 kJ/g; for comparison, the energy release in the explosio

169 rees PCET for the reaction with TEMPO (-48.4 kJ mol(-1)) are very similar to values for the homolepti

170 The corresponding linear triple bond is 50.4 kJ/mol less stable in vacuo according to the calculation

171 han the "chemical accuracy" limit of about 4 kJ/mol.

172 e in the explosion of TNT is approximately 4 kJ/g.

173 ver the range 111-117 degrees C (DeltaH = +4 kJ.mol(-1)) via a melt-recrystallization process, with t

174 tion, providing a binding enthalpy of -34(4) kJ/mol.

175 % higher in DRY than HUM [263 (39), 248 (40) kJ; P < 0.01] in conjunction with equivalent autonomic r

176 ers with relative energies up to ~4 eV (~400 kJ/mol).

177 ound in winter (17.48 +/- 3.98 MJ d(-1), 402 kJ kg(-0.75) d(-1)) and the highest in summer (25.87 +/-

178 d to the conformational energy barrier of 42 kJ/mol for the wild-type pol beta reported previously.

179 rocesses are in the range of 42-52 and 42-43 kJ mol(-1), respectively.

180 r between phases [EF: 257 (37), ML: 255 (43) kJ, P = 0.62], but was 7 (9)% higher in DRY than HUM [26

181 tressor and no stressors translates into 435 kJ, a difference that could add almost 11 pounds per yea

182 for the degradation of betalains was 42.449 kJ mol(-1).

183 e that of MEA-PCC (60-72 kJ/mol versus 33-46 kJ/mol, respectively).

184 A-lattice ones (-462 +/- 70 vs. -472 +/- 46 kJ/mol).

185 theory, where DeltaG degrees was 39.31-51.48 kJ mol(-1).

186 moiety with a modest activation energy of 48 kJ/mol.

187 = 0.51 T, and energy product (BH)max = 43.49 kJ/m(3) (5.47 MGOe).

188 er, consistent with this isomer being >/=0.5 kJ mol(-1) lower in energy than isomers where the carbox

189 d a proton surface affinity of -13.0 +/- 0.5 kJ mol(-1).

190 metal sites, leading to increases of 0.4-1.5 kJ/mol in the H2 binding enthalpies relative to M2(dobdc

191 cule indicated a higher energy of only +10.5 kJ mol(-1) for the mu2 -kappa(1) O:kappa(1) O' bonding m

192 -d-glucose fragments, stronger in fIIa (15.5 kJ.mol(-1)) than in fXa (2.8 kJ.mol(-1)).

193 ding (DeltaH = -2.3 kJ/mol; -TDeltaS = -19.5 kJ/mol) but not as substrate for reduction or oxidation.

194 rge difference in adsorption enthalpy of 2.5 kJ mol(-1) between D2 and H2 results in D2-over-H2 selec

195 ctivation energies: FRT IRE-RNA 47.0 +/- 2.5 kJ/mol, ACO2 IRE-RNA 35.0 +/- 2.0 kJ/mol.

196 on IrO2(110), and equal to a value of 28.5 kJ/mol.

197 indicate that this energy difference is 3-5 kJ mol(-1), in agreement with the experimental results.

198 tivation law with an apparent energy of 32.5 kJ/mol, showing that the redox reaction rate is approxim

199 GPa and specific energy dissipation of 325.5 kJ/kg, surpassing previously reported values at similar

200 ss spectrometry indicated that a loss of 4-5 kJ/mol/protomer in the N3 domain that is peripheral to t

201 rotational barriers (DeltaG()Tc = 56.5-67.5 kJ/mol).

202 action energy was found to vary by about 7.5 kJ mol(-1) on going from a phenyl-phenyl to an anthracen

203 the apparent activation energy from 70 +/- 5 kJ/mol (in product-free gas) to 105 +/- 7 kJ/mol (in ful

204 ees C=0.94+/-0.14 min(-1) and Ea,l=178+/-8.5 kJ/mol, and a stable fraction, representing 58+/-2%, wit

205 nergy difference to the TSA-like form is 8.5 kJ/mol.

206 yield values for the ordering energy of 9.5 kJ/mol-cation.

207 is 0.3 kJ mol(-1) A(-2), corresponding to 5 kJ mol(-1) for each additional CH2 group in the guest, i

208 oscopy showed that DeltaG(assn) = -24.9(2.5) kJ mol(-1) for 4.

209 rent activation energy (Eapp) of 56.5 (+/-5) kJ mol-1 and is kinetically limited by desorption of mol

210 plemented DraE (DraE-sc) by approximately 50 kJ mol(-1) in an exclusively thermodynamic manner, i.e.

211 igher in energy than the tri-keto form by 50 kJ mol(-1) which must be more than compensated by enhanc

212 at 12 months and 143 kJ (95% CI, -241 to 526 kJ) at 24 months.

