https://en.formulasearchengine.com/index.php?action=history&feed=atom&title=Inverse_relationInverse relation - Revision history2026-04-09T01:56:25ZRevision history for this page on the wikiMediaWiki 1.43.0-wmf.28https://en.formulasearchengine.com/index.php?title=Inverse_relation&diff=246459&oldid=preven>JMP EAX: /* Properties */ I'm guess that should be defined there2014-08-23T23:01:19Z<p><span class="autocomment">Properties: </span> I'm guess that should be defined there</p>
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<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div>'<del style="font-weight: bold; text-decoration: none;">''Temperature jump''' </del>is <del style="font-weight: bold; text-decoration: none;">a technique used in </del>the <del style="font-weight: bold; text-decoration: none;">study of </del>[[<del style="font-weight: bold; text-decoration: none;">chemical kinetics]]. It usually involves the discharging of a capacitor (in the kV range) through a small volume (<mL) of a conducting solution containing the molecule</del>/<del style="font-weight: bold; text-decoration: none;">reaction to be studied</del>. <del style="font-weight: bold; text-decoration: none;">In some versions of the apparatus used, the solution is heated instead by the output of a pulsed laser which emits in the near infra-red</del>. <del style="font-weight: bold; text-decoration: none;">When laser heating is employed, the solution need not be conducting</del>. <del style="font-weight: bold; text-decoration: none;">In both cases, the temperature of the solution is caused to rise by a small amount in microseconds (or less in the case of laser heating)</del>. <del style="font-weight: bold; text-decoration: none;">This allows the study of the shift in equilibrium of reactions that equilibrate in milliseconds (or microseconds with laser temperature jump), these changes most commonly being observed using [[absorption spectroscopy</del>]] <del style="font-weight: bold; text-decoration: none;">or </del>[<del style="font-weight: bold; text-decoration: none;">[fluorescence spectroscopy]]</del>. <del style="font-weight: bold; text-decoration: none;">Due to the small volumes involved the temperature of the solution returns to that of its surroundings in minutes</del>.<del style="font-weight: bold; text-decoration: none;"><ref>{{cite book|title=Handbook of biochemical kinetics|author=Daniel L. Purich, R. Donald Allison|year= 1999|publisher=Academic Press|isbn=0-12-568048-1}}<</del>/<del style="font-weight: bold; text-decoration: none;">ref></del></div></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><ins style="font-weight: bold; text-decoration: none;">Golda is what</ins>'<ins style="font-weight: bold; text-decoration: none;">s created on my birth certification although it </ins>is <ins style="font-weight: bold; text-decoration: none;">not </ins>the <ins style="font-weight: bold; text-decoration: none;">name on clairvoyance </ins>[[<ins style="font-weight: bold; text-decoration: none;">http:/</ins>/<ins style="font-weight: bold; text-decoration: none;">www</ins>.<ins style="font-weight: bold; text-decoration: none;">aseandate</ins>.<ins style="font-weight: bold; text-decoration: none;">com/index</ins>.<ins style="font-weight: bold; text-decoration: none;">php?m=member_profile&p=profile&id=13352970 aseandate</ins>.<ins style="font-weight: bold; text-decoration: none;">com</ins>]] <ins style="font-weight: bold; text-decoration: none;">my </ins>[<ins style="font-weight: bold; text-decoration: none;">http://brazil</ins>.<ins style="font-weight: bold; text-decoration: none;">amor-amore</ins>.<ins style="font-weight: bold; text-decoration: none;">com</ins>/<ins style="font-weight: bold; text-decoration: none;">irboothe cheap psychic readings] birth certificate</ins>. <ins style="font-weight: bold; text-decoration: none;">My wife and I live </ins>in <ins style="font-weight: bold; text-decoration: none;">Mississippi but now I</ins>'<ins style="font-weight: bold; text-decoration: none;">m contemplating other choices</ins>. <ins style="font-weight: bold; text-decoration: none;">Invoicing </ins>is <ins style="font-weight: bold; text-decoration: none;">my profession. I am truly fond of handwriting but I can</ins>'t <ins style="font-weight: bold; text-decoration: none;">make it my profession truly.</ins><<ins style="font-weight: bold; text-decoration: none;">br</ins>><<ins style="font-weight: bold; text-decoration: none;">br</ins>><ins style="font-weight: bold; text-decoration: none;">Also visit my web blog psychics online </ins>([http://<ins style="font-weight: bold; text-decoration: none;">medialab</ins>.<ins style="font-weight: bold; text-decoration: none;">zendesk</ins>.<ins style="font-weight: bold; text-decoration: none;">com</ins>/<ins style="font-weight: bold; text-decoration: none;">entries</ins>/<ins style="font-weight: bold; text-decoration: none;">54181460-Will-You-Often-End-Up-Bored-Try-One-Of-These-Hobby-Ideas- visit the next web site</ins>]<ins style="font-weight: bold; text-decoration: none;">)</ins></div></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div> </div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><del style="font-weight: bold; text-decoration: none;">The fractional extent of the reaction (''i</del>.