Chemistry Help?

Question

Consider the following reaction: ﻿ 
2 A + 3 B2   ⇌ A2B6
The initial concentrations of A and B2 are   0.335   M and   0.940   M, respectively, with no A2B6 initially present.  When the reaction comes to equilibrium, the concentration of A2B6 is found to be   1.00×10−2   M.

1.)   What is the equilibrium concentration of A? (3 sig figs with units)
2.)   What is the equilibrium concentration of B2? (3 sig figs with units)
3.)   What is the value of the equilibrium constant? (3 sig figs with units)

Thomas Fiedler · Answer

I figured it out.
The answers are as follows:
1.) 0.315 M
2.) 0.910 M
3.) 0.134

? · Answer

2 A + 3 B2 ⇌ A2B6 
0.335 0.940.......0
0.325...0.91....0.01
so
1) 0.33 M
2) 0.91 M
3) 
K = 0.01 / (0.325^2*0.91^3) M^-4 = 0.126 M^-4 = 0.13  M^-4

Chemistry Help?

Related Questions

Trending Questions