Atoms and the Atomic Theory
Law of Conservation of Mass The total mass of substances present after a chemical reaction is the same as the total mass of substances before the reaction. Or Matter is neither created nor destroyed during a
Equilibrium Constant Worksheet
1. The equilibrium constant for the acid ionization of mercaptoethanol
(HSCH2CH2OH) is 1.91 x 10 .
H (aq) + SCH2CH2OH (aq)
K = 1.91 x 1010
Which of the following statements is true regarding this equilibr
1. Which of the following is true for a chemical reaction at equilibrium?
only the forward reaction stops
only the reverse reaction stops
both the forward and reverse reactions stop
the rate constants for the fo
1. Write an expression for the equilibrium constant for the formation of two moles
of ammonia gas (NH3) from nitrogen and hydrogen in their standard states.
N2(g) + 3 H2(g)
2.Write the correct Kc expression for the followin
1. For the following reaction, write how the each of the changes will affect the
indicated quantity, assuming a container of fixed size. Write increase,
decrease, or no change. (Or use an up arrow to indicate increase, and a
LeChateliers Principle Introductory Problems:
1. 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)
adding heat t
LeChateliers Principle Practice
1. Which of the following occurs when reactantsareaddedto a chemical
reaction in solution or the gas phase at equilibrium?
Qincreases, so the equilibrium shifts to produce more products.
Qincreases, so the equilibrium
1. For the chemical equilibrium A + 2B
2C, the value of the equilibrium
constant, K, is 10. What is the value of the equilibrium constant for the reaction
written in reverse?
Given that: A+2B
Reaction Stoichiometry: Quantitative relationships between reactants and products.
Carbon monoxide and oxygen can combine to form carbon dioxide. How many moles of carbon dioxide will be produ
Titration: A lab technique used to determine the unknown concentration of an acid or
base using a neutralization reaction.
The point in a titration where the moles of acid = moles of base
Endpoint Point a