± The Ideal Gas Law and Stoichiometry Part A The industrial production of nitric
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± The Ideal Gas Law and Stoichiometry Part A 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 (02) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here What volume of O2 at 760. mmHg and 37 °C is required to synthesize 22.0 mol of NO? Express your answer to three significant figures and include the appropriate units Hints ?NH3 (g)+7O3 (g)-?NO(g) +7H20(g) volume of o 839.883 L Submit My Answers Give Up ncorrect, Try Again; 2 attempts remainingExplanation / Answer
The balanced reaction is 4NH3 (g) + 5O2(g) ---> 4NO(g) + 6H2O(g)
4 moles of NO synthesized from 5 moles of O2
22.0 moles of NO synthesized from (22.0x5)/4 = 27.5 moles of O2
Calculation of volume of Oxygen :
We know that ideal gas equation is PV = nRT
Where
T = Temperature = 37 oC = 37+273 = 310 K
P = pressure = 760 mm Hg = 1atm
n = No . of moles = 27.5 mol
R = gas constant = 0.0821 L atm / mol - K
V= Volume of the gas = ?
Plug the values we get V = (nRT) / P
= 700 L
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