AP EAMCET202018 Sep 2020Evening ShiftChemistryChemical EquilibriumActual
For the reaction, ( NO ₂+ CO NO + CO ₂ ) one mole of ( NO ₂ ) and 2 moles of ( CO ) were kept in a vessel. Calculate the equilibrium constant (K_p ), if at equilibrium (25 % ) of initial amount CO is consumed.
Options
- A( 1 2 )
- B( 1 3 )
- C1
- D( 1 4 )
Correct answer
B. ( 1 3 )
Step-by-step solution
In this question, we have to assume that volume of the vessel is (1 ~L ). ( array lcccc & NO ₂(g)+ CO (g) & & NO (g)+ CO ₂(g) t=0 & 1 & 2 & 0 & 0 mole t=t_ eq & 1-0.5 & 2-0.5 & 0.5 & 0.5 & =0.5 & =1.5 & & Molar conc. ( mol L ⁻¹ ) & 0.5 1 & 0.5 1 & 0.5 1 & 0.5 1 & =0.5 & =1.5 & 0.5 & 0.5 array ) Given, ( =2 25 100 =0.5 ) ( K_C= [ NO ] [ CO ₂ ] [ NO ₂ ][ CO ] = 0.5 0.35 0.5 1.5 = 1 3 =K_p ) Because, ( n_g=( l + l )-( l + l )=0 ) ( array ll & K_p=K_C(R T)^ n_s =K_C(R T)^0=K_C & K_p= 1 3 array )