Question

QUESTIONS FOR LE CHATELIER'S 1. a. Write a balanced net ionic equation for the equilibrium reaction in Part A, formation of [Fe(SCN)]2+ (aq). b. For each of the changes in Part A, give the immediate effect of each perturbation on the value for Q (increase, decrease, or no change). Do the color changes you observed agree with the shift predicted by the change in Q? Explain your answers. i. additional iron(III) is added ii. additional thiocyanate is added iii. additional water is added 2. a. Write a balanced net ionic equation for the equilibrium reaction in Part B, formation of [Ni(NH3)6]2+(aq) b. Select which component from the equilibrium mixture reacts with HCl and then write a net ionic equation for that reaction (NOT AN EQUILIBRIUM!). c. The addition of hydrochloric acid impacts one of the components in the equilibrium reaction shown in 2a. Determine the immediate effect on the value of Q due to the addition of HCl. d. Do the color changes you observed agree with the shift predicted by the change in Q? Explain your answer. 3. a. Write a balanced net ionic equation for the (equilibrium) formation of the tetrachloridocobaltate(II) complex. b. Based on your observations of color changes in Part C, did heating the reaction mixture cause a shift in equilibrium? Which direction? Explain your answer based on the color changes you observed. c. Is the formation of tetrachlorocobaltate(II) complex ion exothermic or endothermic? Explain your answer based on the shifts in equilibrium caused by heating and cooling the reaction mixture. d. What is the effect of an increase in temperature on the value for the equilibrium constant? (Increase, decrease or no change)

          QUESTIONS FOR LE CHATELIER'S
1.
a. Write a balanced net ionic equation for the equilibrium reaction in Part A, formation
of [Fe(SCN)]2+ (aq).
b. For each of the changes in Part A, give the immediate effect of each perturbation on
the value for Q (increase, decrease, or no change). Do the color changes you
observed agree with the shift predicted by the change in Q? Explain your answers.
i. additional iron(III) is added
ii. additional thiocyanate is added
iii. additional water is added
2.
a. Write a balanced net ionic equation for the equilibrium reaction in Part B, formation
of [Ni(NH3)6]2+(aq)
b. Select which component from the equilibrium mixture reacts with HCl and then
write a net ionic equation for that reaction (NOT AN EQUILIBRIUM!).
c. The addition of hydrochloric acid impacts one of the components in the equilibrium
reaction shown in 2a. Determine the immediate effect on the value of Q due to the
addition of HCl.
d. Do the color changes you observed agree with the shift predicted by the change in
Q? Explain your answer.
3.
a. Write a balanced net ionic equation for the (equilibrium) formation of the
tetrachloridocobaltate(II) complex.
b. Based on your observations of color changes in Part C, did heating the reaction
mixture cause a shift in equilibrium? Which direction? Explain your answer based on
the color changes you observed.
c. Is the formation of tetrachlorocobaltate(II) complex ion exothermic or
endothermic? Explain your answer based on the shifts in equilibrium caused by
heating and cooling the reaction mixture.
d. What is the effect of an increase in temperature on the value for the equilibrium
constant? (Increase, decrease or no change)

QUESTIONS FOR LE CHATELIER'S
1.
a. Write a balanced net ionic equation for the equilibrium reaction in Part A, formation
of [Fe(SCN)]2+ (aq).
b. For each of the changes in Part A, give the immediate effect of each perturbation on
the value for Q (increase, decrease, or no change). Do the color changes you
observed agree with the shift predicted by the change in Q? Explain your answers.
i. additional iron(III) is added
ii. additional thiocyanate is added
iii. additional water is added
2.
a. Write a balanced net ionic equation for the equilibrium reaction in Part B, formation
of [Ni(NH3)6]2+(aq)
b. Select which component from the equilibrium mixture reacts with HCl and then
write a net ionic equation for that reaction (NOT AN EQUILIBRIUM!).
c. The addition of hydrochloric acid impacts one of the components in the equilibrium
reaction shown in 2a. Determine the immediate effect on the value of Q due to the
addition of HCl.
d. Do the color changes you observed agree with the shift predicted by the change in
Q? Explain your answer.
3.
a. Write a balanced net ionic equation for the (equilibrium) formation of the
tetrachloridocobaltate(II) complex.
b. Based on your observations of color changes in Part C, did heating the reaction
mixture cause a shift in equilibrium? Which direction? Explain your answer based on
the color changes you observed.
c. Is the formation of tetrachlorocobaltate(II) complex ion exothermic or
endothermic? Explain your answer based on the shifts in equilibrium caused by
heating and cooling the reaction mixture.
d. What is the effect of an increase in temperature on the value for the equilibrium
constant? (Increase, decrease or no change)

Added by Purificaci-N M.

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