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4 years ago
Given: N2(g) + 3H2(g)  arrows both directions 2NH3(g)
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wrote...
4 years ago
The rate of the forward reaction would slow, and the backwards reaction would increase.
This is because the equlibrium will shift to minimise the change, hence, the reaction will try to produce more N2.

You could also talk about how there would be less successful collisions between N2 and H2 molecules so less product will be able to be produced as a result.
wrote...
4 years ago
It will increase the rate of forwared rxn because a removal of N will shift the equilibrium position to the left.
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