For the reaction ⇌+2H2gS2g2H2Sg, determine the equilibrium constant at 700°C if at this temperature, the equilibrium concentrations are as follows: [H2] = 0.208 M, [S2] = 1.13 × 10-6 M, [H2S] = 0.725 M
Question
For the reaction ⇌+2H2gS2g2H2Sg, determine the equilibrium constant at 700°C if at this temperature, the equilibrium concentrations are as follows: [H2] = 0.208 M, [S2] = 1.13 × 10-6 M, [H2S] = 0.725 M
Solution
The equilibrium constant (Kc) for a reaction is given by the formula:
Kc = [Products] / [Reactants]
In this case, the reaction is: H2 + S2 ⇌ 2H2S
So, the equilibrium constant expression is:
Kc = [H2S]^2 / ([H2] * [S2])
Given the equilibrium concentrations: [H2] = 0.208 M, [S2] = 1.13 × 10^-6 M, [H2S] = 0.725 M, we can substitute these values into the equilibrium constant expression:
Kc = (0.725)^2 / (0.208 * 1.13 × 10^-6)
Now, calculate the value of Kc.
Similar Questions
Calculate the equilibrium constant Kc for the reaction:2XY(g) ⇌2X (s) + Y2(g)When the number of moles of XY, X2, Y2 : 0.8 ,0.4 & 0.2 moles respectively, put in container of volume = 4L .
The equilibrium constant, KC, for the following reaction is 280 at 1,000 K.2SO2(g) + O2(g) ⇌ 2SO3(g)If [SO2]eq = 0.80 M and [O2]eq = 0.35 M, then [SO3]eq = 6.2 × 10-27.9262.72792 M.
The equilibrium constant for a cell reaction, Cu(g) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s) is 4 × 1016. Find for the cell reaction.(Given log10 2 = 0.301)0.63 V0.49 V1.23 V3.24 V
What is the correct equilibrium constant expression or equation for the reactionH2(g) + Cl2(g) ⇋ 2HCl(g) Question 2Select one:a.b.c. d.
0.924 mole of A (g) is placed in a 1.00 liter container at 700 ° C, where it is 38.8 % dissociatedwhen equilibrium was established.3 A (g) 5 B (g) + 2 C (g)What is the value of the equilibrium constant, Kc, at the same temperature?
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.