Please help!!! Desperate for answer!!!?

Did the equation do not know the 2nd questions"s answers for the problems

a) 2O3(g) = 3 O2(g) + heat (O3 IS UNDERLINED)
[6.0x10-1] [0.21]

b) 2 CO2 (g) + heat = 2 CO(g) +O2(g) (CO IS UNDERLINED)
[0.103] [0.024] [1.18 x10-2]

c) NO2(g) + O2(g) + heat =NO (g) + O3(g) (NO IS UNDERLINED)
[0.072] [0.083] [6.73X10-2] [6.73 X10-2]
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For all three equilibria in problem #1 predict(1) how Ke is affected by an increase in temperature,(2)predict how the equilibrium will shift when pressure is decreased,(3)predict how the equilibrium will shift when the concentration of the underlined substance is increased ,and (4)predict how the equilibrium will shift when the temperature is decreased

Here is some information that might help you....

Effects of stress

Temperature Increase
exothermic.......shift to left
endothermic......shift to right

Temperature Decrease
exothermic.......shift to right
endothermic......shift to left

Pressure change
(only for unequal numbers of moles of gaseous products and reactants)
Decrease........shift toward side having larger # of gaseous molecules

Concentration Increase
Prouduct........shift toward left
Reactant........shift toward right

To answer these questions, we need to analyze the given equations and understand how changes in temperature, pressure, and concentration affect the equilibrium position.

1) How Ke is affected by an increase in temperature:
To determine how Ke is affected by changes in temperature, we need to consider the enthalpy (ΔH) of the reaction. The general relationship between temperature and equilibrium constant Ke is given by the Van't Hoff Equation:

ln(Ke2/Ke1) = ΔH/R * (1/T1 - 1/T2)

Where ΔH is the enthalpy change of the reaction, R is the gas constant, T1 is the initial temperature, and T2 is the final temperature. The value of ΔH can be positive, negative, or zero, which will define whether an increase in temperature will favor the forward or reverse reaction.

2) How the equilibrium will shift when pressure is decreased:
To understand how pressure changes affect the equilibrium, we need to evaluate the stoichiometry of the equation. If the total number of moles of gaseous species on the reactant side is larger, then a decrease in pressure will shift the equilibrium to the product side, and vice versa. This can be explained by Le Chatelier's Principle, which states that when a system at equilibrium is subjected to a stress, it will shift in a way to counteract that stress. Since reducing pressure is a stress on the system, it will shift to the side with a higher number of moles of gas to relieve the stress.

3) How the equilibrium will shift when the concentration of the underlined substance is increased:
When the concentration of a substance involved in the equilibrium is increased, the equilibrium will shift in the direction that consumes that substance in an attempt to restore the balance. This is again governed by Le Chatelier's Principle. If the underlined substance is on the reactant side, the equilibrium will shift towards the product side, and if it is on the product side, the equilibrium will shift towards the reactant side.

4) How the equilibrium will shift when the temperature is decreased:
Similar to point 1, when the temperature is decreased, we can refer to the Van't Hoff Equation. If ΔH is positive (endothermic reaction), a decrease in temperature will favor the forward reaction to generate more heat. If ΔH is negative (exothermic reaction), a decrease in temperature will favor the reverse reaction to generate more heat.

Now, armed with this knowledge, you can analyze the given equations and apply these principles to predict the effects of temperature, pressure, and concentration changes on the equilibrium position.