ライフサイエンスコーパス: kJ

1 .0 +/- 2.5 kJ/mol, ACO2 IRE-RNA 35.0 +/- 2.0 kJ/mol.

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

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

4 cm(3) (47 degrees C) compared to 3.9 and 7.0 kJ/cm(3) (86 degrees C).

5 m(3) (68 degrees C) to 2.23 +/- 0.04% at 7.0 kJ/cm(3) (86 degrees C).

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

7 aG degrees values of 0.64, 56.55, and -10.00 kJ/mol, respectively.

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

9 .59 kJ mol(-1)), enthalpy (DeltaH(0) = 18.05 kJ mol(-1)), and entropy (DeltaS(0) = 68.92 J/K/mol) wer

10 +/- 0.09 M(-1) and DeltaG of -19.2 +/- 0.06 kJ mol(-1) for COX-1.

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

12 in energy density from 0.34 +/- 0.09% at 0.1 kJ/cm(3) (68 degrees C) to 2.23 +/- 0.04% at 7.0 kJ/cm(3

13 (DeltaG(*) values ranging from 85.0 to 137.1 kJ.mol(-1) and above).

14 1 gN m(-2) d(-1) at an energy demand of 26.1 kJ gN(-1).

15 eal a solution Lewis acidity of 3 (FIA=262.1 kJ mol(-1) ) that is higher than that of the landmark Le

16 nd - TDeltaDelta S degrees (R - S) = 3 +/- 1 kJ/mol.

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

18 on enthalpies are Delta H(*)(app) = 43 +/- 1 kJ mol(-1) irrespective of active site location, confini

19 ior, DeltaDelta H degrees (R - S) = -5 +/- 1 kJ/mol and - TDeltaDelta S degrees (R - S) = 3 +/- 1 kJ/

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

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

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

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

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

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

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

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

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

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

30 croorganisms, with available energies of -10 kJ/mol for acetate oxidation and -20 kJ/mol for hydrogen

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

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

33 n for a model compound in the vacuum: 90-100 kJ mol(-1) ).

34 calcium content levels (ca. 6.5-30 mg Ca/100 kJ) were prepared in accordance with the guidelines of C

35 coupling, which can be as large as 1 eV (100 kJ mol-1), leads to the formation of new hybrid states,

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

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

38 eef briskets were subjected to shockwave (11 kJ/pulse) and were sous vide-cooked at 60 degrees C for

39 ation energy drops from 130 kJ mol(-1) to 11 kJ mol(-1) .

40 ions that have a high activation energy (120 kJ/mol).

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

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

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

44 n apparent activation barrier of (72 +/- 13) kJ mol(-1).

45 The strain in these nanorings is 90-130 kJ mol(-1), as estimated both from DFT calculation of ho

46 he apparent activation energy drops from 130 kJ mol(-1) to 11 kJ mol(-1) .

47 +/- SD of 175 +/- 1362 kJ/d and 86 +/- 1344 kJ/d, respectively.

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

49 timated TEE by a mean +/- SD of 175 +/- 1362 kJ/d and 86 +/- 1344 kJ/d, respectively.

50 The 9 and 14 kJ/mol magnitudes of the effects for 3HB6H and HPAH-C(2)

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

52 n phase reaction is decreased by 162 and 140 kJ mol(-1) according to calculations done with the SMD a

53 stimated TEE by a mean +/- SD of 24 +/- 1401 kJ/d.

54 /mol for vacuum, and 1.089, 4.923 and 14.142 kJ/mol for non-vacuum, respectively.

55 95% CI, -284 to 395 kJ) at 12 months and 143 kJ (95% CI, -241 to 526 kJ) at 24 months.

56 ime of 240 s at Ultraviolet-C dosage of 2.15 kJ/m(2) was observed to provoke a considerable increase

57 wer hazard when 20% versus 10% of a fixed 15 kJ kg(-1) d(-1) PAEE volume was from MVPA).

58 gy required to phosphorylate organics is ~15 kJ/mol, requiring either very low water activities or re

59 nterval 4-35%) lower hazard for 20 versus 15 kJ kg(-1) d(-1) PAEE with 10% from MVPA).

60 74.150 kJ mol(-1), 111.174 kJ mol(-1) and 93.311 kJ mol(-1) of

61 * oxidants possess energies greater than 150 kJ mol(-1).

62 possesses even higher toughness (Gamma ~ 155 kJ m(-3) ), which is 40% higher over that of (silica) =

63 how that a minimum energy consumption of 164 kJ.mol(-1) CO(2) could be achieved.

