Key Question #11 - consumed by the reaction 52 a An...

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Lesson 11 Key Questions 50) The reaction is a two-step reaction. At the first step the reaction the NO combines with O 2 to form N 2 + O 2 . As the concentration of the starting materials decrease to form products the remaining reaction slows down. When the concentration is at its highest, that is when most collisions occur. 51) The first method would be to increase the temperature of the water. We learned from the text that by increasing the kinetic energy the molecules have more vibration, therefore more collisions would occur. The second method is to crush the lump of sugar into small granules. This increases the surface area of the solid. In a heterogeneous mixture the increase in surface area increases the rate of the reaction. The granules should dissolve faster than the big lump of sugar. The third method would be to use a catalyst. A catalyst is any reagent that increases the rate of reaction without being
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Unformatted text preview: consumed by the reaction. 52) a) An increase in temperature would increase the energy of the system closer to the activation energy and speed up the reaction. b) The effect of a temperature increase on the rate constant of the reverse reaction would also be an increase in the rate of reaction. Increasing the temperature increases the rate of the reverse reaction to a greater extent than it does the rate of the forward reaction. 53) a) The heat of the reaction can be expressed as H=(H f products ) – (H f reactants ) = (-110.0 kJ/mol + 34.0 kJ/mol) - (-393.5 kJ/mol + 90.4 kJ/ mol) =227.1 kJ/mol b) Activation energy reverse = Activation energy forward- H forward =(135 kJ/mol – 227.1 kJ/mol) = -92.1 kJ/mol c) 54) Experiment #4 can be found on the next pages....
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Key Question #11 - consumed by the reaction 52 a An...

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