Not yet answered Points out of 1.00 P Flag question You wish to monitor the prog

Question

Not yet answered Points out of 1.00 P Flag question You wish to monitor the progress of a reaction using pressures. Suppose 16.71 gN2 (28.02 g/mol) and 1.290 g H2 (2.016 g/mol) are initially present in a 23.0 L reaction vessel at 112°C. Nitrogen and hydrogen can react to form ammonia (17.04 g/mol) according to the reaction shown. At a given point, the total pressure (the sum of the pressures of N2, H2, and NH3 present) is 1.18 atm. What percentage of the initial N2 has reacted? (%) N2(g) + 3 H2(g) 2 NH3(g) Answer Previous page Next page

Explanation / Answer

total no of mol of mixture = PV/RT

        = (1.18*23.0)/(0.0821*(112+273.15))

        = 0.858 mol

after the reaction

total no of mol of mixture = ((16.71/28)-x)+((1.29/2)-3x)+(2x) = 0.858

x = 0.192

no of mol of N2 reacted = (16.71/28)-x

             = (16.71/28)-0.192

       = 0.405 mol

no of mol of N2 taken initially = 16.71/28 = 0.6 mol

percentage of N2 reacted = 0.405/0.6*100

    = 67.8%

Related Questions

Navigate

• Browse (All)
• Browse N
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.