<del style="font-weight: bold; text-decoration: none;">e.'' the percentage change </del>in <del style="font-weight: bold; text-decoration: none;">concentration of a measurable species) depends on the molar enthalpy change (Δ''H'</del>'<del style="font-weight: bold; text-decoration: none;">°) between the reactants and products and the equilibrium position</del>. <del style="font-weight: bold; text-decoration: none;"> If ''K'' </del>is <del style="font-weight: bold; text-decoration: none;">the equilibrium constant and ''dT'' is the change in temperature then the enthalpy change is given by the [[Van </del>'t <del style="font-weight: bold; text-decoration: none;">Hoff equation|Van't Hoff equation]]:</del></div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div> </div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><del style="font-weight: bold; text-decoration: none;">:</del><<del style="font-weight: bold; text-decoration: none;">math</del>> <del style="font-weight: bold; text-decoration: none;"> {\Delta H^o} = {RT^2}.\frac{d \ln K}{dT} </del><<del style="font-weight: bold; text-decoration: none;">/math</del>></div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div> </div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><del style="font-weight: bold; text-decoration: none;">where ''R'' is the [[Gas constant|universal gas constant]] and ''T'' is the [[Thermodynamic temperature|absolute temperature]]. When a single step in a reaction is perturbed in a temperature jump experiment, the reaction follows a single [[exponential decay]] function with the reciprocal [[time constant]] </del>(<del style="font-weight: bold; text-decoration: none;">1/τ) equal to the sum of the forward and reverse intrinsic rate constants. In more complex reaction networks, when multiple reaction steps are perturbed, then the reciprocal time constants are given by the </del>[<del style="font-weight: bold; text-decoration: none;">[eigenvalue]]s of the characteristic rate equations. The ability to observe intermediate steps in a reaction pathway is one of the attractive features of this technology.<ref>{{cite journal|last1=Urbanke|first1=C|last2=Wray|first2=J.|title=A fluorescence temperature-jump study of conformational transitions in myosin subfragment 1|journal=Biochemical Journal|year=2001|volume=358|pages=165–173|pmid=11485564|url=</del>http://<del style="font-weight: bold; text-decoration: none;">www</del>.<del style="font-weight: bold; text-decoration: none;">biochemj</del>.<del style="font-weight: bold; text-decoration: none;">org</del>/<del style="font-weight: bold; text-decoration: none;">bj</del>/<del style="font-weight: bold; text-decoration: none;">358/0165/3580165.pdf|issue=Pt 1|pmc=1222044}}</ref></del></div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div> </div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><del style="font-weight: bold; text-decoration: none;">==References==</del></div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><del style="font-weight: bold; text-decoration: none;">{{reflist}}</del></div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div> </div></td><td colspan="2" class="diff-side-added"></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><del style="font-weight: bold; text-decoration: none;">[[Category:Chemical kinetics]</del>]</div></td><td colspan="2" class="diff-side-added"></td></tr>
</table>en>JMP EAXhttps://en.formulasearchengine.com/index.php?title=Inverse_relation&diff=12707&oldid=preven>Spiffy sperry: /* See also */ remove item that redirects to this article2013-10-16T17:06:28Z<p><span class="autocomment">See also: </span> remove item that redirects to this article</p>
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<td colspan="2" style="background-color: #fff; color: #202122; text-align: center;">Revision as of 19:06, 16 October 2013</td>
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<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><del style="font-weight: bold; text-decoration: none;">Alyson Meagher </del>is the <del style="font-weight: bold; text-decoration: none;">name her parents gave her but she doesn't like when people use her full name</del>. <del style="font-weight: bold; text-decoration: none;">To climb </del>is <del style="font-weight: bold; text-decoration: none;">some thing I really appreciate performing</del>. <del style="font-weight: bold; text-decoration: none;">Invoicing </del>is <del style="font-weight: bold; text-decoration: none;">what I do for </del>a <del style="font-weight: bold; text-decoration: none;">living but I've always needed my personal business</del>. <del style="font-weight: bold; text-decoration: none;">Mississippi is </del>the <del style="font-weight: bold; text-decoration: none;">only location I've been residing </del>in <del style="font-weight: bold; text-decoration: none;">but I will have </del>to <del style="font-weight: bold; text-decoration: none;">move </del>in a <del style="font-weight: bold; text-decoration: none;">yr or two</del>.<<del style="font-weight: bold; text-decoration: none;">br</del>><<del style="font-weight: bold; text-decoration: none;">br</del>><del style="font-weight: bold; text-decoration: none;">Here </del>is <del style="font-weight: bold; text-decoration: none;">my weblog </del>... <del style="font-weight: bold; text-decoration: none;">[</del>http://<del style="font-weight: bold; text-decoration: none;">brazil</del>.<del style="font-weight: bold; text-decoration: none;">amor-amore</del>.