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Found 14 results

  1. Please help me! I am supposed to design my chemistry IA, but I honestly have NO IDEA on how to even start. Chemistry is my worst subject and I have a lot of trouble in understanding it. I always try so hard on my IA's but I always end up making B's. I have to decide on one factor that affects the rate of a reaction to investigate in my design lab IA and this lab is supposed to be easily reproducible. Here's my IA guidelines: Aspect 1 includes: Formulating a focused problem/research question and identifies the relevant variables. Aspect 2: Designs a method for the effective control of the
  2. I can't seem to remember them well and have this information stay in my mind for prolonged periods of time!
  3. Hello! next year is my last year so it is the year for me to finish my EE. I need a little help with the research question. So my topic is about the making of biodiesel from waste cooking oil and before the actual process of turning waste cooking oil into biodiesel, the free fatty acids in cooking oil needs to be esterified first to lower the cooking oil's acid value. I decided to title my EE "the kinetics of FFA esterification in waste vegetable oil". there are several things that can be independent variables such as methanol:oil ratio, temperature and the concentration of the catalyst,
  4. So my research question was to determine activation energy of HCl and Sodium Thiosulfate, but I changed the concentration of Sodium Thiosulfate instead of the HCl -- I just found out that the H+ ions in HCl catalyse the reaction???? IM NOT SURE WHAT TO DO !!! HELP OH MY GOD
  5. The question is this: at 25 degrees C, 200 cm^3 of 1 mol dm^3 of nitric acid is added to 5g of magnesium powder. If experiment is repeated using same mass of magnesium powder, which conditions will result in the same initial reaction rate? I chose 100 cm^3 of nitric acid , 2 mol dm^3 as conc and 25 degrees C. However, the answer is 100 cm ^3 of 1 mol dm^3 HNO3. How is it the case? If it is so, then in 200 cm^3, there would be 2 mol dm^3. As there is a higher conc, then the reaction rate should be higher, so it doesn't give the same rate?
  6. Guest

    Kinetics/Equilibrium

    Please help me understand this question!
  7. Guest

    Equilibirum

    Please help me understand why the answer is D.
  8. Hello! I try to find the mechanism for the following chemical reaction: 2KI(aq)+ H2O2(aq) + H2SO4(aq) Ã K2SO4(aq) + I2(aq)+ H2O(l) The rate equation I got is as following: Rate = k * [KI] * [H2O2] * [H2SO4] I was thinking about the following:2KI+ H2SO4 Ã K2SO4 + 2HI2HI+ H2O2 Ã I2 + 2H2O But it does not fit my rate equation. Maybe you can give me a hint? I think I am doing something wrong here. Thank you in advance!
  9. Hello, I have a chemistry SL Kinetics Design Lab due tomorrow The formula given is You will be investigating a factor that affects the rate of the following reaction: CaCO3(s) + 2H+(aq) ïƒ Ca 2+(aq) + CO2(g) + H2O(l) o Identify a problem you wish to solve and frame your problem as a hypothesis, you o Identify your variables (MV, RV, and relevant CVs) o Design an experiment that will enable you to test the validity of your hypothesis. must be able to explain the hypothesis. Assume you are given any equipment you need (available in any high school laboratory).  Be sure you
  10. Hi, I'm currently doing an DCPCE IA for kinetics and I'm a bit confused So the aim is ' to investigate the rate of this reaction as a function of the sodium thiosulfate concentration.' Basically in the experiment we took different sodium thiosulfate concentrations, and a constant amount of HCl and reacted them. We then timed how long it took for us to be unable to see the bottom (colour change). So to find the rate of reaction, do I use 1. (rate = 1/time) or 2. (rate of reaction = - change in reactant concentration/time taken) or 3. (rate = k [A)mn)? I'm thinking that I don't use 2. bec
  11. Hi all, So I've recently been trying to calculate the rates of reaction, but I've been slightly confused as to how I should go about it. Should I use this equation: rate of reaction = 1 / t (t is time in minutes) OR rate of reaction = concentration of reactant / time taken for reaction to occur Thanks in advance!
  12. Hello I would like to know if my method is suitable to determine the order of reaction of HCl. I was doing an experiment on a scale which was producing a CO2 gas. CaCO3+ 2HCl-> CaCl2+ CO2+ H2O I was recording mass of the substances HCl and CaCO3 every 20 secounds. (A decrease in mass is observable) Can i use the gradient of the tangent line from the initial weight and the first recorded weight 20 secounds later to determine the rate of reaction? (Did this reaction with 5 different HCl concentrations) These rate of reaction I could compare with the different HCl concentration to determine t
  13. 30 downloads

    Here are my notes on Kinetics for Chemistry.
  14. So I am going to start my chemistry IA soon and I was hoping for suggestions. Our IA deals w/ chem kinetics and I pretty sure that I'm just going to do something with temperature change. I was planning on changing the temperatures, finding the orders of the reactions, and then plotting an arrhenioius plot and finding the activation energy. I'm wondering if this seems like a good plan? And what solutions do you think would be the simplest to use?
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