Question

Nitrogen gas is produced by the following reaction in laboratory: NHANO2(s) - N2(9) + 2H2O(1) In one reaction, 3.4 kg of ammonium nitrite is heated at 527 °C in a 20.0-L vessel. The pressure of Ny is 0.15 bar after 7.0 minutes. x Incorrect What is the average rate of Ny production in mol/min during the 7-minute interval? 0.0061129 mol/min the tolerance is +/-2% LINK TO TEXT Incorrect How many moles of ammonium nitrite consumed in the 7-minute interval? 9.54

Answer 1

Initial moles of ammonium nitrite

moles of Ammonium nitrate = (mass /molar mass)

mass = 3.4 Kg = 3.4 $\times$ 1000 = 3400 g

molar mass = 64 g/mol

so, moles = (3400/64)

= 53.125

now , ideal gas equation is PV = nRT

R = 0.08341 L-bar /mol. K

T = 527 + 273 = 800 K

V = 20.0 L

pressure of N₂ after 7 min = 0.15 bar

so, moles of N₂ after 7 min

n = (PV)/(RT)

= ( 0.15$\times$ 20.0)/0.0831$\times$800)

= 0.045

mole ratio of NH₄NO₃ and N₂ = 1 :1

BCA table is

	moles of NH4NO3	moles of N2
before	53.125	0
change	- 0.045	+0.045
after	53.125 - 0.045 = 53.08	0.045

therefore average rate production of N₂

= - change in moles of ammonium nitrite/ time interval

= moles of N₂ formed/time interval

4 (moles of NH4 002) Almoles of N2) At At

= (0.045)/7

= 0.00642 mol/min

moles of ammonium nitrite consumed = moles of N₂ formed

= 0.045