# chemistry

The correct interpretation of the equation below is:?
Fe3+(aq) + SCN¨C(aq)¡ú FeSCN2+(aq)

A. The reaction is incomplete because the product is still charged.
B. A heterogeneous equilibrium exists because of the charged ions.
C. The equilibrium constant is Kc = [Fe3+][SCN¨C][FeSCN2+]
D. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.
E. None of these.

I think its E because c is def wrong. the others don't make much sense.

1. 👍 0
2. 👎 0
3. 👁 87
1. The correct answer is D.
At equilibrium, the forward rate equals the reverse rate.

1. 👍 0
2. 👎 0
2. thanks

1. 👍 0
2. 👎 0
posted by david

## Similar Questions

1. ### CHEMISTRY HELP! ICE TABLES?

At a certain temperature, K = 9.1 10-4 for the following reaction. FeSCN2+(aq)= Fe3+(aq) + SCN -(aq) Calculate the concentrations of Fe3+, SCN -, and FeSCN2+ in a solution that is initially 4.0 M FeSCN2+. OKAY SO i started by

asked by Taylor on January 15, 2009
2. ### chemistry

The correct interpretation of the equation below is: Fe3+(aq) + SCN–(aq) --> FeSCN2+(aq) A. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. B. The equilibrium constant is Kc =

asked by Jerome on April 10, 2008
3. ### chemistry

The correct interpretation of the equation below is: Fe3+(aq) + SCN–(aq) --> and

asked by Lindsey on April 9, 2008
4. ### chemistry

In a certain trial, the initial concentrations of Fe3+ and SCN- are both 1.00x10^-3 M and the initial concentration of FeSCN2+ is zero. Suppose that after the reation reaches equilibrium, the concentration of FeSCN2+ was found to

asked by Elly on June 20, 2011
5. ### Chemistry

I am having trouble getting the right answer for this question please help. Calculate Kc for the FeSCN2+ formation equilibrium [FeSCN2+] = 3.49x10^-5 M [Fe3+] = 4.39x10^-4 M [SCN-] = 1.93x10^-4 Kc = [FeSCN2+] / ([Fe3+]-[FeSCN2+])

asked by Amanda on March 20, 2017
6. ### Chemistry

A student mixes 5.0 mL of 0.00200 M Fe(NO3)3 with 5.0 mL 0.00200 KSCN. She finds that the concentration of FeSCN2+ in the equilibrium mixture is 0.000125 M. Follow these steps to determine the corresponding experimental value of

asked by anon on March 10, 2015
7. ### Chemistry

A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be M. What permits

asked by Neil on June 20, 2011
8. ### chemistry

Assume that it is necessary to determine the [FE^3+ in a solution that may be 0.0001 to 0.0005 M range . Outline the spectrophotometric method that would accurately give the required data. Be spectific about the solutions that you

asked by jxv on November 13, 2016
9. ### chemistry

fe 3+ + scn- fescn2+ Apparatus and materials: 0.2 M Fe(NO3)3, 0.002M Fe(NO3)3, 0.002 M KSCN. PRELAB: for this section [fe3+]i = y [scn-]i = z and [fescn2+]eq = x using the symbols y,z,x, fill in the ice char. note that the rxn

asked by Tri on October 26, 2008
10. ### Chemistry

Write the Kc expression for the following reaction: Fe3+ + SCN- = FeSCN2+

asked by Aiyana M. on February 20, 2017

More Similar Questions