Question

Please answer all six thanks

1) The equilibrium constant for the following reaction is 2.90×10^-2 at 1.15×10³K.

2SO₃(g) ------------------->2SO₂(g) + O₂(g)

If an equilibrium mixture of the three gases in a 17.3 L container at 1.15×10³K contains 0.437 mol of SO₃(g) and 0.422 mol of SO₂, the equilibrium concentration of O₂ is  M.

2) A student ran the following reaction in the laboratory at 1100 K:

2SO₃(g) -------------------->2SO₂(g) + O₂(g)

When she introduced 7.74×10^-2 moles of SO₃(g) into a 1.00 liter container, she found the equilibrium concentration of O₂(g) to be 1.75×10^-2 M.

Calculate the equilibrium constant, K_c, she obtained for this reaction.

K_c =

3) Consider the following reaction where K_c = 1.80×10^-2 at 698 K:

2HI(g) --------------------->H₂(g) + I₂(g)

A reaction mixture was found to contain 0.268 moles of HI(g), 3.93×10^-2 moles of H₂(g), and 4.03×10^-2 moles of I₂(g), in a 1.00 liter container.

Is the reaction at equilibrium?
If not, what direction must it run in order to reach equilibrium?

The reaction quotient, Q_c = .

The reaction:
A. must run in the forward direction to reach equilibrium.
B. must run in the reverse direction to reach equilibrium.
C. is at equilibrium.

4) Consider the following reaction where K_c = 1.29×10^-2 at 600 K:

COCl₂(g) -------------------------->CO(g) + Cl₂(g)

A reaction mixture was found to contain 0.104 moles of COCl₂(g), 2.68×10^-2 moles of CO(g), and 3.83×10^-2 moles of Cl₂(g), in a 1.00 Liter container.

Indicate True (T) or False (F) for each of the following:

___TF1. In order to reach equilibrium COCl₂(g) must be consumed.
___TF2. In order to reach equilibrium K_c must increase.
___TF3. In order to reach equilibrium CO must be produced.
___TF4. Q_c is greater than K_c.
___TF5. The reaction is at equilibrium. No further reaction will occur.

5) The equilibrium constant, K_c, for the following reaction is 55.6 at 698 K:

H₂(g) + I₂(g) ---------------------->2HI(g)

Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H₂ and 0.309 moles of I₂ are introduced into a 1.00 L vessel at 698 K.

[H2]	=	M
[I2]	=	M
[HI]	=	M

6) The equilibrium constant, K_p, for the following reaction is 0.444 at 452 K:

(CH₃)₂CHOH(g) ------------------------------->(CH₃)₂CO(g) + H₂(g)

Calculate the equilibrium partial pressures of all species when (CH₃)₂CHOH(g) is introduced into an evacuated flask at a pressure of 1.11 atm at 452 K.

P(CH3)2CHOH	=	atm
P(CH3)2CO	=	atm
PH2	=	at

Answer 1

(2)o Equilibrium concentration of SO2,SO, 10.422 mol = 0.0244 M )Equilibrium equati on: 2SO3 (g) 2SO2(g) + 17.3 L concentration of SO3, SO,10.437 mol 17.3 L 0.0253 M Equilibrium SO,l0] SO, (0.0244) [0,] (0.0253)3 Equilibrium constant, Kc 2.90x10 (2.90x10) (0.0253) (0.0244) 2 Equilibrium concentration of O. [O2m 2. equil 0.0312M 7.74x10 mol 7.74x10 M 2) Initi al concentrati on of SO 1.00 L ICE table 2SO (g) 2SO2(g) (2)0 0 Initi al (M) Change (M) Equilibrium (M): 7.74x10-2 7.74x10 -2x +2x x 2x 1.75x10 mol = 1.75x10 M According to the ICE table, [02 = (x) M = 1.00 L 1.75x10 Equilibrium concentration of SOs, [So] (7.74x102- 2(1.75x10)) 4.24x10 M Equilibrium concentration of SO2, [SO2]= 2(x) M = 2(1.75x10M = 3.50 x10 M So,o,] SO, (3.50x103 (1.75x10-2) (4.24x103) Equilibrium constant, K _ 1.19 x10 = 0.0119