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11 Nov 2019
Nitrous oxide, N2O, undergoes decomposition on a gold surface at 900 °C, obeying the following stoichiometry: 2 N2O (g) --> 2 N2(g) +O2 (g)
The concentration of the reactant was monitored as a function of time. A graph of ln(N2O) vs. t gave a graph simlilar to the one in the lab manual. The trendline is Y= -0.01255 X + -2.867, with a y axis of ln(N2O) and x of time. The correlation coefficient r is -0.9994, for a nearly perfect anticorrelation.
What is the half-life for a first order reaction with k = -0.1783 1/min? t1/2=
Nitrous oxide, N2O, undergoes decomposition on a gold surface at 900 °C, obeying the following stoichiometry: 2 N2O (g) --> 2 N2(g) +O2 (g)
The concentration of the reactant was monitored as a function of time. A graph of ln(N2O) vs. t gave a graph simlilar to the one in the lab manual. The trendline is Y= -0.01255 X + -2.867, with a y axis of ln(N2O) and x of time. The correlation coefficient r is -0.9994, for a nearly perfect anticorrelation.
What is the half-life for a first order reaction with k = -0.1783 1/min? t1/2=
Irving HeathcoteLv2
8 Apr 2019
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