E.g. CH3COCH3 + I2 ---> CH2ICOCH3 + HI = Rate = K[CH3COCH3][H+]
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Finding The Rate Constant, K
E.g. 2NO + O2 ----> 2NO2 = Rate=k[NO]2[O2] = 28x10-4 = k[2x10-3]2 x [1x10-3], k=28x10-4/(2x10-3)2(1x10-3)
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The Effect of Temperature on K
The rate constant is the part of the equation that changes when the temperature changes, the larger the value of K, the faster the reaction will happen.
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Why the Rate Constant depends on temperature
Temperature is the measure of kinetic energy. Particles will only react together if their collisions have enough energy to start bond breaking, this is called the Activation Energy.
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Rate Determining Step
A + B + C ---> Y + Z - Any reaction that involves any of the species in the equation will be faster than the ones that aren't.
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Other cards in this set
Card 2
Front
E.g. 2NO + O2 ----> 2NO2 = Rate=k[NO]2[O2] = 28x10-4 = k[2x10-3]2 x [1x10-3], k=28x10-4/(2x10-3)2(1x10-3)
Back
Finding The Rate Constant, K
Card 3
Front
The rate constant is the part of the equation that changes when the temperature changes, the larger the value of K, the faster the reaction will happen.
Back
Card 4
Front
Temperature is the measure of kinetic energy. Particles will only react together if their collisions have enough energy to start bond breaking, this is called the Activation Energy.
Back
Card 5
Front
A + B + C ---> Y + Z - Any reaction that involves any of the species in the equation will be faster than the ones that aren't.
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