what volume of O2 at 798 mmHg and 41 degrees C is required to synthesize 23.0 mol of NO? (b) what volume of H2O (g) is produced by the reaction under the same conditions?

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The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here:

?NH3(g)+?O2(g)→?NO(g)+?H2O(g)

 

(a) what volume of O2 at 798 mmHg and 41 degrees C is required to synthesize 23.0 mol of NO?

(b) what volume of H2O (g) is produced by the reaction under the same conditions?

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