What is the equilibrium constant expression for the following reaction?
Fe(OH)3(s) <--> Fe3+(aq) + 3OH-(aq)
Question 2
2.
If the temperature of the equilibrium system X + Y <--> XY + 25 kJ decreases,
Question 3
3.
How many moles of HCl are present in 0.70 L of a 0.33 M HCl solution?
Question 4
4.
What is the expression for the equilibrium constant for the reaction described by the following equation?
2A2B(g) + 3CD(g) <--> A4D3(g) + C3B2(g)
Question 5
5.
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.
At equilibrium,
Question 8
8.
If the pressure on the reaction N2(g) + O2(g) <--> 2NO(g) at equilibrium is increased,
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.
When preparing a solution, decreasing the solvent but keeping the same amount of solute would result in
Question 12
12.
A pitcher of lemonade and a glass filled with lemonade from the pitcher
Question 13
13.
If a reaction system has come to equilibrium, it can be made to run to completion
Question 14
14.
A very low value of the equilibrium constant for a reaction can indicate that
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.