1: Kinetic Factors Problem Sta predictable from the balanced equation? The React

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1: Kinetic Factors Problem Sta predictable from the balanced equation? The Reaction: Permanganate lon Reduced by Oxalic Acid In this experiment you will be studying the reaction between permanganate, Mno, and oxalic acid G204Hz, in acid solution. The overall balanced reaction equation is: 2MnO41 (aq) + 5Go4H2(aq) + 6H.(aq) 2 Mn®(aq) + 10 COdaq) + 8H20(1) Experimental (10 pts) Your lab notebook should contain the following data and copies of those pages are then included in the lab report. I. Watching the Reaction Obtain a dropper bottle for each of the stock solutions 0.0014 M K:MnO, 0.20 M C:04H2 and 2.0 M H2504. Put about 30 mL of distilled water in a 100 mL beaker. Get a clean plastic pipet for the distilled water. You will be making various mixtures of these four solutions by counting drops. Be careful that the droppers are not switched between solutions during any of the a. b. Take three clean, distilled-water rinsed, large test tubes and label them 1 through 3. You will be doing experiments three runs at a time and need to keep track of each run. These can be supported in a test tube rack or in a 250 mL beaker while you observe them. Viewing them against a white background is advised. Make up the three solutions as described below. Mix each by flicking the bottom of the tube while holding its top securely. Observe these solutions for about 10 minutes and record your observations. You should include a data table with these volumes in your lab notebook. c. Drops of Stock Solutions H20 H2S04 Run # 1A 2A. KMnO4 15 15 15 C204H2 15 25 10 15 Data Collection: Effect of H' Concentration a. In the experimental runs from here on, you will be timing how long it takes for all the MnO II. 1 ions to react by watching the color fade. The recommended procedure is as follows: Dump the current contents of your test tubes into your waste beaker and rinse each a few times with about 1 mL of water. The rinse water can go down the drain. Shake out excess water Add the stock solutions to each tube as called for except for the C204H2. Then quickly add the drops of Cz04H2 to each tube, mix by flicking, and record this as the starting time. Also record the time when the color has faded. Sample Data Table: This data table should be copied into your laboratory notebook. You will not receive credit for data written on this page. b. 1: Kinetic Factors

Explanation / Answer

PROBLEM:

# Factors effecting rate of reaction:

·         Temperature Effects: The rate of reactions increases with increasing temperature.

·         Phase and Surface Area Effects: If two reactants are in the same fluid phase, their particles collide more frequently, so reaction rate increases. Surface area effects to increase reaction rates when surface are is more.

·         Solvent Effects: The nature of the solvent can also affect the reaction rates of solute particles. Solvent viscosity is also important in determining reaction rates. The reaction rates of most reactions decrease rapidly with increasing solvent viscosity.

·         Catalyst Effects: Catalysts are highly selective, they often determine the product of a reaction by accelerating only one of several possible reactions that could occur.

## All this above factor we can calculate from balance equation. If we are able to measure the changes then obviously we are able to predict. If any factor change the condition for the equilibrium also change. So, we are able to calculate the changes (i.e. rate of the reaction).

### Experimental part:

·         If you see the given reaction you will find that the reaction depend upon pH (i.e. concentration of H+).

·         Concentration of H+ increases the rate of reaction increases.

·         The pink color will be going to fade faster when pH is low (i.e. high H+ concentration).

·         Time vs concentration of H+ you have to plot. From the plot you are able predict that concentration of H+ will affect the rate of the reaction.

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