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13 Dec 2019

Consider the reaction at equilibrium:

MgO(s) + H2O(l) <---> Mg(OH)2(aq)

If you increase the system's pressure, how will the system respond?

a.) the reaction will shift to the left

b.) not enough information

c.) the reaction will shift to the right

d.) nothing will happen

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Reid Wolff
Reid WolffLv2
17 Dec 2019

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Related questions

Consider the reaction at equilibrium:

MgO(s) + H2O(ℓ) ←→ Mg(OH)2(aq)

If you remove Mg(OH)2 from the system, how will the system respond?

1.)nothing will happen

2.) the reaction will shift to the left

3.) not enough information

4.) the reaction will shift to the right

Q1) The reaction shown below is endothermic.

NH4NO3 (s) NH4 + (aq) + NO3 − (aq)

a) Add energy (heat) to the above reaction as either a product or a reactant.

b) If the system shown above is cooled down, would the equilibrium shift to the right or to the left? Why?

c) Suppose you increase the concentration of NH4 + (aq). Would the equilibrium shift to the right or to the left? Why?

Q2) Consider the equilibrium reaction shown below.

HF(aq) + H2O(l) H3O + (aq) + F− (aq)

a) What will happen to the concentration of hydronium (H3O + ) in the system if a solution containing hydroxide (OH− ) is added? (Hint: see Equation (1).)

b) In which direction will the equilibrium shift if hydroxide is added? Why?

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system?

2 H2S(g) + 3 O2(g) <=> 2 H2O(g) + 2 SO2(g)

A. The equilibrium constant will decrease.

B. The reaction will shift to the right in the direction of products.

C. The reaction will shift to the left in the direction of reactants.

D. The equilibrium constant will increase.

E. No effect will be observed.

Could you please explain the answer?

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