predict the changes in equilibrium position for this reaction when the following changes are made. in each...?

1.
2A(g) + B(g) ⇌ 4C(g) + heat

In the equation, there are 3 moles of gaseous molecules on the left, while there are 4 moles of gaseous molecules on the right. There are more gaseous molecules on the right.

When pressure increases, according to Le Chatelier’s principle, the equilibrium position will shift to the left in order to decrease the number of gaseous molecules.


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2.
2A(g) + B(g) ⇌ 4C(g) + heat

When concentration of C decreases, according to Le Chatelier’s principle, the equilibrium position will shift to the right in order to produce more C.


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3.
2A(g) + B(g) ⇌ 4C(g) + heat

When concentration of A increases, according to Le Chatelier’s principle, the equilibrium position will shift to the right in order to consume more A.


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4.
2A(g) + B(g) ⇌ 4C(g) + heat
The forward reaction is exothermic, and the backward reaction is endothermic.

According to Le Chatelier’s principle, increase in temperature favors the endothermic reaction, i.e. the backward reaction. Therefore, the equilibrium position will shift to the left.