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.

stupid i wont let you get a chance

explanation:

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: