Question

Consider the following equilibrium: Fe3+ + SCN1-   ↔ FeSCN2+ Fe3+ and SCN1- are essentially colourless and...

Consider the following equilibrium:

Fe3+ + SCN1-   ↔ FeSCN2+

Fe3+ and SCN1- are essentially colourless and FeSCN2+ is blood red in colour.

How would you expect the intensity of colour to change if SCN1- were added? (Choose...IncreaseDecreaseNo change)

How would you expect the reaction to shift if OH1- were added? (Choose...ForwardReverseNo change)

How would you expect the intensity of colour to change if Ag+ were added (Choose....increase,decrease,no change)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

To discuss this question,let us first be aware of the Formation Constant of Fe and thiocyaanate complex.The Fe and SCN- can form complex in presence of excess Thiocyanate.

So,Intensity of colour would increase if excess SCN-is added.

If OH- is added to the equilibrium, The complex would be formed in some amount which would result decrease in the rate of forward reaction of Fe-Thiocyanate complexation and from Le Chatelier's principle,in fact some would dissociate to give back i.e. the reaction would shift in reverse direction.

has a formation constant in the order of whereas has a formation constant in order.So the colour intensity of the Fe-Thiocyanate would decrease as the equilibrium shifts backwards.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. When the system Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) is at equilibrium, which one of the...
1. When the system Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) is at equilibrium, which one of the following statements best describes the equilibrium state? a.neither the forward nor the reverse reaction has stopped b. the value of the equilibrium constant is 1 c. the concentrations of Fe3+, SCN-, and FeSCN2+ are always equal at equilibrium d. both the forward and the reverse reaction has stopped 2. Which of the following will change the value of an equilibrium constant? I) varying the...
Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.0×10^−3 M...
Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.0×10^−3 M and an initial [SCN−] of 7.8×10^−4 M . At equilibrium, [FeSCN2+]= 1.7×10^−4 M . Part A Calculate the value of the equilibrium constant (Kc). Express your answer using two significant figures. Kc =
Consider the following reaction: Fe3+(aq)+SCN?(aq)?FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.1
Consider the following reaction: Fe3+(aq)+SCN?(aq)?FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.1
Consider the following endothermic reaction: N_2 O_4 (g)+Heat↔〖2NO〗_2 (s) a). In what direction would you expect...
Consider the following endothermic reaction: N_2 O_4 (g)+Heat↔〖2NO〗_2 (s) a). In what direction would you expect the equilibrium to shift when the reaction mixture is placed in a low temperature bath? b). If you carried out this experiment in the lab, what change would you look for to confirm this shift? c). In what direction would you expect the equilibrium to shift when the reaction mixture is placed in a high temperature bath? d). If you carried out this experiment...
2.) FeSCN2+ equilibrium concentration was found to be 3.20 x 10-5 M in a solution made...
2.) FeSCN2+ equilibrium concentration was found to be 3.20 x 10-5 M in a solution made by mixing 5.00 mL of 1.00 x 10-3 M Fe(NO3)3 with 5.00 mL of 1.00 x 10-3 M HSCN. The H+ concentration is maintained at 0.500 M at all times since the HSCN and Fe3+ solutions were prepared using 0.500 M HNO3 in place of distilled water. a. How many moles FeSCN2+ are present at equilibrium? b. How many moles each of Fe3+ and...
.   Consider the following equilibrium: 2 NO2 (g) + O2 (g) ⇌ 2 NO3 (g) +...
.   Consider the following equilibrium: 2 NO2 (g) + O2 (g) ⇌ 2 NO3 (g) + heat. (A)   How would the equilibrium shift if extra NO2 were added? (B) How would the equilibrium shift if O2 were removed? (C) How would you change the temperature to cause a shift to the products? (D) How would you change the pressure/volume to cause a shift to the reactants?
How does [B] change when D is added to the following reaction at equilibrium? 2 A(g)...
How does [B] change when D is added to the following reaction at equilibrium? 2 A(g) + B(g) ↔ 2 C(g) + D(s) How does [B] change when D is added to the following reaction at equilibrium? 2 A(g) + B(g) ↔ 2 C(g) + D(s) [B] will not change. Cannot be predicted. [B] will increase. [B] will decrease.
Refer to the reaction system C(s) + H2O(g) ↔ CO(g) + H2(g) at equilibrium for which...
Refer to the reaction system C(s) + H2O(g) ↔ CO(g) + H2(g) at equilibrium for which ΔH°rxn = +131 kJ. Assume ideal gas behavior. Predict the direction in which the above equilibrium will shift as a result of the stated change in conditions. a) An increase in the reaction temperature. b) A decrease in the amount of C(s). c) A decrease in the reactor volume. d) An increase in PH2O. e) Addition of N2 gas to the reaction mixture.
Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration...
Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration of H2O is increased. (a) In which direction does the reaction shift to reestablish equilibrium? (b) What happens to the concentrations of CH4, CO2, and H2 as the reaction shifts to reestablish equilibrium?
Consider a galvanic cell based upon the following half reactions: Fe3+ + 3e- → Fe -0.0036...
Consider a galvanic cell based upon the following half reactions: Fe3+ + 3e- → Fe -0.0036 V Cu2+ + 2e- → Cu 0.34 V How many of the following responses are true? 1. Increasing the mass of the Cu will change the initial potential of the cell 2. Fe is being oxidized during the reaction 3. Increasing the concentration of Cu2+ (assuming no volume change) will decrease the potential of the cell 4. Decreasing the concentration of Fe3+ (assuming no...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT