(b) In a second experiment, the nitrogen monoxide gas produced in the reaction o

Question

(b) In a second experiment, the nitrogen monoxide gas produced in the reaction occupied 638 cm2 at 101 kPa and 298 K. Calculate the amount, in moles, of NO gas produced (The gas constant R-8.31 JK'mor') (c) When lead(ll) nitrate is heated it decomposes to form lead(ll) oxide, nitrogen dioxide and oxygen 0 Balance the following equation that shows this thermal decomposition. .. . .PONOlds) PbOs) + NOdg) + 01g) () Suggest one reason why the yield of nitrogen dioxide formed during this reaction is often less than expected d for

Explanation / Answer

Apply Ideal Gas Law,

PV = nRT

where

P = absolute pressure

V = total volume of gas

n = moles of gas

T = absolute Temperature

R = ideal gas constant

V = 638 cm3 = 0.638 L

P = 101 kPa = 1 atm

T = 298K

then

n = PV/(RT)

n = (1)(0.638)/(0.082*298)

n = 0.0261 mol of NO are produced

c)

balance reaction

Pb(NO3)2 --> PbO(s) + NO2(g) + O2(g)

balance Pb, then N, then O

Pb(NO3)2 --> PbO(s) + 2NO2(g) + O2(g)

Pb(NO3)2 --> PbO(s) + 2NO2(g) + 1/2O2(g)

ii)

not allt Pb(NO3)2 is forming PbO, and some remains, therefore not enough NO2 is obtained

Related Questions

Navigate

• Browse (All)
• Browse #
• Subjects

---

---

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