Exciting Chemical Reaction: CS2 with Cl2

What is the percent yield for the given reaction?

If 5.82 g Cl2 is reacted with excess CS2 and 2.11 g of CCl4 is ultimately isolated, what is the percent yield for the reaction?

The percent yield for the given reaction is 70.37%

The percent yield calculation is explained below.

When considering the reaction of CS2 with Cl2 to form CCl4 and SCl2, it's important to calculate the percent yield to understand the efficiency of the reaction. In this case, the percent yield is found to be 70.37%.

The chemical equation for this reaction is: CS2 + 4 Cl2 → CCl4 + 2 SCl2. In this reaction, excess CS2 is the reactant, and the limiting reagent is 6.47 g of Cl2. To calculate the theoretical yield of CCl4, we start by determining the moles of Cl2 present.

Using the molar mass of Cl2 (71 g/mol) and the molar mass of CCl4 (154 g/mol), we can calculate the theoretical yield as follows:

6.47 g Cl2 * 1 mol Cl2 / 71 g Cl2 * 1 mol CCl4 / 4 mol Cl2 * 154 g CCl4 / 1 mol CCl4 = 6.47 g * 154 g / 71 * 4 g = 3.51 g

Next, we calculate the percent yield using the formula: percent yield = actual yield / theoretical yield * 100. Since the actual yield is 2.11 g of CCl4, the percent yield can be calculated as:

Percent yield = 2.11 g / 3.51 g * 100 = 70.37%

Understanding percent yield is crucial in determining the efficiency of chemical reactions. It reflects how much of the expected product was obtained in reality. In this case, achieving a percent yield of 70.37% indicates a relatively successful reaction.