posted by Michelle

Lime (CaO) is used to prevent SO2 from escaping smokestacks of coal burning power plants by the formation of solid CaSO4•2H2O also known as the mineral gypsum. One of the important reactions in the overall process is the dissociation of CaCO3(s).

b. If a 12.0 g sample of solid CaCO3 is placed in an evacuated vessel at 725oC, what will the pressure of CO2 be when the system reaches equilibrium?

c. Which of the following actions cause an increase in the pressure of CO2 in the vessel described in question 2 above? Make your choice then justify your answer.
iii. Addition of more CaCO3 solid
iv. Increasing the volume of the vessel

d. If a 12.0 g sample of solid CaCO3 is placed in a vessel at 750oC in which the pressure of CO2 is 2.5 atm what mass of lime will form?

1. DrBob222

For a, do you have a Kc or Kp? Or does the question assume ALL of the CaCO3 decomposes?

2. Michelle

I have part b if that helps
100 g of CacO3 give 44 g of CO2

so 12 g will give 5.28 g of CO2

so moles of CO2 = 0.12 moles

Volume = 0.12 X 22.4 L = 2.688 L

PV = nRT

Pressure = 0.12 X 0.0821 X 998 / 2.688 = 3.65 atm

## Similar Questions

1. ### chemistry

I have been staring at this one for awhile now... I would so appreciate any help on approaching this problem! A certain sample of coal contains 1.6 percent sulfur by mass. When the coal is burned, the sulfur is converted to sulfur …
2. ### Chemistry

I was wondering if you could help me with this problem. If the reaction proceeds with a 96.8% yield, how many kilograms of CaSO4 are formed when 5.34 kg SO2 reacts with an exfess of CaCO3 and O2?
3. ### Chemistry

CaSO4.2H2O ==> CaSO4 + 2H2O moles CaSO4.2H2O = 15.00 g x (1 mole CaSO4.2H2O/172.172) = 0.08712 moles. moles CaSO4 = same. grams CaSO4 = moles CaSO4 x molar mass CaSO4 = ?
4. ### AP CHEM

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)  …
5. ### Chemistry Question

The reaction of quicklime (CaO) with sulfur dioxide (SO2) is an important reaction for reducing SO2 emissions from coal-fired power plants: CaO(s) + SO2(g) → CaSO3(s) This reaction is an example of: A. a precipitation reaction …
6. ### physics

If all the solid waste of 230 million tonnes were burned in waste-to-energy power plants that are 20% efficient, a) how many kilowatt-hours of electrical energy could be produced in a year?
7. ### physics

If all the solid waste of 230 million tonnes were burned in waste-to-energy power plants that are 20% efficient, a) how many kilowatt-hours of electrical energy could be produced in a year?
8. ### Chemistry<--------

Sulfur dioxide in the effluent gases from coal-burning electric power plants is one of the principal causes of acid rain. One method for reducing SO2 emissions involves partial reduction ofSO2 to H2S followed by catalytic conversion …
9. ### Chemistry

When coal is burned, the sulfur it contains is converted into sulfur dioxide. This is SO2 is a serious pollutant, so it needs to be removed before it escapes from the stack of a coal fired plant. One way to remove the SO2 is to add …
10. ### Chemsitry

Calcium Oxide is used to remove pollutant SO2 from smokestack gases. The ΔG° of the overall reaction CaO (s) + SO2 (g) + ½ O2 (g) ⇔ CaSO4 (s) is -418.6 kJ. What is PSO2 in equilibrium with air (PO2 = 0.21 atm) and solid CaO?

More Similar Questions