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? . ? 1 CMY SCF Home: State College | () MyLab and Mastering Course Ho CHM1025C Introductory Chemistry -Jie Sun MasteringChemistry: Chp. 11 Gases- Internet Explorer https/session masteringchemisty.com/myct/itemView?assignmentProblemiD-94798445 KChp. 11 Gases ± The Ideal Gas Law and Stoichiormetry K10 of 31 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 722 mmHg and 35 oC is required to synthesize 13 0 mol of NO? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) NH3(g)+?02(g)-+?NO(g)+?H20(g) volume of O2 = Value Units Submit Part B This question will be shown after you complete previous question(s) Next > Provide Feebback

Explanation / Answer

Exercise 11.53

Part -A

Use the combined gas law

P1 V1 / T1 = P2 V2 / T2

( 1.0 atm) ( 2.3 L) / ( 306 K) = ( 4.0 atm) V2 / 289 K

V2 = ( 1.0 atm)(2.3 L)(289 K ) / ( 4.0 atm ) ( 306 K)

V = 0.54 L

Part - A

The balanced equation is

4NH3(g) + 5O2(g) = 4NO(g) + 6H2O(g)

You required 13.0 mol of NO

( 5 / 4 ) * 13.0= 16.25 mol of O2

Convert 35°c = 35+273 = 308 K

Using ideal gas law PV = nRT

V = nRT/P

V = 16.25 * 62.364 * 308 / 722

V = 432.3 Liters

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