Nitrogen dioxide reacts with water to produce oxygen and ammonia. a 5.00 L sampl

Question

Nitrogen dioxide reacts with water to produce oxygen and ammonia. a 5.00 L sample of H2O (g) reacts at a temperature of 375 degrees Celsius and a pressure of 722 mmHg.
Hiw many grams of NH3 can be produced? 4NO2 (g) + 6H2O (g) ---> 7O2 (g) + 4NH3 (g) Nitrogen dioxide reacts with water to produce oxygen and ammonia. A 5.00 L sample of H2O(g) reacts at a temperature of 375 C and a pressure of 722 mmHg Part A How many grams of NH, can be produced? 4NO2(9)+6HO)702(9) +4NH(9) Express your answer with the appropriate units. m= Value Units Submit My Answers Give Up

Explanation / Answer

moles of H2O at 375 deg.c and 722 mmg Hg

T= 375+273.15K=648.15, P= 722/760 atm =0.95 atm V= 5 L

from PV= nRT, n= PV/RT, R=0.0812atm.L/mole.K

n= number of moles of water= 0.95*5/(0.0821*648.15)=0.089 moles

as per the reaction 4NO2+6H2O----------> 7O2 +4NH3, 6 moles of Water gives 4 moles of NH3

0.089 moles of Water gives 0.089*4/6=0.059333

molecular weight of NH3= 17, mass of NH3= moles* Molecular weight= 0.059333*17=1.008 gms

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