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The reaction stays the same and does not favor a side because if you double each of the two reactants it is the same as quadrupling the concentration of reactants so if you quadruple the concentration of the products, there is an equivalent increase on both side resulting is no change in equilibrium.
If the reaction would move from left to right if you double one side and quadruple the other. You just have to think about the reaction as a scale with products on one side and reactants on the other. This scale wants to be in balance and for that to happen you must move something from the lower side (products in this case) to the higher side of the scale (reactants). Also, according to Le Chatelier's Principle: "states that when a system experiences a disturbance (such as concentration, temperature, or pressure changes), it will respond to restore a new equilibrium state" and in this case you're raising the concentration of the two sides unevenly so there would be movement from right to left to attain equilibrium again.
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