**Unformatted text preview: **. The algebra of this was covered in a previous file. The two key working equations are: R S RT H K ∆ + ∆-= ln and -∆ = 1 2 2 1 1 1 ln T T R H K K or -∆ =-1 2 2 1 1 1 ln ln T T R H K K The number crunching is not particularly taxing. One should discover (confirm this for practice) that: K 273 = 75.1 and K 298 = 8.8 and K 373 = 0.079 Note that as the temperature increases, K decreases and the equilibrium shifts left (favors ‘the stuff of the left’) favoring the NO 2 . Since the NO 2 is colored, an increase in temperature should deepen the color of the mixture of gases; conversely, a decrease in temperature should tend towards less color....

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- Fall '07
- Warren
- Chemistry, Thermodynamics, Equilibrium, Chemical reaction, temperature increases