chemistry

In the reaction CaO(s) + SO2(g) ---> CaSO3(s)

(Hint: try drawing the Lewis structures of SO2 and SO32-)

a. ) Ca2+ acts as a Lewis base, and SO32- acts as a Lewis acid.
b. ) SO32- acts as a Lewis base, and SO2 acts as a Lewis acid.
c. ) O2- acts as a Lewis base, and SO2 acts as a Lewis acid.
d. ) SO2 acts as a Lewis base, and O2- acts as a Lewis acid.
e. ) SO2 acts as a Lewis base, and Ca2+ acts as a Lewis acid.

  1. 👍
  2. 👎
  3. 👁
  1. An electron acceptor is a Lewis acid.
    An electron donor is a Lewis base.

    1. 👍
    2. 👎
  2. would it be c)?

    1. 👍
    2. 👎
  3. I believe c is right. Can this question have more than one answer? What's wrong with answer b?

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Enthalpy Change Given the following reactions: S(s) + O2(g) → SO2(g) ΔH = -297 kJ/mol SO2(g) + ½ O2(g) → SO3(g) ΔH = -141 kJ/mol Calculate the ΔH for the reaction: S(s) + 3/2O2(g) → SO3(g)

  2. chemistry

    Use standard enthalpies of formation to calculate ΔHrxn° for each reaction. (See the appendix. Enter your answer to the tenth place.) (a) 2 H2S(g) + 3 O2(g) 2 H2O(l) + 2 SO2(g) (b) N2O4(g) + 4 H2(g) N2(g) + 4 H2O(g) (c) SO2(g) +

  3. chemistry

    what is thbe total number of molecules of so2 in a 0.10 mole same of so2

  4. chemistry

    If the reaction below proceeds with a 96.8% yield, how many kilograms of CaSO4 are formed when 5.97 kg SO2 reacts with an excess of CaCO3 and O2? 2 CaCO3(s) + 2 SO2(g) + O2(g) 2 CaSO4(g) + 2 CO2(g)

  1. CHEMISTRY

    Consider the following reaction: 2H2S+SO2=S(s)+H2O A reaction mixture initially containing 0.500M H2S and 0.500M SO2 was found to contain 1.0×10−3M at a certain temperature. A second reaction mixture at the same temperature

  2. Chemistry

    Consider the reaction: 2 SO2 (g) + O2 (g) ⇋ 2 SO3 (g) 4.0 mol of SO2 and 2.2 mol of O2 were placed in a 10 L flask and allowed to reach equilibrium. The flask was found to contain 2.6 mol SO2. Calculate the equilibrium constant

  3. chemistry

    What happens to the concentration of SO2(g) when the total pressure on the equilibrium reaction 2 SO2(g) + O2(g) 2 SO3(g) is increased (by compression)? I thought it remained the same but that was incorrect.

  4. chemistry

    Which of the following is considered a Lewis acid or a Lewis base. I- H2O BCl3 NH3 OH- H+ CO2 SO2

  1. 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

  2. Chemistry

    Sulfur dioxide (SO2) is an unwelcome result of burning soft coal in power plants. Some of the SO2 ends up as sulfuric acid in acid precipitation. The net reaction is 2 SO2(g) + O2(g) + 2 H2O(ℓ) −→ 2 H2SO4(ℓ) What mass in

  3. chemistry

    Nitrogen dioxide reacts with SO2 to form NO and SO3: $$NO2​(g)+SO2​(g) NO(g)+SO3​(g) An equilibrium mixture is analyzed at a certain temperature and found to contain [NO2] = 0.100 M, [SO2] = 0.300 M, [NO] = 2.00 M, and [SO3]

  4. 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?

You can view more similar questions or ask a new question.