Question

1. Burning coal and oil in a power plant produces pollutants, such as sulfur dioxide, SO2. This compound can be removed by the following reaction:

2 SO2 (g) + 2 CaCO3 (s) + O2 (g) à 2 CaSO4 (s) + 2 CO2 (g)

a. How many grams of carbon dioxide are made from 155 g of SO2 ? This is the theoretical yield.

b. If the actual yield of carbon dioxide is 90.0 grams, what is the percent yield?

Answer 1

To find the mass of carbon dioxide produced from 155 g of SO2, we can use stoichiometry and the molar mass of SO2 and CO2.

Step-by-step explanation:

First, we need to calculate the molar mass of SO2 by adding the atomic masses of sulfur and oxygen. Sulfur has an atomic mass of 32.07 g/mol and oxygen has an atomic mass of 16.00 g/mol. The molar mass of SO2 is 32.07 g/mol + (2 x 16.00 g/mol) = 64.07 g/mol.

Next, we convert the given mass of SO2 to moles using the molar mass. 155 g of SO2 / 64.07 g/mol = 2.42 mol of SO2.

According to the balanced chemical equation, 2 mol of SO2 produces 2 mol of CO2. Therefore, 2.42 mol of SO2 will produce 2 x 2.42 mol = 4.84 mol of CO2.

To convert the moles of CO2 to grams, we multiply by the molar mass of CO2. The molar mass of CO2 is 12.01 g/mol + (2 x 16.00 g/mol) = 44.01 g/mol. Therefore, 4.84 mol of CO2 x 44.01 g/mol = 213.04 g of CO2.

Answer 2

Idk tbh srry man am in quarantine so I have a big packet to do