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

65 entropies, which varied from 92.05 to 99.17 kJ/mol, 88.83 to 95.94 kJ/mol, -35.58 to -4.81 J/mol K,

66 th verified stabilization energies below -17 kJ/(mol Si), comparable to or better than known OSDAs fo

67 coupling low heat of adsorption (-10 to -17 kJ mol(-1) (alkene) ), high alkene:alkane selectivity (4

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

69 74.150 kJ mol(-1), 111.174 kJ mol(-1) and 93.311 kJ mol(-1) of activation energy va

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

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

72 ctivation energies in the range of 96 +/- 19 kJ/mol are determined, with Pt leading to the lowest ene

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

74 d observation of a corrin triplet (E(T) =190 kJ mol(-1) ) and was found to be an excellent photo-sens

75 ous (DeltaG = -39.7 +/- 0.1 to -43.2 +/- 0.2 kJ/mol) between 14 and 43 degrees C.

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

77 couple by up to 220 mV (DeltaDeltaG = -22.2 kJ mol(-1)).

78 rbon was exothermic (Delta H = -14.4 +/- 3.2 kJ mol(-1) for T = 20-94 degrees C) and followed the Fre

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

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

81 Joule heating with a low energy input of 7.2 kJ per gram graphene.

82 ) was most favorable with a DeltaG(*) of 7.2 kJ/mol.

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

84 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(

85 on nor after UV-C treatment with a dose of 2 kJ/L, which is sufficient for the inactivation of microo

86 teurization as well as with a UV-C dose of 2 kJ/L.

87 eaking the hydrogen bond is found to be 6-20 kJ mol(-1) .

88 of -10 kJ/mol for acetate oxidation and -20 kJ/mol for hydrogenotrophic methanogenesis.

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

90 d light was obtained after treatment with 20 kJ/m(2) and 3-days of storage at 20 degrees C.

91 methyl acetate despite high barriers of >200 kJ/mol.

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

93 position (Delta H(D)) of -1135 J g(-1) (-207 kJ mol(-1)).

94 after UV-C treatment with a high dose of 21 kJ/L.

95 termined the triplet energy of HDA to be 217 kJ mol(-1), whereas a complementary method based on trip

96 chnology (energy varied between 7.27 and 218 kJ/kg).

97 in water from HVED pre-treated peels at 218 kJ/kg and in aqueous glycerol from pre-treated peels at

98 , decreasing the heat of adsorption by 19-22 kJ molH2-1 while inducing an additional entropy loss of

99 .42 kJ mol(-1); [Formula: see text] = -32.22 kJ mol(-1); [Formula: see text] = -31.84 kJ mol(-1)).

100 methane adsorption enthalpies of -15 to -22 kJ/mol.

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

102 transitions in A(1)R-G279S(7.44) (73 +/- 23 kJ/mol) than in wild-type A(1)R (135 +/- 4 kJ/mol) or in

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

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

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

106 kJ/mol) or in A(1)R-Y288A(7.53) (184 +/- 24 kJ/mol).

107 nding site with a binding free energy of -24 kJ/mol.

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

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

110 activation directly at the MSI (E(app) ~ 25 kJ/mol) and significantly slower heterolytic H(2) activa

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

112 xhibit fracture energy, Gamma, of up to 2500 kJ m(-2) , exceeding the toughest existing materials.

113 si-phases (qF: 268 +/- 31 kJ, qL: 263 +/- 26 kJ, P = 0.31) but was 5 +/- 7% higher during DRY than du

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

115 ct was only observed in water media after 27 kJ/cm(3) by FRAP (47 degrees C) and DPPH (86 degrees C)

116 e of solutes (citric acid and NaCl) after 27 kJ/cm(3) reduced degradation of flavonoids.

117 In the water media, at 27 kJ/cm(3) and 47 degrees C, the total flavonoid content i

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

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

120 alculated to be Delta(vap)H = 91.27 +/- 0.28 kJ/mol compared to Delta(vap)H(corr) = 91.44 kJ/mol for

121 Y than during HUM (273 +/- 29 kJ, 258 +/- 28 kJ; P = 0.03).

122 igher during DRY than during HUM (273 +/- 29 kJ, 258 +/- 28 kJ; P = 0.03).

123 tection for alpha + beta carotene (E(a) = 29 kJ/mol).

124 mS cm(-1) and a low activation energy of 29 kJ mol(-1) as determined by impedance spectroscopy.

125 two HgCN molecules was calculated to be 296 kJ mol(-1) and that for CNHg-HgNC into two HgNC molecule

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

127 resin was exothermic (DeltaH = -6.3 +/- 1.3 kJ/mol) and spontaneous (DeltaG = -39.7 +/- 0.1 to -43.2

128 +/- 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

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

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

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

132 kJ/mol) and deactivation (E(D) = 62.23 +/- 3 kJ/mol) energies of hydrolysis.

