Equilibrium Flashcards

1
Q

dynamic equilibrium

A

The term dynamic means both forward and backward reactions are occurring simultaneously

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2
Q

Two features of Dynamic Equilibrium

A
  1. Forward and backward reactions are occurring at equal rates.
  2. The concentrations of reactants and products stays constant
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3
Q

Le Chatelier’s Principle

A

Le Chatelier’s principle states that if an external condition is changed the equilibrium will shift to oppose the change (and try to reverse it).

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4
Q

Effect of Temperature on equilibrium

A

If the temperature has increased the equilibrium will shift to oppose this and move in the endothermic direction to try to reduce the temperature by absorbing heat

If the temperature has decreased the equilibrium will shift to oppose this and move in the exothermic direction to try to increase the temperature by giving out heat.

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5
Q

What effect would increasing temperature have on the yield of ammonia?

N2 + 3H2—— 2NH3 exothermic

A

If temperature is increased the equilibrium will shift to oppose this and move in the endothermic, backwards direction to try to decrease temperature. The position of equilibrium will shift towards the left, giving a lower yield of ammonia

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6
Q

Effect of Pressure on equilibrium

A

Increasing pressure will cause the equilibrium to shift towards the side with fewer moles of gas to oppose the change and thereby reduce the pressure

Decreasing pressure will cause the equilibrium to shift towards the side with more moles of gas to oppose the change and thereby increase the pressure

If the number of moles of gas is the same on both sides of the equation then changing pressure will have no effect on the position of equilibrium

H2 + Cl2 ⇌ 2HCl

Increasing pressure may give a higher yield of product and will produce a faster rate. Industrially high pressures are expensive to produce ( high electrical energy costs for pumping the gases to make a high pressure) and the equipment is expensive (to contain the high pressures

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7
Q

What effect would increasing pressure have on the yield of methanol?

CO (g) + 2H2(g) ⇌ CH3OH (g)

A

If pressure is increased the equilibrium will shift to oppose this and move towards the side with fewer moles of gas to try to reduce the pressure . The position of equilibrium will shift towards the right because there are 3 moles of gas on the left but only 1 mole of gas on the right, giving a higher yield of methanol.

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8
Q

Effect of Concentration on Equilibrium

I2 + 2OH- ——— I - + IO- + H2O

Brown to colorless

A

Increasing the concentration of OH- ions causes the equilibrium to shift to oppose this and move in the forward direction to remove and decrease the concentration of OH- ions

The position of equilibrium will shift towards the right, giving a higher yield of I- and IO-.

( The color would change from brown to colorless) Adding H+ ions reacts with the OH- ions and reduces their concentration so the equilibrium shifts back to the left giving brown color

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9
Q

Effect of Catalysts on Equilibrium

A

A catalyst has no effect on the position of equilibrium, but it will speed up the rate at which the equilibrium is achieved. It does not effect the position of equilibrium because it speeds up the rates of the forward and backward reactions by the same amount.

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10
Q

Haber process

eqm importance

A

N2 + 3H2 ⇌ 2NH3 H = -ve exo

T= 450oC, P= 200 – 1000 atm, catalyst = iron

Low temp gives good yield but slow rate: compromise temp used

High pressure gives good yield and high rate: too high a pressure would lead to too high energy costs for pumps to produce the pressure

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11
Q

Contact process

eq+ eqm importance

A

Stage 1

S (s) + O2 (g) —— SO2 (g)

Stage 2

SO2 (g) +½O2 (g) ⇌ SO3 (g)

T= 450oC, P= 1 or 2 atm, catalyst = V2O5

Low temp gives good yield but slow rate: compromise moderate temp used

High pressure only gives slightly better yield and high rate: too high a pressure would lead to too high energy costs for pumps to produce the pressure

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12
Q

Production of methanol from CO

eqm importance

A

CO (g) + 2H2(g) ⇌ CH3OH (g) Exothermic

T= 400oC, P= 50 atm, catalyst = chromium and zinc oxides

Low temp gives good yield but slow rate: compromise temp used

High pressure gives good yield and high rate: too high a pressure would lead to too high energy costs for pumps to produce the pressure

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13
Q

Hydration of ethene to produce ethanol

A

CH2 =CH2 (g) + H2O (g) ⇌ CH3CH2OH(l) exo

T= 300oC, P= 70 atm, catalyst = conc H3PO4

Low temp gives good yield but slow rate: compromise temp used

High pressure gives good yield and high rate: too high a pressure would lead to too high energy costs for pumps to produce the pressure High pressure also leads to unwanted polymerisation of ethene to poly(ethene)

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14
Q

carbon neutral

A

The term carbon neutral refers to “an activity that has no net annual carbon (greenhouse gas) emissions to the atmosphere”

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15
Q

Example 3

H2 (g) +Cl2 (g)——— 2HCl (g)

In a container of volume 600cm3 there were initially 0.500mol of H2 and 0.600 mol of Cl2 .

At equilibrium there were 0.200 mol of HCl. Calculate Kc

A
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16
Q

N2 (g) + 3H2 (g )—- 2 NH3 (g)

Initially there were 1.50 moles of N2 and 4.00 mole of H2, in a 1.50 dm3 container. At equilibrium 30% of the Nitrogen had reacted. Calculate Kc

A
17
Q

H2 (g) + Br2 (l) ——2HBr (g)

0.200 mol of H2 and 0.200 mol of Br2 are mixed and allowed to reach equilibrium. If Kc = 0.210 calculate the equilibrium amounts, in mol, of each substance.

A
18
Q
A