Posted by **Joe** on Saturday, December 1, 2012 at 1:13am.

Dimethylamine burns in oxygen according to the following equation:

4 C2H7N + 15 O2 → 8 CO2 + 14 H2O + 2 N2

(a) How many liters of O2 at 35 °C and 0.840 atm will be needed to burn 7.70 L of C2H7N at 35 °C

and 0.840 atm?

(b) How many liters of CO2 at 35 °C and 0.840 atm will be produced?

Report your answers to parts (a) and (b) to 3 significant figures

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