2. xA + yB C + D
Rate of the reaction be written as:
Rate = K[C]*[D]/ [A]x[B]y
3. If different students use different concentrations of same reactants definitely there will be a difference in rate of the reaction as the rate of the reaction depends on the concentration of reactants.
4. Two ways to speed up a reaction is:
1) By using a catyst
2) By increasing the temperature.
Two ways to slow down the reaction is:
1) By decreasing the temperature
2) By decreasing the pressure.
Both these ways slows down the collision between molecules.
5) For toxic chemicals the pictogram present will be the one with skull and for corrosive chemical it will be the one with 2 test tubes spilling on hands.
Kinetics of the permanganate and Oxalate Reaction. 2. Write out the general rate law for today's...
Part A The rate of the reaction in terms of the "disappearance of reactant" includes the change in the concentration of the reactant, the time interval, and the coefficient of the reactant Consider the following reaction: 2A + 3B 3C + 2D The concentrations of reactant A at three different time intervals are given. Use the following data to determine the average rate of reaction in terms of the disappearance of reactant A between time=0s and time = 20 S....
2. When using the method of initial rates to determine the reaction order of each individual reactant, why must data only be used in which one reactant is changing concentration but not the other reactants? 3. Briefly explain why the number of total drops being mixed in each experiment is kept constant throughout all five experiments. 4. Sketch a molecular‐level picture that illustrates why reaction rate increases when the concentration of a reactant is increased. Note – this might be...
answer the questions Experiment 1084-04: lodine Clock Reaction Purpose Determine the rate law for an iodine clock reaction and study the influence of st on that reaction abruptly that it can be as startling as the sudden sound of an alarm clock, hence the clock reaction Background Information chemical equations can be written for chemical reactions, only some will proceed while others do not. Among the ones that do proceed some reactions occur as soon as reactants are mixed, while...
2. Kinetics of an Oscillating Reaction Oscillating reactions are a special kind of chemical reactions and are characterized by an elementary reaction in which at least one of the reactant is also a product. An example of a series of elementary reactions of an oscilating reaction is below: ka (a) Identify the autocatalytic reacton i.e, a reaction in which the products and reactants share atleast one common ingredient) (b) Identify the reactants, intermediates, and products for the overall reaction described...
Question 2 Integrated rate law The other method to establish rate laws is to measure the remaining concentrations of a reactant at different times during the reaction. The concentrations of reactant for reaction A 2B + C measured as a function of time at 25°C are listed in the following table. t(s) 15 25 35 45 55 [A] (M) 0.30 0.26 ? 0.20 0.17 (s) [A] (M) 65 0.15 75 0.13 85 0.11 95 0.10 105 0.09 (a) Use Excel...
need help thanks Write the rate law for the reaction: CH469) + 2 02(g) + 2 H2O(1) + CO2(g) if the order of all reactants is one. Complete the equation using brackets, I ), to represent concentration. Click in the answer box to activate the palette. rate = Write a valid equilibrium constant expression for the reaction below. Remember to use brackets, I). for concentrations, and use exponents where needed. Click in the answer box to activate the palette. H...
Determination of the Rate Law for the Iodination of Acetone in Acidic Solution I conducted an experiment to determine initial concentrations of reactants, reaction times, and reaction orders for the iodination of acetone.... here is my data followed by some questions... help please?? 1. How do you double the concentration of one of the reactant solutions in each experiment? What reagent should you use to control the total volume of each experiment? 2. Could you reduce the concentration of a...
1. Determine which reactant is limiting the rate of reaction. Justify the answer. 2. Determine the rate of reaction in trial 1,2,3 3. What are the experimental values for n and m? Thank you so so much for your help. Experiment: Reaction Kinetics Aim: To find the reaction orders and rate constants for the following reaction: 3 H2C2O4(aq) + 2 MnO4 (aq) --> 6 CO2+ 2 OH(aq) + 2 H2O + 2 MnO2s In other words to obtain m, n,...
just one example/demonstration! Data needed to be calculated is in highlighted in green boxes. And I highlighted in red an equation (not sure if thats what you use to calculate it) And ignore the lab instructions on completeing a graph!! I already know how to do that in excel, just curious how Ln (relative rate) and 1/T in K^-1 is calculated by hand* here is the rest of that lab leading up to the question as I know its typically...
will work with up to 3 partners (similar to a lab group) to prepare a written report which analyzes kinetic data that has been provided to you. All student groups will receive data for the hypothetical reaction aAlE) products where a is a numeric variable and A is a chemical variable. The reaction therefore has the form of a decomposition reaction, in which a single substance forms one or more new substances. For consistency, all concentrations start out at 1.000...