Question

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26. Consider the following system at equilibrium: N2(g) + 3H2(g) = 2NH3(g) + 92.94 kJ Which of the following changes will shift the equilibrium to the right? I. increasing the temperature II. decreasing the temperature III. increasing the volume decreasing the volume V. removing some NH3 adding some NH3 VII. removing some N2 VIII. adding some N2 IV. VI.

Answer 1

The enthapy of reaction is positive so it is an endothermic process.

1. If we increase temperature in endothermic reaction , the Equilibrium shift to the right. In case of exothermic reaction the Equilibrium shift left because in exothermic reaction heat is the product of the reaction.
2. Decreasing the temperature in endothermic reaction shift the Equilibrium left.
3. Increasing volume shift the reaction in the direction where more number of moles formed. So equilibrium shift to the left.
4. Decrease the volume shift equilibrium to the right as lesser number of moles formed.
5. Decreasing the concentration of reactant shift the Equilibrium backward. So decreasing some NH3 shift Equilibrium left.
6. Adding some NH​​​​​3 shift Equilibrium right. As according to collision theory number of effective collision increases and more product formed.
7. Removing N​​​​​​2 shift Equilibrium left , because concentration of reactant decrease.
8. Adding N​​​​​​2, shift Equilibrium right. Greater the concentration of reactant more will be the effective collision between reactant molecules greater the moles of product formed.

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