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
chemistry - christina, T

I will do one, and be happy to critique your thinking.

b) it is endothermic, so adding heat (temperature) will increase the forward reaction. For pressure, shifting to the right increases the amount of volumes generated (3 volumes) from the reactant (2volumes). So, and increase in pressure will shift to the left to relieve the pressure, and vice versa. If you increase the amount of CO, the reaction will try to rid that by shifting to the left.

a solution that is 0.170 M in sodium formate (HCOONa) and .200 M in formic acid (HCOOH)

To answer these questions, you need to understand the effects of temperature, pressure, and concentration changes on equilibrium. Here are the steps you can take to find the answers:

1) Determine the expression for the equilibrium constant, Ke, for each equation. Ke is calculated based on the concentrations of the reactants and products at equilibrium.

2) To predict how Ke is affected by an increase in temperature, you need to know the sign of ΔH (the enthalpy change) for each equation. If ΔH is positive, the reaction is endothermic, and an increase in temperature will favor the forward reaction, causing Ke to increase. If ΔH is negative, the reaction is exothermic, and an increase in temperature will favor the reverse reaction, causing Ke to decrease.

3) To predict how the equilibrium will shift when pressure is decreased, you need to consider the stoichiometry of the balanced equation. Look at the coefficient of the moles of gas on each side of the equation. If the overall stoichiometry contains an equal number of moles of gas on both sides, a decrease in pressure will not cause a shift in equilibrium. If the number of moles of gas is higher on one side, a decrease in pressure will shift the equilibrium towards the side with fewer moles of gas.

4) To predict how the equilibrium will shift when the concentration of the underlined substance is increased, you need to apply Le Chatelier's principle. If the concentration of a reactant is increased, the equilibrium will shift towards the products to minimize the change. If the concentration of a product is increased, the equilibrium will shift towards the reactants to restore equilibrium.

5) To predict how the equilibrium will shift when the temperature is decreased, you use the same logic as for temperature increase. If ΔH is positive, the reaction is endothermic, and a decrease in temperature will favor the reverse reaction, causing the equilibrium to shift towards the reactants. If ΔH is negative, the reaction is exothermic, and a decrease in temperature will favor the forward reaction, causing the equilibrium to shift towards the products.

Apply these steps to each of the given equations, considering the given concentrations and heat values, to find the answers to each part (1, 2, 3, and 4) of the question.