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Energy

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
(332 views)

Special Note: Endothermic Reactions

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
(318 views)

Hess's Law

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
(354 views)

Reaction Types

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
(216 views)

Chemical Kinetics

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
(142 views)

Chemical Equations and Stoichiometry

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
(153 views)

Blast Furnace Reactions

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
(3449 views)

Types of Chemical Reactions

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
(177 views)

2.0 0.5 0.20 5.0 0.012

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
(358 views)

Chapter 12 Review “Stoichiometry”

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
(889 views)

WRITING CHEMICAL EQUATIONS

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
(476 views)

Sodium hydroxide and hydrobromic acid

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
(535 views)

Information given by chemical equations

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
(269 views)

Increasing energy with temp?

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
(96 views)

Chapter 15

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
(167 views)

Energetics

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
(202 views)

Hess's Law

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
(218 views)

Hess’s Law

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
(129 views)

Which of the following reactions could be classified as exothermic ?

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
(106 views)

Equilibrium Systems and Stress

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).

By carol
(219 views)

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