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1. Name the 3 things that vapor pressure are dependent on.
2. Name the 3 things that are independent on.
3. What 3 factors affect principle?
4. Name the 5 characteristics of equilibrium.
5. Name the 3 characteristics of weaker intermolecular forces.
6. Name the 3 characteristics of stronger intermolecular forces
7. What does ICE stand for
8. What is chemical equilibrium
9. What does Le Chatelier's principle state
10. What is the Contact Process

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Le Chatelier's principle | Chemical equilibrium | Chemistry | Khan Academy

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Chem4Kidz (The Contact Process) [Chemistry Assignment]

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This is the result of a assignment I had to do for my Chemistry class having to explain an industrial process in a way that a person with minimal Chemistry knowledge (i.e. A child) could understand. So without further ado, I give you Episode 1 of Chem4Kidz Enjoy!

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What Is The Haber Process | Reactions | Chemistry | FuseSchool

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Understanding Chemical Equilibrium and Equilibrium Constant Kc

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Weaker intermolecular forces →	lower__________enthalpy of vaporization	higher__________ vapor pressure	_lower_________ boiling point

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Weaker intermolecular forces →	lower__________enthalpy of vaporization	higher__________ vapor pressure	_lower_________ boiling point

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pressure exerted by the particles in the vapor phase on it’s liquid at eq’m.

Independent of:

Surface area of liquid

Size of container

although it may take longer for equilibrium to be established in larger container

Dependent on:

Temperature

Nature of the substance

strength of intermolecular forces

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Stronger intermolecular forces →

_Higher_________enthalpy of vaporization

__lower________ vapor pressure

__higher________ boiling point

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The contact process is the current method of producing sulfuric acid in the high concentrations needed for industrial processes. Platinum used to be the catalyst for this reaction; however, as it is susceptible to reacting with arsenic impurities in the sulfur feedstock, vanadium(V) oxide (V2O5) is now preferred.

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The Haber Process combines nitrogen from the air with hydrogen derived mainly from natural gas (methane) into ammonia. The reaction is reversible and the production of ammonia is exothermic.

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Pressure-Increasing the pressure favors the reaction that produces the fewer moles of gas, and vice-versa.

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Temperature- Increasing the temperature always favors the reaction that consumes heat, and vice versa.

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Concentration-

When a substance is added, the stress is relieved by shifting equilibrium in the direction that consumes some of the added substance.

When a substance is removed, the reaction that produces that substance occurs to a greater extent.

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When a change (“stress”) is applied to a system at equilibrium, the system will shift its equilibrium position to counteract the effect of the disturbance.

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The Initial – Change – Equilibrium method of solving these types of problems is affectionately referred to as the ICE method.

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n order to write the equilibrium expression for a system in a state of equilibrium you need to know:
the balanced equation for the reaction and the phases (solid, liquid, gas, or dissolved) of each species involved in the reaction.

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For any reaction: aA + bB ↔ cC + dD at equilibrium at a given temperature, the constant, kc

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Directional-The same equilibrium mixture will result under the same conditions, no matter whether the rxn is started with all reactants, all products, or a mixture of both.

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Macroscopic-This refers to observable properties such as color and density; these do not change as they depend on the concentrations of the components in the mixture.

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Concentration- They are being produced and destroyed at an equal rate.

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Closed System-Prevents exchange of matter with surroundings, so equilibrium is achieved where both reactants and products can react and recombine with each other.

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Dynamic-The rxn has not stopped; the forward and backward rxns are still occurring (same rate).

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the state in which both reactants and products are present in concentrations which have no further tendency to change with time.