Question

R --> 2 P. Initially you start off with 0.5 M reactants and let the reaction run to equilibrium and calculate the equilibrium constant, K, value. What happens to that value if you run the reaction to equilibrium again at the same temperature but double the initial concentration of the reactants to 1.0 M?

Answer 1

Answer:

K still the same value

Step-by-step explanation:

given a reaction aA+bB<->cC+dD the constant K is defined as:

$\frac{C^{c}D^{d} }{A^{a}B^{b} }$

K is a constant so it won't change the value. Instead, the values of C and D are going to change.  The position of equilibrium moves because of the need to keep a constant value for the equilibrium constant.