213 activation energy DeltaG(double dagger) = 54 kJ mol(-1).

214 th an associated moderate energy input of 54 kJ/mol, typical for the full CO2 desorption in conventio

215 ph, with the bct being 0.32 and the fcc 0.55 kJ/mol higher in enthalpy.

216 erence: -567.25 kJ; 95% CI: -697.95, -436.55 kJ; P < 0.001), saturated fat (difference: -2.37 g; 95%

217 timated differences in energy intake were 55 kJ (95% CI, -284 to 395 kJ) at 12 months and 143 kJ (95%

218 conformational pathway varies from 25 to 58 kJ/mol, compared to the conformational energy barrier of

219 hest in summer (25.87 +/- 3.88 MJ d(-1), 586 kJ kg(-0.75) d(-1)).

220 ngitudinal ones (-462 +/- 70 vs. -392 +/- 59 kJ/mol), which suggests a dramatic lateral stabilization

221 rved free adsorption energy of -52.7 +/- 0.6 kJ/mol, PAH adsorption was found to be surprisingly less

222 ydrate and -3.1, -10.3, -7.91, 6.11, and 1.6 kJ/mol for methylglyoxal monohydrate with uncertainties

223 ignificant energy saving equivalent to 175.6 kJ mol(-1).

224 ow thermal activation energy barrier of 22.6 kJ/mol.

225 kJ mol(-1) for BILP-15 and from 32.0 to 31.6 kJ mol(-1) for BILP-16.

226 (-1)s(-1)), with low Ea and Q10 values (42.6 kJ mol(-1) and 1.8, respectively).

227 getic penalty per rotor of approximately 5-6 kJ mol(-1) was observed in less strained situations wher

228 from -16.4 kJ/mol for CPM-200-Sc/Mg to -79.6 kJ/mol for CPM-200-V/Mg.

229 s, in contrast, enhances its stability by ~6 kJ/mol, presumably due to excluded volume and electrosta

230 ncy, resulting in a net energy gain of 57-62 kJ/mol-CO2 captured.

231 ium ion 5 with binding energies of 57 and 62 kJ/mol for cyclopentene and cyclohexene, respectively, w

232 derate enthalpic barrier of approximately 62 kJ/mol, to give H2 and an antiferromagnetically coupled

233 aH(ads)) of -31 kJ mol(-1) for Au(0) and -64 kJ mol(-1) for Au(delta+) at 33% surface coverage.

234 We calculate a PE of 655 kJ/kg CO2, which is lower than that of the best performi

235 values for stearic acid show a spread of 68 kJ mol(-1).

236 5 kJ/mol (in product-free gas) to 105 +/- 7 kJ/mol (in full reformate gas).

237 for nonaqueous H2 oxidation by 610 mV (117.7 kJ mol(-1)).

238 ved for molecular model compounds (148 +/- 7 kJ/mol).

239 latively low activation energy (18.4 +/- 2.7 kJ mol(-1)).

240 equation), DeltaH(double dagger) = 23 +/- 7 kJ mol(-1), and DeltaG(double dagger) = 101 +/- 9 kJ mol

241 rriers were determined to be E(a) = 25 +/- 7 kJ mol(-1) (Arrhenius equation), DeltaH(double dagger) =

242 Overall, the alkoxy group is -41 +/- 7 kJ/mol more stable than physisorbed pentene, establishin

243 Eapp), across the techniques applied, of 8.7 kJ mol-1, within the temperature range investigated (276

244 asification got remarkably reduced from 95.7 kJ/mol to 12.1 kJ/mol (A2 model).

245 IA as a point of reference ( approximately 7 kJ mol(-1)), we examined its impact on various aspects o

246 barrier to screw-sense inversion of about 70 kJ mol(-1) .

247 e olefin binding enthalpies, below 55 and 70 kJ/mol for ethylene and propylene, respectively, indicat

248 gn with DeltaHpart becoming endothermic (+70 kJ/mol) and entropically favored (DeltaSpart = +240 J/(m

249 tion for a 3-effect evaporator, and 980-7000 kJ/kg for a 5-effect evaporator.

250 AC is less than twice that of MEA-PCC (60-72 kJ/mol versus 33-46 kJ/mol, respectively).

251 with much lower barriers of approximately 72 kJ mol(-1).

252 kJ mol(-1) and the overall energy gain of 72 kJ mol(-1).

253 nergies for all colour parameters were 64-73 kJ mol(-1).

254 zontal lineO bond in CO2 ( approximately 750 kJ/mol).

255 n in conjunction with each UVR exposure (1.8 kJ m(-2)).

256 significantly higher (DeltaG() = 102.6-103.8 kJ/mol).

257 ires a very high activation energy (Ea 106.8 kJ mol(-1)) and consequently has a large Q10 value of 4.

258 transition-state recognition by up to -14.8 kJ mol(-1).

259 h(-1) and an activation energy (Ea ) of 18.8 kJ mol(-1) .

