Chem110 Don’t get stressed lab

[Fe3+] [SCN·] [Fe(SCN)2+] Initial Concentration 9.091x10-4 1.818x10-4 0 Change in Concentration       Equilibrium Concentration     3.191x10-5 Can someone help with this ICE table?

Please answer questions 1 through 3 and provide explanations when necessary! Thank you!

What is the value in the concentration of the SCN Suppose the Keq for this experiment is 523. The initial concentration of the Fe+ is 4.00 x 10-2 M The initial concentration of the SCN is 1.00 x 10-3 M The reaction of the experiment: Fe3++ SCN 2 Fe(NCS)2+ The concentration of the SCN at equilibrium is : Y x 104M Your answer should have 2 sf

Fill in this table based on given concentrations Ecell Hypothetical [Zn +2] [Cu *2] e transferred # 1 0.1 M 0.1 M 0.1 M # 2 1 x 10 -3 M # 3 0.1 M 1 x 10 -6 M # 4 0.1 M 1 x 10 -9 M

4. During Part 1, which reactant (Fe3+ or SCN-) is in excess and which is limiting? What is the purpose of making one reactant in excess? (Connect to Le Chatelier's Principle) How will you know the concentration of Fe(SCN)2+?

the equilibrium expressions for the following reactions:   2Fe(s)      +        3H2O(g)   ↔        Fe2O3(s)     +    3 H2(g)   A [Fe2O3][H2]      = Keq [Fe][H2O]   B [Fe2O3][H2]3     = Keq [Fe]2 [H2O]3   C [H2]3     = Keq [H2O]3   D   [Fe]2 [H2O]3     = Keq [Fe2O3][H2]3

2. What is the concentration of [Ag(S2O3)2]3- in a solution which contains 7.5 x 10-7 M Ag+ ions and 1.5 x 10-6 M S2O32- ions?   The Kf for [Ag(S2O3)2]3- is 4.7 x 1013. a. 8.3 x 10-2 M b. 0.529 M c. 7.9 x 10-5 M d. 52.9 M

Equilibrium: Co(H2O)62+ (aq) + 4 Cl-(aq) ⇌ CoCl42- (aq) + 6 H2O (l) pink blue a. You put 5 mL of stock solution into each of five test tubes. (25 mLs divided evenly into 5 test tubes). Test tube 1 was your control. To test tube 2, you added some water. Which direction did the equilibrium shift? How do you know? b. To test tube 3 you added some silver nitrate. Did this shift the equilibrium? If so, how is that possible as silver ion and nitrate ion are not in the equation? c. To test tube 5, you put the stock solution into hot water and it turned blue; then you put it into ice water and it turned pink. Explain what happened.

Determine the initial concentration of Fe3+ and SCN- in the equilibrium solution.   Solution 1 0.002 M iron (III) nitrate in 1 M nitric acid: 5mL 0.002 M potassium thiocyanate: 1 mL DI water: 4mL volume: 10.1mL absorbance: 0.062

uestion 8 Using the table provided, determine the AH for the following reaction: 3N204 + 2H2O() → 4HNO3 + 2NO Moving to another question will save this response.

Cu(s) + 2Ag*(aq) 2Ag(s) + Cu2+(aq) For the above reaction would the Ecell increase, decrease, or remain the same if the concentration of Ag* is halved and the [Cu2+] is reduced to 1/4 of the initial concentration. increase remain the same decrease can't tell

Image below

3. Changing Reaction Equilibrium Conditions - Le Chatelier's Principle 3A. Effect of Changing Reactant Concentration Test tube Is intensity of red color darker Is [Fe(SCN)]²* or lighter compare to the reference test tube color Color of solution increased or decreased? 1. Reference Blood red color 2. Fe* added Dark blood red darker color 3. SCN added Dark blood red darker color 4. Fe* removed Light Blood red lighter by adding CI color 5. SCN' removed Light blood red lighter by adding Ag* color Question 10: With the addition of more Fe*³ ions in test tube 2, did the reaction equilibrium move towards reactants or products? Explain. Question 11: With the addition of more SCN' ions in test tube 3, did the reaction equilibrium move towards reactants or products? Explain. Question 12: The addition of Cl ions in test tube 4 shifts the equilibrium in the backward direction. Explain how.

O KINETICS AND EQUILIBRIUM Writing the concentration equilibrium expression for a... Write the concentration equilibrium constant expression for this reaction. Cu(s)+ 2 Agt(aq) →Cu²+ (aq)+ 2 Ag(s) X 00 0/5

3. Upon addition of CI to the following reaction, which direction will the reaction shift? Co(H2O)6 2+ + 4 Cl CoCl2 + 6 H₂O

For the Reaction: Co(H2O)62++4Cl- = CoCl42+ + 6H2O  When adding CoCl2+ H2O  What stress is applied and what direction does the equilibrium shift?

A student records the following equilibrium concentrations for the iron(III) thiocyanate equilibrium. [Fe(SCN)2+] = 0.00023 M [Fe³+] = 0.0037 M [SCN-] = 0.0038 M What is the value of Kc for this equilibrium?

Are the following reactions predicted to have an equilibrium to the right or left based on HSAB theory?HgI + LiF = HgF + LiI TiH + Na+ = Ti+ + NaH

29. Fe,03 + CO - Fe+CO2 1,3, 2, 3 What coefficients are required to balance the equation above? 1,1, 2, 1 2, 6, 3, 6 1, 1, 2, 2 CLEAR ALL Unanswered ( PREVIOUS 23 24 25 26 O31 27 28 29 30

Scott prepares a solution which contains a large excess of iron and a small amount of thiocyanate. He notices a faint orange color appear in the solution once mixed. He repeats this process with a higher concentration of thiocyanate and notices a deepening of the orange color in the solution once mixed. Explain what has happened to the equilibrium in this case. Has the value of Keq changed? Explain.

. Use stoichiometry to determine the equilibrium [Fe3+] and [SCN-] in each test tube. y = 6170.7x - 0.0153 Solution  0.002M iron(III) nitrate in 1M nitric acid(mL) 0.002M potassium thiocyanate(mL) DI water(mL) Absorbance(A) 1 3 2 1 0.128 2 2 3 1 0.269