In the intermolecular forces lab you destroyed the \"slime\" by adding sulfuric

Question

In the intermolecular forces lab you destroyed the "slime" by adding sulfuric acid. Describe the chemistry that was taking place during this step. In the first kinetics experiment we were able to calculate a rate law and rate constant for the relationship between the concentration of crystal violet and the time (but in reality this was a pseudo rate constant) for the experiment because we did not actually include all of the reactants Did the rate increase or decrease over time? Circle one. How is it that we were able to disregard the other reactant (OH^-) in our calculations? In the second kinetics experiment we used the method of initial rates to determine reaction order and examine reaction mechanism. Describe the effects of the catalyst and the change in temperature on the rate of reaction? Explain the basis for one of these effects using the Arrhenius equation. Do not explain math here. Explain the molecular basis for the effect.

Explanation / Answer

4) Sulphuric acid which is a strong acid disrupts the Hydrogen bonding in the molecule which accounts
   for attraction forces in the molecule.

5) If the concentration of one of the two reactants is significantly higher than the concentration of another, we can assume that particular reactant's concentration to be constant in the reaction. So, as time passes rate will decrease.
   Extra complications can arise if certain amounts of each reactant are required to determine the reaction rate.
  To avoid more complicated, expensive experiments and calculations, we can use the pseudo-1st-order reaction, which involves treating a 2nd order reaction like a 1st order reaction. This can be done by assuming
  the concentration of a reactant whose value is signifcantly high to be constant when compared with the other.
  This is how we disregard the OH- (the other reactant ) in the calculation.

6) A catalyst increases or decreases the rate of the reaction depending on number of collisons between/among
reactant molecules. Increasing the temperature increases reaction rates because of large increase in the number of high energy collisions which result in a reaction.
   To increase the rate of a reaction you need to increase the number of successful collisions. One way of doing this is to provide an alternative way for the reaction to happen which has a lower activation energy.

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