ZuoTi.Pro
Question

At a certain temperature, Keq = 150 for the reaction being studied in today’s lab. Use...

At a certain temperature, Keq = 150 for the reaction being studied in today’s lab. Use Equation (3) to calculate the concentrations of Fe3+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 10-5 M. Assume the equilibrium concentrations of Fe3+ and SCN are equal.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
At a certain temperature, Keq = 150 for the reaction being studied in today’s lab. Use...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Equilibrium Concentrations for a Simple Addition Reaction At a certain temperature K = 1.10x103 for the reaction: Fe3+(...

    Equilibrium Concentrations for a Simple Addition Reaction At a certain temperature K = 1.10x103 for the reaction: Fe3+(aq)SCN"(aq) FeSCN2+(aq) 5.00x102 mol of Fe(NO3)3 is added to 8.70x 10-1 L of 1.84 x 10-1 M KSCN. Neglecting any volume change and assuming that all species remain in solution--: Calculate the equilibrium concentration of Fe3+ (in mol/L) mol/L 1 pts 提交答案 Tries 0/8 Calculate the equilibrium concentration of SCN (in mol/L). mol/L 1 pts [提交答案 Tries 0/8 Calculate the equilibrium concentration of...

  • At a certain temperature, K = 8.60 x 10^-4. for the reaction FeSCN2+(aq) ⇄ Fe3+(aq) +...

    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+.

  • Equilibria can be treated mathematically with the equilibrium constant, K. For the reaction Fe3+ + SCN...

    Equilibria can be treated mathematically with the equilibrium constant, K. For the reaction Fe3+ + SCN − equilibrium reaction arrow FeSCN2+, the equilibrium constant expression is [FeSCN2+ ] K = [Fe3+ ] · [SCN − ] where, for example, [Fe3+ ] is the molar concentration (mol Fe3+ / L solution) present in an equilibrium mixture. At some temperature, a chemist found the following equilibrium concentrations. [Fe3+ ] = 8.17 ✕ 10−3 M, [SCN − ] = 8.60 ✕ 10−3 M,...

  • For each equilibrium sample, calculate the initial concentrations (assuming no reaction occurred)...

    For each equilibrium sample, calculate the initial concentrations (assuming no reaction occurred) of SCN– and Fe3+ based on the dilution factors used. Enter the absorbance values for each sample. For the standard solution, assume that, when equilibrium is reached, the [FeSCN2+]eq is equal to [SCN–]ini. Why is this a good assumption? For the equilibrium solutions, calculate the [FeSCN2+]eq (Ceq) using Eq. 4. Using Eq. 5 and 6, calculate [Fe3+(aq)]eq and [SCN–(aq)]eq for each equilibrium solution. Calculate values for the equilibrium...

  • Use the mean value of 540 for Keq to calculate the SCN- concentration in a solution...

    Use the mean value of 540 for Keq to calculate the SCN- concentration in a solution whose initial Fe3+ concentration was 3.60x10-2 M and initial SCN- concentration was 1.30x10-3 M. Give answer in M. Equation: Fe3+ + SCN- <-----------> FeNCS2+

  • Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL...

    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-] = ___...

  • Use the mean value of 533 for Keq to calculate the SCN− concentration in a solution...

    Use the mean value of 533 for Keq to calculate the SCN− concentration in a solution whose initial Fe3+ concentration was 4.10×10−02 M and initial SCN− concentration was 1.50×10−03 M Fe3+ +SCN- --->FeNCS2+

  • thiocyanatoiron (III)ion? The path length for the light is 1.00 cm? FE(NO3)₂ + KSCN sre(SCN) KT...

    thiocyanatoiron (III)ion? The path length for the light is 1.00 cm? FE(NO3)₂ + KSCN sre(SCN) KT + 3No. [NOPZ Keq & [Lee SCN ) 2+] [x+) Tre(NO3); [ilsen . 1.4 x 10² x (1-x)² = 23 x 3 X 0.77 m Keqz (3x) I Toro-x) (2.00 X 2. Assuming that the equilibrium concentration of [FeSCN2') is 6.08 x 10 Min a solution that initially was 1.00 x 10 Min Fe3+ and 2.00 x 10 Min SCN, calculate the equilibrium concentrations...

  • Consider the reaction represented by the equation: Fe3+ (aq) + SCN- (aq) FeSCN2+ (aq) What is...

    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

  • 4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of...

    4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M. Part A: Calculate the number of moles of Fe3+ initially added to the solution. Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium....

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT