'Nh3 g' diaporamas de présentation

Kinetics and Equilibrium again

Kinetics and Equilibrium again. Kinetics and the Rate constant. Equilibrium constants Kc and Kp. Acids and alkalis and pH. Curves and neutralisation. Buffers. Revised: 6-Jun-14. Need to do:. clarify graphs Expand rate-limiting step & mechanism. Remember:.

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The Gaseous Phase

The Gaseous Phase. The three phases of matter, solids, liquids and gases, have different characteristics. A gas expands to fill any container it occupies A liquid has a fixed volume but takes the shape of the volume of the container it occupies A solid has both fixed volume and shape.

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Reactions in Aqueous Solution

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THERMODYNAMICS

THERMODYNAMICS. Chapter 19 . SPONTANEOUS PROCESS. ? A process that occurs without ongoing outside intervention . Examples Nails rusting outdoors. 2H 2 (g) + O 2 (g) 2H 2 O(g). Ice melting at room temperature. Expansion of gas into an evacuated space.

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Thin film deposition: key performance indices

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Chapter 9

Chapter 9. Gases: Their Properties and Behavior. Gases and Gas Pressure. Properties of Gases. Gases mix completely with one another to form homogenous mixtures Gases can be compressed (keyboard cleaner) Gases exert pressure on what ever is around them (balloon, film canister)

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Calorimetry

Calorimetry. Calorimetry is used to measure heat capacity and specific heats. calorimeter: an instrument that measures heat changes for physical and chemical processes insulated , so the only heat flow is between reaction system and calorimeter. Calorimetry. Coffee-Cup Calorimeter

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Acid-Base Concepts -- Chapter 15

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International Baccalaureate Chemistry

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Chapter 4 module 2: Treatment of excreta for safe reuse

Chapter 4 module 2: Treatment of excreta for safe reuse. How should urine and faeces be treated for safe handling and reuse in crop cultivation? How can organic material from households be co-treated? . Incineration. Quick and simple method Faeces are applied in the stove

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Gas Stoichiometry Ideal Gas Law

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T h e r m o d y n a m i c s

T h e r m o d y n a m i c s. The study of energy transfers and chemical driving forces. Enthalpy. Enthalpy (H) ? the total E (KE + PE) of a system at constant P when a system reacts, ?H = H final - H initial for a chemical reaction: ?H rxn = H products - H reactants. ?H.

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Chapter 5 Chemical Reactions and Quantities

Chapter 5 Chemical Reactions and Quantities. Mole Relationships in Chemical Equations. Mole-Mole Factors. Show the mole-to-mole ratio between two of the substances in a balanced equation Use the coefficients of two substances in the equation. Writing Mole Factors.

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Nuclear Fuel Production Fissile Nuclei Uranium and Plutonium

Nuclear Fuel Production Fissile Nuclei Uranium and Plutonium 235 U 239 Pu Uranium Two isotopes 99.3% 238 U not useful for energy production 0.7% 235 U useful for energy production For a nuclear reactor: Need 4% 235 U For a fission bomb: Need 90% 235 U

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Chapter 8 Solutions

Chapter 8 Solutions. 8.2 Electrolytes and Nonelectrolytes. Solutes and Ionic Charge. In water, strong electrolytes produce ions and conduct an electric current weak electrolytes produce a few ions nonelectrolytes do not produce ions. Strong Electrolytes. Strong electrolytes

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Calculating ? H using molar heats of formation

Calculating ? H using molar heats of formation. Chem 12. If 1 mol of compound is formed from its constituent elements, then the enthalpy change for the reaction is called the enthalpy of formation, ? H o f . Standard conditions (standard state): 1 atm and 25 o C (298 K).

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Chapter 5 Chemical Reactions and Quantities

Chapter 5 Chemical Reactions and Quantities. 5.7 Mole Relationships in Chemical Equations. Law of Conservation of Mass. The Law of Conservation of Mass indicates that in an ordinary chemical reaction, Matter cannot be created nor destroyed.

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Entropy (S)

Entropy (S). A measure of the amount of disorder of a system Nature tends to move towards more disorder (higher entropy) Which has the greater entropy in each pair? NH 3 (g) or NH 3 (l) NH 3 (g) or NH 3 ( aq ) CO 2 (s) or CO 2 (g) KBr (s) or KBr (l).

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Haber Process

Haber Process. Fritz Haber. The Haber Process is used to make ammonia, NH 3 :. 3 H 2 (g) + N 2 (g) ? 2 NH 3 (g) + heat. Ammonia ranks in the top five of all chemicals in terms of total mass produced. It is used to make fertilizer and explosives (e.g.- TNT) . .

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