What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L of solution?
Question 6
6.
An NaOH solution contains 1.90 mol of NaOH, and its concentration is 0.555 M. What is its volume?
Question 7
7.
Question 8
8.
Question 9
9.
An equilibrium mixture of SO2, O2, and SO3 gases at 1500K is determined to consist of 0.344 mol/L SO2, 0.172 mol/L O2, and 0.56 mol/L SO3. What is the equilibrium constant for the system at this temperature? The balanced equation for this reaction is 2SO2(g) + O2(g) <-->2SO3(g).
Question 10
10.
Dissolved in water to make 100 mL of solution, 1.00 g of NaCl would have a concentration of
Question 11
11.
Question 12
12.
Question 13
13.
Question 14
14.
What is the equilibrium constant expression for the following reaction?
Fe(OH)3(s) <--> Fe3+(aq) + 3OH-(aq)
If the temperature of the equilibrium system X + Y <--> XY + 25 kJ decreases,
[X] decreases and [XY] increases.
[X] increases and [XY] decreases
[X] decreases and [XY] decreases.
the concentrations of reactants and products do not change.
How many moles of HCl are present in 0.70 L of a 0.33 M HCl solution?
0.23 mol
0.28 mol
0.38 mol
0.47 mol
What is the expression for the equilibrium constant for the reaction described by the following equation?
2A2B(g) + 3CD(g) <--> A4D3(g) + C3B2(g)
At equilibrium,
all reactions cease
the forward reaction continues to occur
the reverse reaction continues to occur
the concentrations of the products and reactants no longer change.
the amount of product is the same as the amount of reactant.
If the pressure on the reaction N2(g) + O2(g) <--> 2NO(g) at equilibrium is increased,
the amount of N2 will decrease.
the amount of NO will increase.
the amount of NO will decrease.
the concentrations of all the gases will remain unchanged.
When preparing a solution, decreasing the solvent but keeping the same amount of solute would result in
a more concentrated solution.
a less concentrated solution.
no change in the concentration of the solution.
a concentration that could increase or decrease, depending on how much solvent was removed.
A pitcher of lemonade and a glass filled with lemonade from the pitcher
have the same concentration, but different amounts of solutes.
have different concentrations, but the same amount of solutes.
have the same concentration, and the same amount of solute.
have different concentrations and different amounts of solute.
If a reaction system has come to equilibrium, it can be made to run to completion
only if it is not reversible.
only if the temperature is low enough.
by applying Le Châtelier’s principle.
under no circumstances.
A very low value of the equilibrium constant for a reaction can indicate that