1.) Consider the reaction 3A <===> 2B, where the value of K is 22.1. If the conc
ID: 1007899 • Letter: 1
Question
1.) Consider the reaction 3A <===> 2B, where the value of K is 22.1. If the concentration of A is 0.015 at equilibrium, what is the concentration of B?
2.) For the reaction
C(s) + CO2(g) <====> 2CO(g) Kc = 168,
determine whether the system is at equilibrium when [CO] = 0.50 M and [CO2] = 0.75 M. The system ____ at equilibrium, because ___.
3.) Consider the reaction A <===> B, where the value of Kc is 1.4 x 10–15. Which statement about the system at equilibrium is correct?
A. 6.5 x 106 B. 0.010 C. 1.0 D. 8.6 x 10-3 E. 7.5 x 10-5Explanation / Answer
Q.1: Given [A]eq = 0.015
The given reaction is
3A <===> 2B: K = 22.1
K = 22.1 = [B]2 / [A]3
=> 22.1 = [B]2 / (0.015)3
=> [B]2 = 22.1 x (0.015)3 =
=> [B] = 8.6x10-3 M (answer)
Option D is correct
Q.2: C(s) + CO2(g) <====> 2CO(g): Kc = 168
Q value for the above reaction is
Q = [CO(g)]2 / [CO2(g)] = (0.5)2 / (0.75) = 0.333
Hence Q < K,
However for a reaction to be in equilibrium, Q must be equal to K
Hence the system is not at equilibrium because Q = 0.33
Hence option A is correct.
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