Question 15 (1 point)

What will happen when the concentration of hydrochloric acid is increased in the following system?

2 HCl (aq) + Mg (s) <--> MgCl₂ (aq) + H₂ (g) + energy

Question 15 options:

	To restore equilibrium the system will shift left.
	There will be effect on the equilibrium.
	To restore equilibrium the system will shift right.

Question 16 (1 point)

An equilibrium expression is provided below. Which of the following balanced chemical equations could it represent?

K = [NO2]4/[NH3]4 [O2]7

Question 16 options:

	NH3 (g) + O2 (g) NO2 (g)
	4NO2 (g) 4NH3 (g) + 7O2 (g)
	4NO2 (g) + 6H2O(l) 4NH3 (g) + 7O2 (g){
	4NH3 (g) + 7O2 (g) 4NO2 (g) + 6H2O(l)

Question 17 (1 point)

Given the following reaction at equilibrium, which of the following alterations will increase the amount (in moles) of SO₂Cl₂: (there is only one correct answer) SO₂(g) + Cl₂(g) SO₂Cl₂(g) H = -67 kJ

Question 17 options:

	Adding heat to the system.
	Increasing the volume of the system.
	Removing SO2Cl2 from the system.
	Adding SO2 to the system.
	Adding a catalyst to the system.

Question 18 (1 point)

In a solution of copper(II) chloride, the following equilibrium exists:

CuCl42(aq) + 4H2O(l) Cu(H2O)42+(aq) + 4Cl(aq)

Which of the following best describes the concentrations changes that occur if concentrated HCl (aq) was added to the reaction vessel? Recall that strong acids dissociate 100% to form H⁺ (aq) and Cl^- (aq) ions.

Question 18 options:

	[CuCl42-] ; initial[Cl-] then decrease,
	[H2O] ; initial [Cl-] then decrease,
	[CuCl4-]; [Cl-]
	[CuCl4- ]; [Cl- ]