Suppose that 3.00 mol of NO(g) is introduced into a 1.00L flask. When the system comes to equilibrium, 1.00 mol of N2O has formed .

Question

Suppose that 3.00 mol of NO(g) is introduced into a 1.00L flask. When the system comes to equilibrium, 1.00 mol of N2O has formed .

2N2O(g)+O2(g)⇌ 4NO(g)

What is the equilibrium concentration of NO(g). 

a)1.00 mol/L

b)2.00 mol/L

c)4.00 mol/L

d)0.5 mol/L

e) none of these

Answer 1

The molar ratio of N₂O is 2:4 (or 1:2). Since we started with 3.00 mol of NO and know that there is 1.oo mol N₂O at equilibrium, then the NO must have decrease by 2 times gain of N₂O. Therefore, the N₂O has decreased by 2.00 moles. We started with 3.00 mole, so losing 2 we are left with 1.00 mole of N₂O per liter.