<del style="font-weight: bold; text-decoration: none;">com</del>/<del style="font-weight: bold; text-decoration: none;">irboothe online psychic reading</del>]</div></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><ins style="font-weight: bold; text-decoration: none;">'''Temperature jump''' is a technique used in the study of [[chemical kinetics]]. It usually involves the discharging of a capacitor (in the kV range) through a small volume (<mL) of a conducting solution containing the molecule/reaction to be studied. In some versions of the apparatus used, the solution </ins>is <ins style="font-weight: bold; text-decoration: none;">heated instead by </ins>the <ins style="font-weight: bold; text-decoration: none;">output of a pulsed laser which emits in the near infra-red</ins>. <ins style="font-weight: bold; text-decoration: none;">When laser heating </ins>is <ins style="font-weight: bold; text-decoration: none;">employed, the solution need not be conducting</ins>. <ins style="font-weight: bold; text-decoration: none;">In both cases, the temperature of the solution </ins>is <ins style="font-weight: bold; text-decoration: none;">caused to rise by </ins>a <ins style="font-weight: bold; text-decoration: none;">small amount in microseconds (or less in the case of laser heating)</ins>. <ins style="font-weight: bold; text-decoration: none;">This allows the study of </ins>the <ins style="font-weight: bold; text-decoration: none;">shift in equilibrium of reactions that equilibrate </ins>in <ins style="font-weight: bold; text-decoration: none;">milliseconds (or microseconds with laser temperature jump), these changes most commonly being observed using [[absorption spectroscopy]] or [[fluorescence spectroscopy]]. Due to the small volumes involved the temperature of the solution returns </ins>to <ins style="font-weight: bold; text-decoration: none;">that of its surroundings </ins>in <ins style="font-weight: bold; text-decoration: none;">minutes.<ref>{{cite book|title=Handbook of biochemical kinetics|author=Daniel L. Purich, R. Donald Allison|year= 1999|publisher=Academic Press|isbn=0-12-568048-1}}</ref></ins></div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div> </div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><ins style="font-weight: bold; text-decoration: none;">The fractional extent of the reaction (''i.e.'' the percentage change in concentration of </ins>a <ins style="font-weight: bold; text-decoration: none;">measurable species) depends on the molar enthalpy change (Δ''H''°) between the reactants and products and the equilibrium position</ins>. <ins style="font-weight: bold; text-decoration: none;"> If ''K'' is the equilibrium constant and ''dT'' is the change in temperature then the enthalpy change is given by the [[Van 't Hoff equation|Van't Hoff equation]]:</ins></div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div> </div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><ins style="font-weight: bold; text-decoration: none;">:</ins><<ins style="font-weight: bold; text-decoration: none;">math</ins>> <ins style="font-weight: bold; text-decoration: none;"> {\Delta H^o} = {RT^2}.\frac{d \ln K}{dT} </ins><<ins style="font-weight: bold; text-decoration: none;">/math</ins>></div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div> </div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><ins style="font-weight: bold; text-decoration: none;">where ''R'' is the [[Gas constant|universal gas constant]] and ''T'' </ins>is <ins style="font-weight: bold; text-decoration: none;">the [[Thermodynamic temperature|absolute temperature]]</ins>. <ins style="font-weight: bold; text-decoration: none;"> When a single step in a reaction is perturbed in a temperature jump experiment, the reaction follows a single [[exponential decay]] function with the reciprocal [[time constant]] (1/τ) equal to the sum of the forward and reverse intrinsic rate constants</ins>. <ins style="font-weight: bold; text-decoration: none;"> In more complex reaction networks, when multiple reaction steps are perturbed, then the reciprocal time constants are given by the [[eigenvalue]]s of the characteristic rate equations</ins>. <ins style="font-weight: bold; text-decoration: none;"> The ability to observe intermediate steps in a reaction pathway is one of the attractive features of this technology.<ref>{{cite journal|last1=Urbanke|first1=C|last2=Wray|first2=J.|title=A fluorescence temperature-jump study of conformational transitions in myosin subfragment 1|journal=Biochemical Journal|year=2001|volume=358|pages=165–173|pmid=11485564|url=</ins>http://<ins style="font-weight: bold; text-decoration: none;">www</ins>.<ins style="font-weight: bold; text-decoration: none;">biochemj.org/bj/358/0165/3580165</ins>.<ins style="font-weight: bold; text-decoration: none;">pdf|issue=Pt 1|pmc=1222044}}<</ins>/<ins style="font-weight: bold; text-decoration: none;">ref></ins></div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div> </div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><ins style="font-weight: bold; text-decoration: none;">==References==</ins></div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><ins style="font-weight: bold; text-decoration: none;">{{reflist}}</ins></div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div> </div></td></tr>
<tr><td colspan="2" class="diff-side-deleted"></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><ins style="font-weight: bold; text-decoration: none;">[[Category:Chemical kinetics]</ins>]</div></td></tr>
</table>en>Spiffy sperryhttps://en.formulasearchengine.com/index.php?title=Inverse_relation&diff=246458&oldid=preven>David Eppstein: /* See also */ Transpose graph2012-09-01T04:09:18Z<p><span class="autocomment">See also: </span> <a href="/index.php?title=Transpose_graph&action=edit&redlink=1" class="new" title="Transpose graph (page does not exist)">Transpose graph</a></p>
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