Part A A mixture of helium, nitrogen, and oxygen has a total pressure of 756 mmH

Question

Part A A mixture of helium, nitrogen, and oxygen has a total pressure of 756 mmHg . The partial pressures of helium and nitrogen are 224 mmHg and 197 mmHg , respectively. What is the partial pressure of oxygen in the mixture?

Part B 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) What volume of O2 at 760. mmHg and 35 C is required to synthesize 13.5 mol of NO? Express your answer to three significant figures and include the appropriate units.

Explanation / Answer

part-A

PT   = 756mmHg

PHe   = 224mmHg

PN2   = 197mmHg

P   = PHe + PN2 + PO2

756   = 224 + 197 + PO2

PO2   = 335mmHg

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

4 mole of NO produced from 5 moles of O2

13.5 moles of NO produced from = 5*13.5/4   = 16.875 moles of O2

PV = nRT

n = 16.875 moles

T = 350C = 35 + 273 = 308K

P   = 760mmHg = 1atm

V = nRT/P

    = 16.875*0.0821*308/1 = 426.7L >>>>>answer

voluyme of O2 = 427L

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