The initial concentrations are [so2]

Reference no: EM13691843

How does [H2O] change when sulfur is added to the following reaction at equilibrium?
2 H2S(g) + O2(g) ? 2 S(s) + 2 H2O(g)

How does [H2O] change when sulfur is added to the following reaction at equilibrium?
2 H2S(g) + O2(g) ? 2 S(s) + 2 H2O(g)
[H2O] will decrease.
[H2O] will not change.
Cannot be predicted.
[H2O] will increase

The reaction 2 SO2(g) + O2(g) ? 2 SO3(g) has an equilibrium constant of 6.23 x 104 at 450°C. If the initial concentrations are [SO2] = 0.230 M, [O2] = 0.113 M, and [SO3] = 15.3 M, which of the following statements is true?

The reaction 2 SO2(g) + O2(g) ? 2 SO3(g) has an equilibrium constant of 6.23 x 104 at 450°C. If the initial concentrations are [SO2] = 0.230 M, [O2] = 0.113 M, and [SO3] = 15.3 M, which of the following statements is true?
The system is at equilibrium and will not shift in either direction.
Cannot be predicted.
The system is not at equilibrium and will shift to the right to establish equilibrium.
The system is not at equilibrium and will shift to the left to establish equilibrium.
If the temperature is decreased and some C is added, how does this affect the amount of A present at equilibrium for the following reaction?
A(g) + B(g) ? 2 C(g) + D(g) ?H° = -80 kJ

If the temperature is decreased and some C is added, how does this affect the amount of A present at equilibrium for the following reaction?
A(g) + B(g) ? 2 C(g) + D(g) ?H° = -80 kJ
Cannot be predicted.
The amount of A will decrease.
The amount of A will not change.
The amount of A will increase.
How does an increase in temperature affect the equilibrium concentration of C and the equilibrium constant for the following reaction?
2 A(g) + B(g) ? 3 C(g) + D(g) ?H° = - 100 kJ

How does an increase in temperature affect the equilibrium concentration of C and the equilibrium constant for the following reaction?
2 A(g) + B(g) ? 3 C(g) + D(g) ?H° = - 100 kJ
[C] will increase and the equilibrium constant will increase.
[C] will increase and the equilibrium constant will decrease.
[C] will decrease and the equilibrium constant will decrease.
[C] will decrease and the equilibrium constant will increase.
How does [H2O] change when sulfur is added to the following reaction at equilibrium?
2 H2S(g) + O2(g) ? 2 S(s) + 2 H2O(g)

How does [H2O] change when sulfur is added to the following reaction at equilibrium?
2 H2S(g) + O2(g) ? 2 S(s) + 2 H2O(g)
[H2O] will decrease.
[H2O] will not change.
Cannot be predicted.
[H2O] will increase

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system?

C3H8(g)+5O2(g)?3CO2(g)+4H2O(l); ?H0 = -2220 kJ
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system?

;delta H = -2220
The equilibrium constant will increase.
The reaction will shift to the right in the direction of products.
The reaction will shift to the left in the direction of reactants.
The equilibrium constant will decrease.
No effect will be observed.

How does an increase in the pressure within the container by the addition of an inert gas like helium affect the amount of the Cl2 present at equilibrium for the following reaction?
4 HCl(g) + O2(g) ? 2 H2O(g) + 2 Cl2(g) ?H° = 120 kJ

How does an increase in the pressure within the container by the addition of an inert gas like helium affect the amount of the Cl2 present at equilibrium for the following reaction?
4 HCl(g) + O2(g) ? 2 H2O(g) + 2 Cl2(g) ?H° = 120 kJ
The amount of Cl2 will decrease.
Cannot be predicted.
The amount of Cl2 will not change.
The amount of Cl2 will increase.

Reference no: EM13691843

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The initial concentrations are [so2] : The reaction 2 SO2(g) + O2(g) ? 2 SO3(g) has an equilibrium constant of 6.23 x 104 at 450°C. If the initial concentrations are [SO2] = 0.230 M, [O2] = 0.113 M, and [SO3] = 15.3 M, which of the following statements is true?

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