Copper metal reacts exothermically with 8 mol dm–3 nitric acid to produce nitrogen monoxide, according to the equation:

Question

Copper metal reacts exothermically with 8 mol dm–3 nitric acid to produce nitrogen monoxide, according to the equation:

Cu(s) + 8HNO3(aq)
 3Cu(NO3)2(aq) + 4H2O(l) + 2NO(g)
Which of the following measures would force the equilibrium position to the right?
a Use more concentrated acid.
b Use a catalyst.
c Heat the mixture.
d Remove NO as it is formed
pick one option explain why in one setnece

Answer 1

d. Remove NO as it is formed.

By removing NO as it is formed, the equilibrium is shifted to the right because Le Chatelier's principle states that if a product is removed from the reaction mixture, the equilibrium will shift in the direction that generates more of that product in order to restore equilibrium.

Answer 2

The option that would force the equilibrium position to the right is d) Remove NO as it is formed because according to Le Chatelier's principle, removing a product from a reaction mixture will shift the equilibrium towards the product side to compensate for the loss.

Answer 3

d) Removing NO as it is formed. This would shift the equilibrium position to the right because according to Le Chatelier's principle, when a product is removed from the reaction, the equilibrium shifts in the direction that produces more of the removed substance.