Chemical EquilibriumHard

Question

The equilibrium constant for the reaction N2(g) + O2(g) $\rightleftharpoons$2NO(g) is 0.09 at 3500 K. The fraction of equimolar mixture of N2 and O2 converted into NO is

Options

A.0.13
B.0.23
C.0.30
D.0.357

Solution

N2 + O2 $\rightleftharpoons$ 2NO

Equilibrium moles 1 – x 1 – x 2x

$0.09 = \frac{(2x)^{2}}{(1 - x)(1 - x)} \Rightarrow x = 0.13$

Create a free account to view solution

View Solution Free
Topic: Chemical Equilibrium·Practice all Chemical Equilibrium questions

More Chemical Equilibrium Questions

The thermal dissociation equilibrium of CaCO3(s) is studied under different conditions.CaCO3(s) ⇋ CaO(s) + CO2(g)F...In the equilibrium mixture H2(g) + I2(g) $\rightleftharpoons$2HI(g), the mole ratio of gases are $\sqrt{2}:\sqrt{2}:10$,...NH4HS(S) ⇋ NH3(g) + H2S(g)The equilibrium pressure at 25oC is 0.660 atm. What is KP for the reaction....When alcohol (C2H5OH (l)) and acetic acid (CH3COOH (l)) are mixed together in equimolar ratio at 27oC , 33% of each is c...Consider the following reversible reactions (at 298 K) :(a) N2O4 ⇋ 2NO2 (b) 2SO2 + O2 ⇋ 2SO3 (c) 2HI ⇋...