For the reaction of nitrogen gas and hydrogen gas to make methane, describe FOUR stresses would shift the equilibrium to the left toward the reactants? (10 points) N2(g) + 3 H2(g) ⇌ 2 NH3(g) + Energy

1) decrease in pressure

2) increase in temperature

3) increase in volume

4) accumulation of the product in the reaction system

Step-by-step explanation:

Equilibrium is generally defined as a state in which there is no observable change in the system over a period of time. In chemical systems, equilibrium is dynamic, this implies that the toward and reverse reactions proceed at the same rate.

The Le Chateliers principle states that if an external constraint such as change in temperature, pressure or concentration is imposed on a reaction system in equilibrium, the equilibrium position will shift so as to annul the constraint.

For the system shown in the question, low pressure, increase in volume, increase in temperature and accumulation of the product in the reaction system will make the equilibrium position to shift towards the left (reactants side)

y=mx+b

step-by-step explanation:

m slope, b y-intercept

goog may have it for you