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Exothermic, endothermic, rate of reactions
 

Exothermic, endothermic, rate of reactions

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The answers are at http://keyquestions.weebly.com

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    Exothermic, endothermic, rate of reactions Exothermic, endothermic, rate of reactions Document Transcript

    • Exothermic, Endothermic, Rate of Reactions<br />Notes<br />ExothermicEndothermicGives out heatTakes in heatBond formingBond breakingNegative ΔHPositive ΔH<br />EnergyEnergy<br />Activation energyEaProgress of reaction<br />Activation energyEaΔHΔH<br />Progress of reaction<br />ENDOTHERMICEXOTHERMIC<br />Increasing the rate of a reaction:<br />
      • Increase the temperature
      • Increase the pressure
      • Increase the concentration of the reactants
      • Increase the surface area of the reactants
      • Use a catalyst
      Workout questions<br />
      • Which of the following reactions are exothermic?
      • Melting
      • Boiling
      • Freezing
      • Evaporating
      • Which of the following is true of endothermic reactions?
      • There is more energy involved in bond breaking than bond forming
      • There is less energy involved in bond breaking than bond forming
      • More bonds are broken than formed
      • Fewer bonds are broken than formed
      • When an acid neutralizes a base, the beaker holding the solution feels warm. Why?
      • Heat is absorbed from the surrounding to break bonds
      • Heat is absorbed from the surrounding to form bonds
      • Heat is given out to the surrounding by breaking bonds
      • Heat is given out to the surrounding by forming bonds
      • In experiment X, an endothermic reaction takes place. Which of the following could be observed?
      • Bubbles
      • White ppt
      • The temperature of the mixture drops
      • There is strong smell evolved
      • With which of the following solutions of sulphuric acid does copper (II) oxide react with the fastest initial rate of reaction?
      • 50g of sulphuric acid in 200cm3 of water
      • 100g of sulphuric acid in 150cm3 of water
      • 150g of sulphuric acid in 100cm3 of water
      • 200g of sulphuric acid in 50cm3 of water
      • Calcium carbonate is reacted with excess aqueous hydrochloric acid to liberate carbon dioxide gas. How can the experiment be changed to liberate twice the amount of carbon dioxide gas?
      • Use more calcium carbonate
      • Use more hydrochloric acid
      • Heat the mixture using a bunsen burner
      • Increase the concentration of the hydrochloric acid solution
      • How does a catalyst work?
      • It increases the rate of a reaction by lowering the reaction’s activation energy
      • It increases the rate of a reaction by increasing the reaction’s activation energy
      • In increases the amount of product that can be formed
      • It eliminates the need to provide heat energy in order for a reaction to take place
      • Which of the following statements is true about a catalyst?
      • It always increases the enthalpy change of a reaction
      • It always decreases the enthalpy change of a reaction
      • It does not change the enthalpy change of a reaction
      • It can either increase or decrease the enthalpy change of a reaction
      • The enthalpy change of a reaction depends on
      • The number of bonds formed and broken
      • The amount of energy needed to form and break bonds
      • The surrounding temperature
      • The presence of a catalyst
      • When a solid X is added to the aqueous solution YZ2, the products are precipitates of XZ3 and Y.
      • Write a balanced chemical equation to show the reaction
      • Given the following information about the bond energies, calculate the total energy change that takes place when 1 mol of X is added to an excess of YZ2
      • kJ/molY-Z500X-Z600
      • Sketch a labeled energy profile diagram for this reaction
      • Suggest three possible ways to increase the speed of this reaction
      • ________________________________________________________________________
      • ________________________________________________________________________
      • ________________________________________________________________________
      • Suggest one possible way to increase the amount of product formed
      ________________________________________________________________________<br />
      • According to the information given,
      • CompoundΔH of combustion (kJ/mol)A- 2000B- 2500C- 500
      • Which compound has the most exothermic combustion reaction? Explain.
      • ________________________________________________________________________
      • Combustion reactions can never be endothermic. Explain why you agree/disagree with this statement.
      • ________________________________________________________________________
      ________________________________________________________________________<br />