Consider the following reaction at equilibrium. what effect will increasing the temperature have on the system? fe3o4(s) + co(g) ↔ 3 feo(s) + co2(g) δh°= +35.9 kjthe equilibrium constant will decrease. no effect will be observed. the reaction will shift to the right in the direction of products. the equilibrium constant will increase. the reaction will shift to the left in the direction of reactants

The reaction will shift to the right in the direction of products.

Explanation:

According to Le Chatelier's Principle, the change in any state of the equilibrium say temperature, volume, pressure, or the concentration, the equilibrium will oppose these changes and will shift in such a way that the effect cause must be nullified.

For an endothermic reaction,

On increasing the temperature, reaction will go in forward direction (towards right), because according to Le Chatelier's principle as we increase the temperature,  the equilibrium is will be disturbed , so to again establish the equilibrium, the reaction will go in forward direction as it is endothermic in nature (towards right).

Thus, the of the given reaction is positive and thus, on increasing temperature, reaction will go in forward direction.

- The reaction will shift to the right in the direction of products.

answer; i believe the correct answer is (solid gold);

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !