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The equilibrium constant for the chemical equation

\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]

is \[ K_p = 0.0133 \] at 181 °C. Calculate the value of \[ K_c \] for the reaction at 181 °C.

Answer :

Answer:

Kc is 18.478

Explanation:

Here we want to calculate Kc given Kp

The equation that links both is given as follows;

Kc = Kp/(RT)^Δn

where Kp = 0.0133

R is molar gas constant = 0.0821 L.atm/mol.k

T is temperature in kelvin = 181 + 273 = 454K

Δn is the change in number of moles between products and reactants = 2-4 = -2

Substituting these values, we have;

Kc = 0.0133/(0.0821 * 454)^-2

Kc = 18.478

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Rewritten by : Barada

4.47 x 10- 4 spook/ L is the value of Kc for the response N2( g) 3H2( g) 2NH3( g) at 181 °C.

Given

the chemical equation N2(g)+3H2(g)↽−−⇀2NH3(g) is Kp=0.0133 at 181 ∘C.

To Find

the value of Kc for the reaction at 181 ∘C.

Solution

In order to determine the value of Kc for the response N2( g) 3H2( g) 2NH3( g) at 181 °C, we can use the relationship between Kp and Kc.

This equation relates Kp with Kc

Kc = Kp( RT) n

where

Partial pressures are used to express Kp, the equilibrium constant.

In molar attention, Kc represents the equilibrium constant.

The gas constant, or R, is0.08206 L atm/ K spook.

The temperature in Kelvin is T.

The stoichiometric measure n is the difference between the aggregate of the gassy products' and gassy reactants' stoichiometric portions.

Then are the data

Δn = ( 2-( 1 3)) = -2

still, we get

If we substitute the values handed.

The formula for 0.0133 is Kc(0.08206 L/ atm/ Kmol *( 181 273) K)- 2.

When we simplify and find Kc, we gain

Kc equals4.47 x 10- 4 spook/L.

thus,4.47 x 10- 4 spook/ L is the value of Kc for the response N2( g) 3H2( g) 2NH3( g) at 181 °C.

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