Question

Part B N (9) + 3 H, (g) = 2 NH3(g) Kp = 6.2 x 10(at 298 K) Express your answer to two significant figures. View Available Hint(s) V AC O ? Submit Part N2 (9) + O2(g) + 2NO(9) K = 4.10 x 10-1 (at 298 K) Express your answer to three significant figures. View Available Hint(s) 10 AED + Om ? Submit Q Search or type URL C 5 6 7 8 9 0

Answer 1

K_p is the equilibrium constant in terms of partial pressure of the components. K_c is the equilibrium constant in terms of molar concentration of the components.

The relation between K_p and  K_c is given by the relation -

Ke= K (RT)-In

where $\Delta n$ = (number of moles of gaseous products) - (number of moles of gaseous reactants)

R = universal gas constant = 0.0821 L atm K^-1 mol^-1

(this value of R is taken as the concentration is taken in mol L^-1)

T = temperature of the system

Part B

N2(g) + 3H2(g) + 2NH3(9

All the components are gaseous.

$\Delta n$ = 2-(3+1) = -2

T = 298 K

K_p = 6.2 * 10⁵

Ke= K (RT)-In

= 6.2 x 105 (0.0821 x 298)-(-2)

= 6.2 x 10(0.0821 x 298)

= 3.7 * 10⁸(rounding off to 2 significant figure)

Part C

N2(g) + O2(g) + 2NO(9)

All the components are gaseous.

$\Delta n$ = 2-(1+1) = 0

T = 298 K

K_p = 4.10 * 10^-31​​​​​

Ke= K (RT)-In

= 4.10 x 10-31 (0.0821 x 298)

= 4.10 * 10^-31​​​​​ (rounding off to 3 significant figure) [Since a⁰ = 1]