PART B ONLY< The Ideal Gas Law and Stoichiometry The industrial production of nitric acid (HNO3) is...

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PART B ONLY<
The Ideal Gas Law and Stoichiometry The industrial production ofnitric acid (HNO3) is a multistep process. The first step is theoxidation of ammonia (NH3) over a catalyst with excess oxygen (O2)to produce nitrogen monoxide (NO) gas as shown by the unbalancedequation given here: ?NH3(g)+?O2(g)â†’?NO(g)+?H2O(g)
Part A What volume of O2 at 912 mmHg and 33 âˆ˜C is required tosynthesize 16.0 mol of NO?
volume of O2 = 419 L
Part B
What volume of H2O(g) is produced by the reaction underthe same conditions? Express your answer to three significantfigures and include the appropriate units. volume of H2O=

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4.2 Ratings (664 Votes)

Balance the equation 4 NH3 g 5 O2 g 4 NO g 6 H2O g A As per the balanced stoichiometric equation the molar ratios of O2 and NO is 54 ie 5 moles of O2 are required to synthesize 4 moles of NO We need to find out the moles of O2 required from the given data by using the ideal gas law See Answer

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