File:Table22-1.jpg
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| Description |
English: Table 22-1 from Chapter 22: Rates and Mechanics of Chemical Reactions
Textbook title: Chemical Principles |
| Date | |
| Source | Adapted from http://caltechbook.library.caltech.edu/178/23/Chapter_22.pdf |
| Author | Dickerson, Richard E. and Gray, Harry B. and Haight, Gilbert P |
| Permission (Reusing this file) |
Used by permission of Harry B. Gray |
| Other versions |
{| class="wikitable" style="float:right; margin: 0em 0em 1em 1em; text-align:center; <!--
--> border-collapse: collapse; border-width: 0px;"
|+
! scope="col" style="background: #ccf;" colspan="6" | <!--
--> Decomposition of [N<sub>2</sub>O<sub>2</sub>] in CCl<sub>4</sub><!--
--> Solution at 45°C<sup>''a'',''b''</sup><br/><!--
--> [N<sub>2</sub>O<sub>2</sub>] → 2 NO<sub>2</sub> + ½ O<sub>2</sub>(''g'')
|-
! scope="col" style="background: #ccf; width: 6em;" | <!--
--> Time t (sec)
! scope="col" style="background: #ccf; width: 9em;" | <!--
--> [N<sub>2</sub>O<sub>2</sub>] (mol liter<sup>−1</sup>)
! scope="col" style="background: #ccf; width: 6em;" | <!--
--> Δ[N<sub>2</sub>O<sub>2</sub>]
! scope="col" style="background: #ccf; width: 6em;" | <!--
--> Δt
! scope="col" style="background: #ccf; width: 15em;" | <!--
--> −Δ[N<sub>2</sub>O<sub>2</sub>]/Δt (mol liter<sup>−1</sup> sec<sup>−1</sup>)
! scope="col" style="background: #ccf; width: 15em;" | <!--
--> k=(1/[N<sub>2</sub>O<sub>2</sub>])×(−Δ[N<sub>2</sub>O<sub>2</sub>]/Δt)
|-
| 0 || 2.33 || − || − || − || −
|-
| 184 || 2.08 || −0.25 || 184 || 1.36 × 10<sup>−3</sup> || 6.2 × 10<sup>−4</sup>
|-
| 319 || 1.91 || −0.17 || 135 || 1.26 × 10<sup>−3</sup> || 6.3 × 10<sup>−4</sup>
|-
| 526 || 1.67 || −0.24 || 207 || 1.16 × 10<sup>−3</sup> || 6.5 × 10<sup>−4</sup>
|-
| 867 || 1.35 || −0.32 || 341 || 0.94 × 10<sup>−3</sup> || 6.2 × 10<sup>−4</sup>
|-
| 1198 || 1.11 || −0.24 || 331 || 0.72 × 10<sup>−3</sup> || 5.9 × 10<sup>−4</sup>
|-
| 1877 || 0.72 || −0.39 || 679 || 0.57 × 10<sup>−3</sup> || 6.2 × 10<sup>−4</sup>
|-
| colspan="6" style="border-width: 0px; text-align:left;" | <!--
--> <sup>''a''</sup> From H. Eyring and F. Daniels. ''J. Am. Chem. Soc.'' '''52''', 1472 (1930).<br /><!--
--> <sup>''b''</sup> In the last column, [N<sub>2</sub>O<sub>2</sub>]=average of <!--
--> concentrations at beginning and end of this time interval. For the first entry,<!--
--> [N<sub>2</sub>O<sub>2</sub>]=(2.33+2.08)/2
|} |
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| current | 14:30, 23 April 2009 | | 1,081 × 331 (99 KB) | Zatore (talk | contribs) | {{Information |Description={{en|1=Table 22-1 from Chapter 22: Rates and Mechanics of Chemical Reactions Textbook title: Chemical Principles}} |Source=Adapted from http://caltechbook.library.caltech.edu/178/23/Chapter_22.pdf |Author=Dickerson, Richard E. a |
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