0.300 mol of S2 and 0.310 mol of C are placed in a 1.00 L flask and allowed to reach equilibrium according to this reaction:
S2(g) + C(s) ⇔ CS2(g)
At equilibrium, 0.271 mol of CS2 is present. The value of Keq for the reaction is ----
a)9.3
b)0.91
c)240
d)2.9
Not too certain about this question.
It would be much easier to help you if you didn't change screen names. See your post above on K (where you didn't post the equation). Mathmate answered that.
To find the value of Keq for the reaction, we first need to determine the concentrations of the species involved at equilibrium.
Given:
Initial moles of S2 = 0.300 mol
Initial moles of C = 0.310 mol
Moles of CS2 at equilibrium = 0.271 mol
To find the concentrations, we divide the number of moles of each species by the volume of the flask:
Concentration of S2 at equilibrium = moles of S2 / volume = 0.300 mol / 1.00 L = 0.300 M
Concentration of C at equilibrium = moles of C / volume = 0.310 mol / 1.00 L = 0.310 M
Concentration of CS2 at equilibrium = moles of CS2 / volume = 0.271 mol / 1.00 L = 0.271 M
Now, we can use the concentrations to determine the value of Keq using the following equation:
Keq = [CS2] / ([S2][C])
Inserting the values, we get:
Keq = 0.271 M / (0.300 M * 0.310 M) = 0.271 / 0.093 = 2.91
Therefore, the value of Keq for the reaction is approximately 2.91. Since none of the given options matches exactly, we can conclude that the correct answer is not provided.