Determining the Rate of a Chemical Reaction _ Effect of Concentration. Of interest here is the reaction of potassium permanganate with oxalic acid. This is quite a complex oxidation reduction reaction.

In this experiment, you’ll investigate the effect of concentration and temperature on the rate of the reaction between solutions of potassium permanganate (KMnO 4, an ionic compound) and oxalic acid (H2C2O4, a molecular compound). 5 H2C2O4 (aq) + 2 MnO 4 - (aq) + 6 H + (aq) → 2 Mn 2+ (aq) + 10 CO 2 (aq) + 8 H2O (aq)

Changes in concentrations of individual reactants and the effect on the rate can be expressed mathematically through the rate equation (1): rate= k[H2C2O4]x [KMnO4]y (1) In this equation, k is the rate constant which only varies with changes in temperature.

The purpose of this analytical laboratory experiment is to determine the unknown concentration of potassium permanganate (KMnO4) solution by finding its absorbance through the use of spectrophotometer.

To elucidate the rate law of the reaction, we are to study the effect of Mn(III) complex concentration on the overall decomposition rate. Therefore, we make a series of solution which consist of species in different concentration while their ratio is maintained to be the same. We record the decay of the Mn(III) concentration in time.

Surface area, concentration and pressure all have the same effect on reaction rate (an increase leads to a faster reaction rate). This is because in each case an increase in the property leads to an increase in the number of collisions in that phase of matter.

Jan 26, 2023 · I'm writing a lab report investigating the effects of temperature on the rate constant in the reaction between potassium permanganate and oxalic acid. For my practical I've measured the time of colour change (purple to colourless). I've confirmed that the rate expression is: $$\mathrm{rate}=k[\ce{KMnO4}][\ce{H2C2O4}]$$

Jun 21, 2024 · In summary, the experiment investigates the reaction rate between potassium permanganate and hydrogen peroxide, focusing on how varying concentrations of the reactants affect the speed of the reaction.

In this experiment, the effect of temperature and concentration on the rate of a chemical reaction will be studied. The reaction chosen, frequently termed the “clock reaction”, is actually a series of consecutive reactions represented by the following equations:

This reaction al so involves the concentration of oxalate ion, wh i ch is itself dependent upon the acidity of the sol ution. The rate of the reaction is then determined by reaction 5, whose rate should be exnressed by the equation: (7)