Hi, can someone please show me how to solve this problem, Iforgot how to approac

Question

Hi, can someone please show me how to solve this problem, Iforgot how to approach it correctly. An 11L vessel contains 2.0 mols H2 and 1.0 molN2 at 298.15 K initially. H2 reacts withN2 to form NH3 . Calculate the partialpressure and the total pressure of the final mixture. Thanks for your help!! Hi, can someone please show me how to solve this problem, Iforgot how to approach it correctly. An 11L vessel contains 2.0 mols H2 and 1.0 molN2 at 298.15 K initially. H2 reacts withN2 to form NH3 . Calculate the partialpressure and the total pressure of the final mixture. Thanks for your help!!

Explanation / Answer

So you gotta start off with the equation of the reaction andfinding out how much gas is at the end 3H2 + N2 --> 2NH3 2mol H2 x ( 2mol NH3 / 3 mol H2) = 4/3 mol NH3 - This is the total amount of NH3 produced through thisreaction. Now you must check to see if all the N2 was used orif it was the limiting reagent 4/3 mol NH3 x ( 1 mol N2 / 2molNH3) = 2/3 mol N2 - This shows that only2/3 mol N2 reacted with the H2 gas to producethe NH3. Therefore 1/3 mol N2 gasremains in the vessel with the NH3. So to find the total pressure of the system: PV = nRT -where n = total number of moles = 4/3 + 1/3 = 5/3 mol P(11L) = (5/3mol)(0.0821 Latm/molK)(298.15 K) PTotal = 3.71 atm find partial pressures take mole ratios: PNH3 = (4/3)/(5/3) x 3.71atm = 2.97 atm PN2 = (1/3)/(5/3) x 3.71atm = 0.74 just did a problem like this for a test i just took recently sohopefully it all seems clear :)

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