O2 g - PowerPoint PPT Presentation
Energy
Energy. The capacity to do work or to produce heat. System and Surroundings. System : That on which we focus attention Surroundings : Everything else in the universe Universe = System + Surroundings. Figure 6.9. Components of internal energy (E). Components of Internal Energy.
By Rita
Special Note: Endothermic Reactions
Special Note: Endothermic Reactions. As long as the total entropy is slightly positive, endothermic reactions will go forward Spontaneity is determined by the increase in the entropy of the system, NOT a decrease in the ENERGY (heat) of the system!. . Equilibrium.
By emily
Hess's Law
Hess's Law. Hess’s law. Hess’s Law states that the heat of a whole reaction is equivalent to the sum of it’s steps. For example: C + O 2 CO 2 (pg. 165) The book tells us that this can occur as 2 steps C + ½O 2 CO H = – 110.5 kJ CO + ½O 2 CO 2 H = – 283.0 kJ.
By niveditha
Reaction Types
Reaction Types. Combination (Synthesis) Reactions. Two or more substances combine to form a new compound. A + X AX. Reaction of elements with oxygen and sulfur Reactions of metals with Halogens Synthesis Reactions with Oxides There are others not covered here!.
By damita
Chemical Kinetics
Chemical Kinetics. CA Standards. Collision Model. Collisions must have enough energy to produce the reaction (must equal or exceed the activation energy). Reactants must have proper orientation to allow the formation of new bonds. Activation Energy.
By lola
Chemical Equations and Stoichiometry
Chemical Equations and Stoichiometry. Chapter 4. Chemical Equations. 2H 2 (g) + O 2 (g) 2H 2 O(g). Chemical Equations. 2H 2 (g) + O 2 (g) 2H 2 O(g) The materials you start with are called Reactants . Chemical Equations. 2H 2 (g) + O 2 (g) 2H 2 O(g)
By raleigh
Blast Furnace Reactions
Blast Furnace Reactions. Carbon oxidised by hot air:. Carbon (s) + oxygen (g) carbon dioxide (g). C (s) + O 2 (g) C O 2 (g). Carbon oxidised by carbon dioxide:. Carbon (s) + carbon dioxide (g) carbon monoxide (g). C (s) + CO 2 (g) 2C O (g).
By libitha
Types of Chemical Reactions
Types of Chemical Reactions. Combination/Synthesis Reaction. General Equation: R + S RS Reactants: Generally two elements or two compounds. Probable Products: A single compound Example: 2Mg (s) + O 2(g) 2MgO (s ) Practice problems pg 214 #13-14. Decomposition. General Equation:
By pooky
2.0 0.5 0.20 5.0 0.012
For the reaction 2A + B {image} C + 2D at 35°C, the value of kf is 3.0 x 10-3 M-2•s-1 and the value of kr = 1.5 x 10-2 M-2•s-1. Calculate the value of Kc for this reaction. 2.0 0.5 0.20 5.0 0.012.
By mercia
Chapter 12 Review “Stoichiometry”
Chapter 12 Review “Stoichiometry”. Chapter 12 Review. The first step in most stoichiometry problems is to ____. How many liters of hydrogen gas are needed to react with CS 2 to produce 2.50 L of CH 4 at STP: 4H 2(g) + CS 2(l) → CH 4(g) + 2H 2 S (g) ?
By maren
WRITING CHEMICAL EQUATIONS
WRITING CHEMICAL EQUATIONS. Reactants (starting materials) Products (ending materials) (g) = gas (l) = liquid (s) = solid (aq) = aqueous D = heat = yields (dissolved in water) X = catalyst + = combines
By violet
Sodium hydroxide and hydrobromic acid
Sodium hydroxide and hydrobromic acid. NaOH (aq) +HBr (aq) NaBr (aq) +H 2 O (l). OH - (aq) +H + (aq) H 2 O (l). Propane combusts. 2C 4 H 10(g) +O 2(g) 8CO 2(g) + 10H 2 O (l). 2C 4 H 10(g) +O 2(g) 8CO 2(g) + 10H 2 O (l). Potassium and water. 2K (s) +2H 2 0 (l) 2KOH (aq) +H 2(g).
By darva
Information given by chemical equations
Information given by chemical equations. 2 C 6 H 6 (l) + 15 O 2 (g) 12 CO 2 (g) + 6 H 2 O (g). In this equation there are 2 molecules of benzene reacting with 15 molecules of oxygen to produce 12 molecules of carbon dioxide and 6 molecules of water .
By lee
Increasing energy with temp?
Increasing energy with temp?. The added energy in a substance that occurs as temperature increases is stored in modes of motion in the substance For any molecule – modes are vibration, translation, and rotation Solid bond vibrations Gases translation Liquid water – complex function….
By cruz
Chapter 15
Chapter 15. Equilibrium. Equilibrium. N 2 + 3 H 2 2 NH 3 Both reactions occur, Closed system No change in Equilibrium reached no matter what direction. Write:. Rate law for forward Rate = Rate Law for reverse Rate =. Then…. Rate f = Rate r. So…. K f. =. k r. Or. k c.
By raziya
Energetics
Energetics. IB Topics 5 & 15 PART 2: Calculating H via Bond Enthalpies & Hess’s Law. Above: thermit rxn. BOND ENTHALPIES. Enthalpy change ( H) can also be calculated directly from bond enthalpies .
By adonia
Hess's Law
Hess's Law. Hess’s law. Hess’s Law states that the heat of a whole reaction is equivalent to the sum of it’s steps. For example: C + O 2 CO 2 The book tells us that this can occur as 2 steps C + ½O 2 CO H = – 110.5 kJ CO + ½O 2 CO 2 H = – 283.0 kJ.
By jabari
Hess’s Law
Hess’s Law. A consequence of the 1 st of Thermodynamics (conservation of energy). If a reaction is the sum of 2 or more reactions, then the H of the overall reaction is the sum of the H of the constituent reactions.
By marcin
Which of the following reactions could be classified as exothermic ?
Which of the following reactions could be classified as exothermic ?. 2H 2 (g) + O 2 (g) 2H 2 O (g) + 241.8 kJ reactants + energy products N 2 (g) + O 2 (g) + 43kcal 2NO(g) reactants products + energy. ANSWER = A & D because …
By gayora
Equilibrium Systems and Stress
Equilibrium Systems and Stress . Chemical Equilibrium. Chemical Equilibrium When the rates of the forward and reverse reactions are equal in a chemical reaction The concentration (amount) of reactants and products of the reaction remains the same Ex: 2CO (g) + O 2(g) ↔ 2O 2(g).
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