15.2.1 Approaching Chemical Equilibrium Flashcards
Consider the following equation:
CH4(g) + Cl2(g) Ch3Cl(g) + HCl(g) + 110 kJ
What happens to this reaction when the temperature is increased? (delta(triangle)H = -110 kJ/mol)
The equilibrium will shift to the left, because the backward reaction requires energy.
Consider the equilibrium between the following ions:
CoCl4^2-(aq) + 6H2O(l) Co(H2O)6^2+(aq) + 4Cl-(aq)
The colors of the aqueous solutions of the ions CoCl4^2- and Co(H2O)6^2+ are blue and pink, respectively.
The formation of CoCl42- is endothermic. What happens to the solution on heating?
The solution will turn blue.
When the temperature of an exothermic reaction is increased, what happens to the value of the equilibrium constant?
The value of the equilibrium constant decreases.
At a low temperature, which of these factors favors a forward reaction?
enthalpy
Increasing the temperature of a system increases the rate of a reaction and changes the value of the equilibrium constant. What other factor increases the rate of a reaction without affecting the equilibrium position?
a catalyst
Predict the direction in which the following equilibrium will shift if the pressure on the system is decreased by expansion.
ClF5(g) ClF3(g) + F2(g)
Equilibrium will shift to the right.
Consider the following equilibrium.
4NH3(g) + 3O2(g) 2N2(g) + 6H2O(l). Where delta(triangle) = -1530.4 kJ.
The dissociation of ammonia can be reduced by ___________.
increasing the temperature and increasing the volume of the system.
For a certain reaction the ΔH0 value, or change in enthalpy, is 508 kJ. How does the equilibrium constant for the reaction change with temperature?
It will increase because the forward reaction rate increases as temperature increases.
Look at the reaction shown below.
2HI(g) H2(g) + I2(g).
where delta H0 = 58 kJ
Which statement about this reaction is correct?
If the temperature of the system is increased, the equilibrium shifts toward the formation of the products.
Consider the following reaction:
SO2(g) + NO2(g) NO(g) + SO3(g) + 320 kJ.
Which of the following statements about this reaction is correct?
(delta H = -320 kJ/mol)
Products are favored in terms of enthalpy, but not entropy.
