Question

10) The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 10) 2 SO2(8) + O2(8) - 2 SO3(3). If initial concentrations are [SO2) = 6.00 M, [02] -0.45 M, and (SO3) = 9.00 M, the system is A) not at equilibrium and will shift to the right to achieve an equilibrium state. B) not at equilibrium and will shift to the left to achieve an equilibrium state. C) at equilibrium D) not at equilibrium and will remain in an unequilibrated state. concentration in a 0.169 M Ca(OH)2 solution. 11) Determine the [OH A) 5.92 x 10-14 M B) 2.96 10-14 M C) 0.338 M D) 0.169 M E) 0.298 M 12) What is the Kw of pure water at 50.0°C, if the pH is 6.6307 A) 2.34 x 10-7 B) 2.13 x 10-14 C) 1.00 x 10-14 D) 5.50 x 10-14 E) There is not enough information to calculate the Kw.

Answer 1

Multiple questions , student have not specifically asked question to be answered, as per guideline only, first one will be answered :

11).

Reaction equilibrium:

2 SO₂(g) + O₂ (g) $\rightleftharpoons$ 2SO₃ (g)

K (equilibrium constant) = [ SO₃ ]² / [ SO₂ ]² [O₂ ] = 5.00 (at 1300 K

From given data , reaction quotient :

Q =   [ SO₃ ]² / [ SO₂ ]² [O₂ ] =  [9.00 ]² / [ 6.00 ]² [0.45 ] = 5.00

We have, K = Q ( Reaction mixture is already at equilibrium )

So, answer will be : (c) the system is at equilibrium.