133 ees C and intrinsic stability DeltaGu = 24.3 kJ/mol) and a sub-optimal immunogenicity profile.

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

135 and with a low reaction-energy barrier (47.3 kJ mol(-1) ).

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

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

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

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

140 )) values were determined to be 45.9 x 10(3) kJ/kg-mol and 18125.95 min(-1), respectively using the A

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

142 ts, with barrier lowering on the order of 30 kJ mol(-1) in dimethyl sulfoxide and acetonitrile.

143 The frameworks exhibit a significant (30 kJ.mol(-1)) variation in the enthalpy of formation depen

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

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

146 for CNHg-HgNC into two HgNC molecules is 304 kJ mol(-1) .

147 differ between quasi-phases (qF: 268 +/- 31 kJ, qL: 263 +/- 26 kJ, P = 0.31) but was 5 +/- 7% higher

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

149 50 kJ mol(-1), 111.174 kJ mol(-1) and 93.311 kJ mol(-1) of activation energy values were found for L(

150 significant enhancements in catalysis (10-32 kJ mol(-1) in barrier lowering) when the catalyst was pr

151 m temperature and activation energy of 30-32 kJ mol(-1) expanding the recently introduced family of l

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

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

154 ee molecules (DeltaG(25 degrees C)(0)=-29.35 kJ mol(-1)), and the binding constant was 1.39 x 10(5) M

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

156 al phenolic content increased >56% at 3.6-36 kJ/cm(3), indicating production of phenolic compounds.

157 ed better protection to vitamin E (E(a) = 36 kJ/mol), whereas SD-M provided better protection for alp

158 shorter lengths from treatments at 27 and 36 kJ/cm(3) (47 degrees C) compared to 3.9 and 7.0 kJ/cm(3)

159 queous glycerol from pre-treated peels at 36 kJ/kg.

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

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

162 desorption with an energy consumption of 374 kJ.mol(-1) CO(2) and a CO(2) purity higher than 95%.

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

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

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

166 , creatinine, and glutamine was 72.2 +/- 0.4 kJ.mol(-1).

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

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

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

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

171 nd with an activation energy of 81.1 +/- 1.4 kJ/mol.

172 3 kJ/mol) than in wild-type A(1)R (135 +/- 4 kJ/mol) or in A(1)R-Y288A(7.53) (184 +/- 24 kJ/mol).

173 electrochemical energy consumption of 155.4 kJ mol(-1) or 0.98 kWh kg(-1) of CO(2) and a CO(2) captu

174 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

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

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

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

178 the isosteric heat of adsorption (21.9-30.4 kJ/mol) for these CPMs is as low as about one-third of t

179 horter 2.347 angstrom Zn-Zn bond in the 37.4 kJ mol(-1) higher energy isocyanide CNZnZnNC, and a long

180 opants can affect the internal energy (-39.4 kJ mol(-1) with humidity in a nitrogen plasma and +15.7

181 ess (8.4 MN.m/kg) and energy absorption (4.4 kJ/kg) upon loading.

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

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

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

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

186 n state for racemization by approximately 40 kJ mol(-1) , thereby facilitating the observed dynamic k

187 ergy per volume (Q(UV)) ranged from 12 to 40 kJ/L (90 min to 5 h).

188 % higher in DRY than HUM [263 (39), 248 (40) kJ; P < 0.01] in conjunction with equivalent autonomic r

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

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

191 ) for binding ( [Formula: see text] = -33.42 kJ mol(-1); [Formula: see text] = -32.22 kJ mol(-1); [Fo

192 attraction raises the energy barrier from 42 kJ/mol for unsubstituted DBCOD to 68 kJ/mol for diamide-

193 ormation requires an activation energy of 42 kJ/mol, which is substantially lower than those of exist

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

195 an +/- SD of the residuals is -0.02 +/- 0.44 kJ/min.

196 kJ/mol compared to Delta(vap)H(corr) = 91.44 kJ/mol for the reference correlation.

197 urely carbon-fibre reinforced composites (44 kJ m(-2)).

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

199 2) activation mediated by water (E(app) ~ 45 kJ/mol).

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

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

202 = 0.51 T, and energy product (BH)max = 43.49 kJ/m(3) (5.47 MGOe).

203 text]) was found to be in the range of 45~49 kJ/mol, which was about 20% larger than that between the

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

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

206 rbonate formation: DeltaG(*) = +92.6 +/- 2.5 kJ mol(-1).

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

208 dmark Lewis acid B(C(6) F(5) )(3) (FIA=220.5 kJ mol(-1) ).

