The industrial production of nitric acid (HNO3) is a multistep process. The firs
ID: 587143 • Letter: T
Question
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)
Part A
What volume of O2 at 836 mmHg and 27 C is required to synthesize 10.5 mol of NO?
Express your answer to three significant figures and include the appropriate units.
Part B
What volume of H2O(g) is produced by the reaction under the same conditions?
Express your answer to three significant figures and include the appropriate units
Explanation / Answer
Balance
NH3 + O2 = NO + H2O
4NH3 + 5O2 = 4NO + 6H2O
A)
4 mol of NO requires 5 mol of O2
10.5 --> 5/4*10.5 = 13.125 mol of O2 required
PV = nRT
V = nRT/P = (13.125)(62.4)(27+273)/(836) = 293.899 L = 294 L
B)
if 10.5 mol of NO produced --> 6/4 ratio --> 6/4*293.899 = 440.848 mol of H2O
V --> 6/4*293.899 = 440.84 L = 4.40*10^2 L
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