Correct Answer - Option 1 : K
p = K
c (RT)
-2
Concept:
Haber's process:
- This process is used in large scale preparations of ammonia.
N2 + 3H2 → 2NH3
- During the process, nitrogen and hydrogen are used in the ratio 1:3.
- The process is exothermic ΔH = -ve in nature means heat is produced in the process.
- According to the Le-chateliar principle, the temperature is kept high to speed up the process.
- The gaseous ammonia produced is converted to liquid ammonia to remove the products formed.
- This drives the reaction forward.
Equilibrium Constants:
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The constants Kp and Kc are both equilibrium constants.
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Kp is used when the concentration terms are given in partial pressures i.e, in gaseous reactions.
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Kc is used when the reaction terms are expressed in molarities.
- The relation between Kp and Kc is given by:
\({K_p} = {K_c} \times {\left( {RT} \right)^{\Delta n}}\) where R = Universal gas constant, T = Temperature, and \(\triangle n\) = change in moles of gases in the reaction.
Calculation:
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The relation between Kp and Kc is
\({K_p} = {K_c} \times {\left( {RT} \right)^{\Delta n}}\)
For the reaction
N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g)
\(No.\;of\;moles\;of\;products = 2\)
\(No.\;of\;moles\;of\;reactants = 3 + 1 = 4\)
\(Change\;in\;number\;of\;moles\;of\;gases = {n_{products}} - {n_{reactants}} = \;\Delta n\)
\( = 2 - 4 = - 2\)
Hence,
\({K_p} = {K_c} \times {\left( {RT} \right)^{-2}}\)
Hence, or the reaction N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g) ΔH = -ve, \({K_p} = {K_c} \times {\left( {RT} \right)^{-2}}\)