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

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

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

212 re respectively 38.2, 24.7, 38.0, 38.2, 41.5 kJ/mol.

213 ees C and intrinsic stability DeltaGu = 63.5 kJ/mol).

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

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

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

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

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

219 ng of the barrier to unfolding in G37R by >5 kJ/mol(-1) over the other variants, consistent with expe

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

221 exergonic ( DeltaG (r) <0), yielding ~30-50 kJ mol(-1) .

222 s, and with an activation energy of about 50 kJ/mol.

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

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

225 dissociation free energies that are over 50 kJ/mol below those of their keto equivalents.

226 pai bond strength is found to be 0.53 eV (51 kJ mol(-1)).

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

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

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

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

231 on to 2 degrees carbocations were -49 to -58 kJ/mol.

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

233 Gibbs free energy (DeltaG(0) = -2.59 kJ mol(-1)), enthalpy (DeltaH(0) = 18.05 kJ mol(-1)), an

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

235 oxidative stability (activation energy 105.6 kJ/mol).

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

237 vironment with an adsorption energy of - 4.6 kJ mol(-1) per He atom.

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

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

240 ith this surface stabilizes the protein by 6 kJ mol(-1) , a value that is in good agreement with theo

241 All FimA monomers proved to be 50-60 kJ/mol less stable against unfolding than their pilus ro

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

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

244 ted, with an activation energy as high as 63 kJ mol(-1) in DMSO-d(6) solution (DFT prediction for a m

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

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

247 from 42 kJ/mol for unsubstituted DBCOD to 68 kJ/mol for diamide-substituted DBCOD.

248 lectric fields (PEF) (1.4-1.7 kV/cm, 653-695 kJ/kg) and heating (60 and 80 degrees C for 10 min) at d

249 es well with the experimental value of 102.7 kJ/mol.

250 with humidity in a nitrogen plasma and +15.7 kJ mol(-1) with fluorobenzene in an air plasma).

251 kinetics found a triplet energy of 184 +/- 7 kJ mol(-1).

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

253 ination of the activation (E(A) = 50.3 +/- 7 kJ/mol) and deactivation (E(D) = 62.23 +/- 3 kJ/mol) ene

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

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

256 exhibiting an overall activation energy of 7 kJ mol(-1), which was estimated in vacuum at the B3LYP/6

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

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

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

260 an adsorption enthalpy (DeltaH(ads)) of +71 kJ mol(-1).

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

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

263 est negative values ofDeltaH degrees (-11.74 kJ/mol) andDeltaS degrees (-8.08 J/K.mol) led to the mos

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

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

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

267 than CLE (81.3 +/- 27.7 versus 48.9 +/- 23.8 kJ, p = 0.0001).

268 34.6 mJ/m(2) and E(a) was quantified as 32.8 kJ/mol.

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

270 one-third of that for peroxo-MOF-74-Fe (66.8 kJ/mol).

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

272 an apparent activation barrier of (80 +/- 8) kJ mol(-1).

273 owers the fragmentation barrier by around 80 kJ mol(-1) in the gas phase, while a negative charge has

274 .22 kJ mol(-1); [Formula: see text] = -31.84 kJ mol(-1)).

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

276 nity (873 kJ mol(-1)) compared to NH(3) (854 kJ mol(-1)).

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

278 d because of its higher proton affinity (873 kJ mol(-1)) compared to NH(3) (854 kJ mol(-1)).

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

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

281 activation energy of 0.665, 2.650 and 13.893 kJ/mol for vacuum, and 1.089, 4.923 and 14.142 kJ/mol fo

282 The calculated barrier (DeltaG( ) = 107.9 kJ/mol; at the M06L/6-311+G(d,p)/SDD level of theory) fo

283 nce between the two polymorphic forms of 2.9 kJ/mol was estimated.

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

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

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

287 ndard free energy change of approximately -9 kJ/mol, which is a large contribution to the delicate ba

288 The Delta(soil-air)U values were 328 and 90 kJ/mol for chlorpyrifos in the absence and presence of f

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

290 Up to 92 kJ/mol of thermal energy was stored in the compounds, de

291 d from 92.05 to 99.17 kJ/mol, 88.83 to 95.94 kJ/mol, -35.58 to -4.81 J/mol K, respectively (R(2) > 0.

292 ary carbocations were calculated as 76 to 97 kJ/mol and enthalpies for subsequent charge migration to

293 lk fibres achieving an impact strength of 98 kJ m(-2), which is twice that of purely carbon-fibre rei

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

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

296 ., 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

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

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

299 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

300 ating with shorter survival by 4.8 years per kJ.