Answer:
The reaction occurring in the forward direction is favored.
Explanation:
Consider the reversible reaction
A+B ----------------->. C
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It can easily be seen that the equilibrium position lies more to the product side than the reactants side( the longer arrow points towards the products while the sorter one points towards reactants). That is, the forward reaction (product formation) is favoured under a given set of conditions. Hence there will be more products in the reaction system than reactants.
