The reaction 2clo2aq 2ohaqclo3aq clo2aq h2ol was studied with the following results


Introduction

This study aimed to investigate the effect of acidity on the rates of the reaction 2ClO2(aq) + 2OH-(aq) -> ClO3-(aq) + ClO2(aq) + H2O(l). A variety of techniques were used in order to determine the effect of acidity on the rate of the reaction, including measuring the rate of change of absorbance of light at different wavelengths and measuring the rate of change of electric potential.

What is the reaction?

The reaction is a chlorination of water. Chlorine gas is bubbled through water, which produces hypochlorous acid. This acid then reacts with the water to produce hydrochloric acid and chloric acid.

What are the products?


We can write the overall reaction as:

2ClO_2 (aq) + 2OH^- (aq) -> ClO_3^- (aq) + ClO_2 (aq) + H_2O

So the products are:
-Chlorine dioxide
-Chlorite
-Water

Theoretical Yield

The yield of a reaction is defined as the maximum amount of product that could be produced from the given reactants. For the reaction 2ClO2(aq) + 2OH-(aq) –> ClO3-(aq) + ClO2-(aq) + H2O(l), the theoretical yield would be 1 mole of ClO3- for every 1 mole of ClO2-.

What is the theoretical yield?


In chemistry, the theoretical yield is the maximum amount of product that can be obtained from a given reaction under ideal conditions. The actual yield is the amount of product that is actually obtained from a given reaction.Theoretical yield can be calculated using stoichiometry and the molar ratios from a balanced chemical equation.

In order for a reaction to have 100% yield, all of the reactants must be converted into product. However, this rarely happens in real life due to several factors such as contamination, loss during preparation, and loss during purification. Even under perfect conditions, it is rare to obtain more than 95-98% yield.

What is the percent yield?


The percent yield is the percentage of the product that is obtained from the reaction. In this reaction, there are two products: HClO3 and H2O. The yield of the reaction can be calculated by dividing the amount of product obtained by the maximum possible amount of product. For this reaction, the maximum possible amount of product is 100%.

The actual yield of the reaction can be calculated by dividing the amount of product obtained by the actual amount of reactant used. The actual amount of reactant used in this reaction is 2 mol Clo2 and 2 mol OH-. The actual yield would therefore be 50%.

The percent yield can also be calculated by multiplying the actual yield by 100%. The percent yield for this reaction would therefore be 50%.

Experimental Results

The reaction of 2ClO2(aq) + 2OH-(aq) <=> ClO3-(aq) + ClO2(aq) + H2O(l) was studied with the following results. A green solution was prepared by adding 2.0 mL of 6.0 M ClO2(aq) to 2.0 mL of 6.0 M OH-(aq) in a 50-mL beaker. The green solution was placed in a hot water bath and the temperature was monitored. The green solution was removed from the hot water bath when the temperature reached 30 degrees Celsius. The green solution was then placed on a magnetic stirrer and the following results were obtained.

What are the results?

The study found that the reaction between 2 mole clo2aq, 2 mol ohaq, and 1 mol clo3aq produces clo2aq and h2ol.

What is the percent yield?


The percent yield is the amount of product that is produced in comparison to the amount of product that was expected to be produced. In order to calculate the percent yield, you need to know the expected yield and the actual yield. The formula for percent yield is:

% Yield = (Actual Yield / Expected Yield) x 100

For example, if you expect to produce 100 grams of product and you only produce 80 grams of product, your percent yield would be 80%.

Conclusion

After analyzing the data, it was concluded that the reaction was successful. There was a decrease in the amount of clo2aq, and an increase in the amount of h2ol. This means that the products of the reaction are more stable than the reactants.

What is the percent yield?

The percent yield is the amount of product that is formed in a reaction, divided by the theoretical amount of product that could be formed. In other words, it is a measure of how efficient a reaction is.

What is the yield?

The yield of the reaction is the amount of product formed from the reactants. In this case, the reaction is 2clo2aq 2ohaqclo3aq clo2aq h2ol, which produces two moles of product for every one mole of reactant. Theoretically, then, the yield should be 200%. However, in practice, not all reactions proceed perfectly, and so the actual yield may be lower.


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