Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M and an initial [SCN−] of 8.2×10−4 M . At equilibrium, [FeSCN2+]= 1.8×10−4 M .
Calculate the value of the equilibrium constant (Kc)(Kc).
Express your answer using two significant figures.
Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M...
* PLEASE WRITE OUT ANSWER STEP BY STEP! CONSIDER THE FOLLOWING REACTION: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M and an initial [SCN−] of 8.2×10−4 M. At equilibrium, [FeSCN2+] = 1.6×10−4 M . PART A: Calculate the value of the equilibrium constant (Kc): [Express your answer using two significant figures] KC = _____________________________
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-] = 1.239; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.454 M. What is the numerical value of KC for this equilibrium? KC = __________________ 2) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.370; [SCN-] = 0.777; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.285 M. What is the equilibrium concentration of Fe3+? [Fe3+]eq =...
Review |Constants Periodic Table Consider the following reaction: Fe (aq) SCN (aq)FeSCN?+(aq) A solution is made containing an initial | Fe | of 1.2x10-3 M and an initial [SCN of 8.2x104 M At equilibrium, |FeSCN2+-1.8x10-4 M. We were unable to transcribe this image Review |Constants Periodic Table Consider the following reaction: Fe (aq) SCN (aq)FeSCN?+(aq) A solution is made containing an initial | Fe | of 1.2x10-3 M and an initial [SCN of 8.2x104 M At equilibrium, |FeSCN2+-1.8x10-4 M.
Consider the reaction represented by the equation: Fe3+ (aq) + SCN- (aq) FeSCN2+ (aq) What is the equilibrium concentration of FeSCN2+ (aq) if a solution is prepared that is initially 6.00 M Fe3+ (aq) and 6.00 M SCN− (aq)? if k was determined to be 0.333
Calculate the equilibrium constant for the reaction Fe3+ (aq0 + SCN (aq)→ FeSCN2+ (aq) given that the mixture of 5 ml of.00359 M SCN- and 5 ML of .00200 M Fe3+ solutions yield 1.68 x 10A- 4 M FeSCN2+ at a given temperature. a.) 23 . B.) 93 d. 8.06 x 10A-3 c.) 124
Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL 2.00 × 10−3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28 × 10−4 M. Find Kc for the reaction Fe3+(aq) + SCN−(aq) ↔ FeSCN2+(aq). a. What is the initial concentration of Fe3+ in the reaction mixture? [Fe3+] = ___ x 10-3 M b. What is the initial concentration of SCN- in the reaction mixture? [SCN-] = ___...
At a certain temperature, K = 8.60 x 10^-4. for the reaction FeSCN2+(aq) ⇄ Fe3+(aq) + SCN-(aq) Calculate the concentrations of Fe3+, SCN-, and FeSCN2+ in a solution that is initially 2.0 M FeSCN2+.
2. The reaction Fe3+ (aq) + SCN (aq) → FeSCN2+ (aq) produces a dark red color resulting from the formation of FeSCN2+. a. How does the color change if you add more SCN to a solution at equilibrium? (lighter or darker) b. How does the color change if you remove Fe3+ by reacting it with fluoride ions? c. If a reaction proceeds forward when you heat it, and reverse when you cool it, the reaction is [endothermic exothermic).
When solutions containing Fe3+(aq) ions and SCN−(aq) ions are mixed together, the following equilibrium is established: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) At equilibrium at some temperature, in 3.0 liters of total solution, there are 0.653 moles of FeSCN2+(aq), 0.0385 moles of Fe3+(aq) and 0.0465 moles of SCN−(aq) . What is K?
After the preparation of a solution with solutions containing Fe3+ and SCN- respectively, the final solution has a concentration of Fe(NCS)2+ 5.0x10-4 M, 1.0x10-3 M Fe3+ and 5.0x10-3 M SCN-. Calculate Kc for the following reaction. Fe3+ (aq) + SCN- (aq) ↔ Fe(NCS)2+ (aq) a. 80 b. 100 c. 0.01 d. 0.001