Magnesium hydroxide is used in several antacid formulations. When it is added to water it dissociates into magnesium and hydroxide ions.                            Mg(OH)2(s)  —->   Mg2+(aq) + 2OH–(aq) The equilibrium constant at 25°C is 8.9 x 10–12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH)2 are now added to the mixture?

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 12.5% of its initial value?

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 12.5% of its initial value?

The first-order reaction, 2 N2O(g) → 2 N2(g) + O2(g), has a rate constant equal to 0.76 s-1 at 1000 K. How long will it take for the concentration of N2O to decrease to 42% of its initial concentration?

In going from room temperature (25.0 °C) to 10 °C above room temperature, the rate of a reaction doubles. Calculate the activation energy for the reaction.

Which of the following statements are true about reaction mechanisms?I. A rate law can be written from the molecularity of the slowest elementary step.II. The final rate law can include intermediates.III. The rate of the reaction is dependent on the fastest step in the mechanism.IV. A mechanism can never be proven to be the correct pathway for a reaction.

In going from room temperature (25.0 °C) to 10 °C above room temperature, the rate of a reaction doubles. Calculate the activation energy for the reaction.

Consider a reaction that occurs by the following mechanism:A + BC → AC + BAC + D → A + CDThe potential energy profile for this reaction is shown below. Intermediates occur at which reaction stages?

Which of the following statements are true about reaction mechanisms?I. A rate law can be written from the molecularity of the slowest elementary step.II. The final rate law can include intermediates.III. The rate of the reaction is dependent on the fastest step in the mechanism.IV. A mechanism can never be proven to be the correct pathway for a reaction.

The following two isomers of C3H7NO exist in equilibrium with each other in solution:If Kc = 0.57 at 25°C and the initial concentration of the reactant is 0.50 M and the product is 0.70 M, what are the concentrations at equilibrium?