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The reaction 2N2O5 ? 2N2O4 + O2 obeys the rate law:
rate = k[N2O5], in which the rate constant is 0.00757 s-1, at acertain temperature. If 3.09 moles of N2O5 was placed in a5.00-liter container at this temperature, how many moles of N2O5would remain after 0.52 minute and How long would it take for 72.0%of the original N2O5 to react?
The reaction 2N2O5 ? 2N2O4 + O2 obeys the rate law:
rate = k[N2O5], in which the rate constant is 0.00757 s-1, at acertain temperature. If 3.09 moles of N2O5 was placed in a5.00-liter container at this temperature, how many moles of N2O5would remain after 0.52 minute and How long would it take for 72.0%of the original N2O5 to react?
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Patrina SchowalterLv2
1 Mar 2019
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4 NO2(g) + O2(g), at 70 °C is 6.82 ×10-3 s-1. Suppose we start with 0.0250 mol of N2O5(g) in a volume of 2.0 L. (a) How many moles of N2O5 will remain after 5.0 min? (b) How many minutes will it take for the quantity of N2O5 to drop to 0.010 mol? (c) What is the half-life of N2O5 at 70 °C?