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 0 answersPost by Marian Iskandar on April 30, 2013I got 170 KJ, so I'm not sure how the professor got 105 kj...any suggestions would help. I tripled check my calculations.

### Temperature Effects, Reaction Rate Theory, Catalysis

• For most reactions as T increases, so does rate

• Kinetic molecular theory can explain this

• Arrhenius equation for temperature effects: k = Ae-E/RT ; A is an orientation factor; E is the activation energy

• Do calculations of E and A from exptl. Data

• Catalyst: accelerates rate without being consumed in reaction

• Catalysts can be homogeneous e.g. acid in hydrolysis of esters; heterogeneous, solid metallic catalysts in reaction of nitrogen with hydrogen to make ammonia

• Enzymes: common biochemical catalysts, e.g. in digestion

### Temperature Effects, Reaction Rate Theory, Catalysis

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

• Intro 0:00
• Effects of Temperature on Reaction Rates 1:05
• Common Examples
• Arrhenius' Equation 6:40
• Activation Energy
• Example: Nitrogen Pentoxide
• Reaction Rate Theory 15:20
• Activated Complex and Transition State
• Example: Methyl Bromide and Hydroxide Ion
• Calculating Activation Energy 22:32
• Plotting ln K and Inverse T
• Catalysis in Practice 25:33
• Example: Catalytic Converter
• Example: Oil Refinery
• Acid Catalysis of Ehtyl Acetate Hydrolysis 31:48
• Example
• Industrial Production of Ammonia 35:54
• Haber Bosch Process
• Industrial Production of Sulfuric Acid 41:02
• Series of Processes
• Enzymes as Catalysts 45:59
• Example: Amino Acid
• Example: Protein