19. Burning coal and oil in a power plant produces pollutants such as sulfur dioxide, SO2. The sulfur-containing compound can be removed from other waste gases, however, by the following reaction:

2 SO2(g) + 2 CaCO3(s) + O2(g)  2 CaSO4(s) + 2 CO2(g)
[Molar masses: 64.07 100.1 32.00 136.2 44.01]
(a) Name the compounds involved in the reaction.
(b) What mass of CaCO3 is required to remove 155 g of SO2?
(c) What mass of CaSO4 is formed when 155 g SO2 is consumed completely?

(a) The compounds involved in the reaction are:

- SO2: Sulfur dioxide
- CaCO3: Calcium carbonate
- O2: Oxygen
- CaSO4: Calcium sulfate
- CO2: Carbon dioxide

(b) To find the mass of CaCO3 required to remove 155 g of SO2, we need to use stoichiometry.

From the balanced equation, we can see that the molar ratio between SO2 and CaCO3 is 2:2.

Molar mass of SO2 = 32.07 g/mol
Molar mass of CaCO3 = 100.1 g/mol

Using the molar ratio, we can set up the following equation:

(155 g SO2) x (1 mol SO2/64.07 g SO2) x (1 mol CaCO3/1 mol SO2) x (100.1 g CaCO3/1 mol CaCO3) = x

x is the mass of CaCO3 required to remove 155 g of SO2.

Simplifying the equation:

x = (155 g SO2) x (100.1 g CaCO3/64.07 g SO2) ≈ 242.2 g

Therefore, approximately 242.2 g of CaCO3 is required to remove 155 g of SO2.

(c) To find the mass of CaSO4 formed when 155 g of SO2 is consumed completely, we can use stoichiometry again.

From the balanced equation, we can see that the molar ratio between SO2 and CaSO4 is 2:2.

Using the molar masses of SO2 and CaSO4, we can set up the following equation:

(155 g SO2) x (1 mol SO2/64.07 g SO2) x (1 mol CaSO4/1 mol SO2) x (160.6 g CaSO4/1 mol CaSO4) = x

x is the mass of CaSO4 formed when 155 g of SO2 is consumed completely.

Simplifying the equation:

x = (155 g SO2) x (160.6 g CaSO4/64.07 g SO2) ≈ 387.0 g

Therefore, approximately 387.0 g of CaSO4 is formed when 155 g of SO2 is consumed completely.

To answer these questions, we will need to use stoichiometry. Stoichiometry is a branch of chemistry that deals with the calculation of quantities of substances involved in chemical reactions.

(a) Name the compounds involved in the reaction:
- SO2 (sulfur dioxide)
- CaCO3 (calcium carbonate)
- O2 (oxygen)
- CaSO4 (calcium sulfate)
- CO2 (carbon dioxide)

(b) What mass of CaCO3 is required to remove 155 g of SO2?

To calculate the mass of CaCO3 needed, we need to use the stoichiometry of the reaction. We can start by writing and balancing the chemical equation:

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

From the balanced equation, we can see that the stoichiometric ratio between SO2 and CaCO3 is 2:2. This means that for every 2 moles of SO2, we need 2 moles of CaCO3.

To calculate the mass, we need to convert the given mass of SO2 to moles, and then use the stoichiometric ratio to determine the mass of CaCO3.

The molar mass of SO2 is 64.07 g/mol. Therefore, the number of moles of SO2 can be calculated as:

Number of moles SO2 = Mass of SO2 / Molar mass of SO2
= 155 g / 64.07 g/mol

Now that we have the moles of SO2, we can use the stoichiometric ratio to find the moles of CaCO3. Since the stoichiometric ratio is 2:2, the moles of CaCO3 will be equal to the moles of SO2.

Number of moles CaCO3 = Number of moles SO2

Finally, we can calculate the mass of CaCO3 by multiplying the number of moles of CaCO3 by its molar mass:

Mass of CaCO3 = Number of moles CaCO3 * Molar mass of CaCO3

Plug in the given values and calculate the result.

(c) What mass of CaSO4 is formed when 155 g of SO2 is consumed completely?

To determine the mass of CaSO4 formed, we can use a similar approach. First, calculate the moles of SO2 as described in part (b), and then use the stoichiometric ratio between SO2 and CaSO4.

From the balanced equation:

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

We can see that the stoichiometric ratio between SO2 and CaSO4 is 2:2, just like with CaCO3. This means that the moles of SO2 will be equal to the moles of CaSO4.

Now, multiply the number of moles of CaSO4 by its molar mass to find the mass:

Mass of CaSO4 = Number of moles CaSO4 * Molar mass of CaSO4

Again, plug in the given values and calculate the result.

Surely you know the names.

For b and c follow the steps in this example.
http://www.jiskha.com/science/chemistry/stoichiometry.html