Question

9780968206904

consider the equilibrium: 21018) 12(8) + Cl2 (s) keq" 10.0 moles of ICI were placed in a 5.0 L container at 10 °C and if an equilibrium concentration of 12 was found to be 0.60 M, calculate the number of moles ICI initially present. 8. A student places 2.00 moles SO3 in a 1.00 L flask. At equilibrium (O2) = 0.10 M at 130 °C. Calculate the Keq. 2SO2(g) + O2(g)>2503(8)

please help me with the question 7 and 8。

Answer 1

Sol 7.

2ICl(g) <----> I2(g) + Cl2(g)

As Equilibrium Concentration of I2 = [I2] = 0.60 M

So , Equilibrium Concentration of Cl2

= [Cl2] = [I2] = 0.60 M

As Keq  = [I2] [Cl2] / [ICl]²  

So , 10 = (0.60)² / [ICl]²

Equilibrium Conc. of ICl = [ICl] = 0.1897 M

Now , Initial Conc. of ICl  

= Equilibrium Conc. of ICl + 2 × Equilibrium Conc. of I2

= 0.1897 + 2 × 0.60

= 1.3897 M

As Volume of container = 5 L

So , Initial Moles of ICl = x

= Initial Conc. of ICl × Volume of container

= 1.3897 × 5

=   6.9485 mol