Solutes and react to produce solutes and in a reversible reaction, as shown by the equation. In a solution at equilibrium, the concentrations of , , , and are , , , and respectively. When a small quantity of compound is added to this solution, the composition of the solution changes according to Le Chatelier’s principle.
According to Le Chatelier’s principle, how and why does the position of equilibrium change?
Which equilibrium concentrations increase when compound is added?
Which of the following ratios of equilibrium concentrations does not change when compound is added?
In which of the following reactions would the addition of hydrochloric acid decrease the quantity of solid material?
In which of the following gas-phase reactions would the equilibrium yield increase with increasing pressure?
Methane reacts with steam in the presence of a catalyst to produce carbon monoxide and hydrogen gases, as shown in the equation:
The enthalpy change for this reaction is +206 kJ/mol.
Which of the following changes would produce the greatest increase in the yield of hydrogen?
Which of the following graphs best represents the change in equilibrium yield as the reaction temperature decreases below at 1 atm pressure?
A suspension contains solid in equilibrium with dissolved and ions. If more solid is added to the suspension, which of the following effects is not observed?
A suspension contains solid in equilibrium with dissolved and ions. If solid is added to the suspension, which of the following effects is not observed?
Gaseous phosphorus pentachloride decomposes into phosphorus trichloride and chlorine gases, as shown in the equation:
The enthalpy change for this reaction is +87.9 kJ/mol. The rates of the forward and backward reactions are shown schematically in the diagram:
Which diagram represents the rates of the forward and backward reactions when the temperature is increased at constant pressure?
Which diagram represents the rates of the forward and backward reactions when the pressure is decreased at constant temperature?
The colorless gas dinitrogen tetroxide decomposes reversibly into the brown gas nitrogen dioxide with a reaction enthalpy of +57.2 kJ/mol: A student stores a sample of dinitrogen tetroxide in a gas syringe at room temperature and 1 atm pressure and allows the plunger of the syringe to move freely. The gas is left to decompose until equilibrium is reached, as shown.
Why is the position of the plunger at equilibrium different from its position at the start of the reaction?
The student heats the gas syringe and allows the plunger of the syringe to move freely. Which diagram best illustrates the gas syringe under the new reaction conditions once equilibrium has been reached?