260 r within a HPW molecule is higher (29.1-18.8 kJ/mol) than the barrier for intermolecular proton trans

261 r in fIIa (15.5 kJ.mol(-1)) than in fXa (2.8 kJ.mol(-1)).

262 (-1) K(-1), and DeltaG(double dagger) = 59.8 kJ mol(-1) at 293 K).

263 ength of this second coordination is ca. 6-8 kJ mol(-1).

264 e latch region results in an approximately 8 kJ mol(-1) decrease in the activation energy for ion tra

265 lglyoxal monohydrate with uncertainties of 8 kJ/mol.

266 al cycle to yield DeltaHf,298K = (325 +/- 8) kJ mol(-1), ca. 10 kJ mol(-1) below the previous value.

267 ) atm and increased the DeltaHvap,eff to >80 kJ/mol, at least in part via the formation of ammonium o

268 t is stabilized by an unexpectedly large -80 kJ mol(-1).

269 ion barrier of 280 kJ/mol, in contrast to 82 kJ/mol for the slowest step in the iron(IV)-oxo catalyti

270 genetic risk group versus control group 0.85 kJ/kg/d (95% CI -2.07 to 3.77, p = 0.57); phenotypic ris

271 especially high barriers, ranging from 75-86 kJ mol(-1).

272 f rotation, DeltaG(double dagger)298 = 82-86 kJ mol(-1), were determined by (1)H NMR for 12a, 12d, 12

273 The diets were equal in energy (8750 kJ/d), protein (17% of energy), and food profile, emphas

274 Fperm(TcO4(-)) and DeltaFperm(SO4(2-)) of 89 kJ mol(-1).

275 (10,149 +/- 831 compared with 11,931 +/- 896 kJ; P < 0.01), and daily EI remained lower when the PPX

276 dard enthalpy of formation, -1,779.6 +/- 1.9 kJ/mol, was obtained by high temperature oxide melt drop

277 l(-1), and DeltaG(double dagger) = 101 +/- 9 kJ mol(-1) (Eyring equation).

278 -1)), and electrical activation energy (12.9 kJ mol(-1)) was also carried out.

279 ing affinity (Qst) dropped from 33.0 to 28.9 kJ mol(-1) for BILP-15 and from 32.0 to 31.6 kJ mol(-1)

280 rk performed (55.6+/-35.3 versus 49.2+/-28.9 kJ; P=0.04).

281 uraninite) and SiO2 (quartz) by 25.6 +/- 3.9 kJ/mol.

282 cess (DeltaH = -80.3 kJ/mol; -TDeltaS = 37.9 kJ/mol, Kd = 39 nm) whereby the thioimide adduct is form

283 its lower activation energy, 2-FM-GABA (55.9 kJ/mol) and 2-FM-Lys+2-FM-Arg (58.2 kJ/mol) were shown t

284 ll ligands bound, is lower by only about 8.9 kJ/mol than that of the Michaelis or apo complex conform

285 ) = 91 +/- 3 kJ.mol(-1), DeltaH() = 84 +/- 9 kJ.mol(-1), and DeltaS() = -23 +/- 31 J.mol(-1).K(-1) fo

286 rotating bonds, but ranged between -5 and -9 kJ mol(-1) for </=5 rotors.

287 tially identical heats of adsorption near 90 kJ/mol.

288 ,f show high rotational barriers of up to 92 kJ mol(-1), unlike those of (1R)-2e,f and with much lowe

289 ion (7904 +/- 610 compared with 9041 +/- 928 kJ; P < 0.05).

290 ive Gibbs free energy gain, DeltaG = -115.95 kJ/mol, calculated using the density functional theory a

291 gnificant temperature dependence (Ea = 20-96 kJ mol(-1)).

292 o pastes and purees varies from 1200 to 9700 kJ/kg over the range of 8%-40% outlet solids concentrati

293 mol(-1) for ascorbic acid and from 49 to 99 kJ mol(-1) for colour intensity.

294 ome, objectively measured physical activity (kJ/kg/day), and also measured several secondary outcomes

295 oportion of variance in total energy intake (kJ) and amount of food intake (g) predicted by frequency

296 C-H bond cleavage is 9.5 kilojoule per mole (kJ/mol) lower than the binding energy of the adsorbed pr

297 ., 1.05 [0.89-1.23] and 0.92 [0.71-1.18] per kJ/m(2) for center-level monthly mean UVR for the 13- to

298 r kJ/m(2)) and minimum (1.25 [1.06-1.47] per kJ/m(2)) UVR dose exposure.

299 - to 7-year-olds (e.g., 1.24 [0.96-1.59] per kJ/m(2) for country-level monthly mean UVR).

300 31 [95% confidence interval = 1.05-1.63] per kJ/m(2)) and minimum (1.25 [1.06-1.47] per kJ/m(2)) UVR

301 ating with shorter survival by 4.8 years per kJ.