# chemistry

posted by .

When carbon dioxide is heated in a closed container, it decomposes into carbon monoxide and oxygen according to the following equilibrium equation:
2CO2(g) ---> 2CO(g) + O2(g)

When 2.0 mol of CO2(g) is placed in a 5.0-L closed container andheated to a particular temperature, the equilibrium concentration of CO2(g) is measured to be 0.039 mol/L. Use an ICE table to determine the equuilibrium concentrations of CO(g) and O2(g)

• chemistry -

It's difficult to do spacing on these boards but if I turn the equation down instead of sideways, we may be able to do it. First will be I, followed by C and E horizontally. Let me know if this is too confusing. (First, (CO2) = 2.0 mols/5 L = 0.4 mols/L.
2CO2(g)  0.4   -2x   0.039
|
|
v
2CO(g)     0   +2x
+
O2(g)     0   +x
If equilibrium for CO2 is 0.039 and it was 0.4 initially, that means it must have changed by 0.4 - 0.039 = 0.361 and that is 2x. Then CO must be the same and O2 must be 1/2 that.

• chemistry -

Calculate the solubility of zinc hydroxide at 25 °C. The Ksp of Zn(OH)2(s) is 4.5 x 10^-17 at 25 °C?

What did I do wrong?

Zn(OH)2 <----> Zn2+ + 2 OH-

let x = moles/L of Zn(OH)2 that dissolve. This gives us x moles/L of Zn2+ and 2x moles / L of OH-
[Zn2+] = x
[OH-] = 2x

Ksp = [Zn2+][OH-]^2 = x ( 2x)^2 = 4x^3

4.5 x 10^-17 = 4x^3

x = molar solubility = 2.2 x 10^-6 M

• chemistry -

2.2 x 10^-6 M looks ok to me. Perhaps they want g/L instead of mols/L.

## Similar Questions

1. ### chemistry

When carbon dioxide is heated in a closed container, it decomposes into carbon monoxide and oxygen according to the following equilibrium equation: 2CO2(g) 2CO(g) + O2(g) When 2.0 mol of CO2(g) is placed in a 5.0-L closed container …
2. ### chemistry

Gaseous CO2 decomposes to form the gaes CO and O2. At 20.0 degrees Celsius, =2.0*10^-8. 2.0 mol carbon dioxide is placed in a 5.0 L flask. What are the equilibrium concentrations of each species. My attempt to get the answer: Balanced …
3. ### Chemistry

"Given that the bond enthalpy of the carbon-oxygen bonds in carbon monoxide and carbon dioxide are 1073 kJ/mol and 743 kJ/mol respectively, and that of the bond in the oxygen molecule is 496 kJ/mol, calculate the enthalpy change for …
4. ### chemistry

What volume (in Liters) of oxygen must react to form 17.0L of carbon dioxide according to the following balanced equation: 2CO(g) + O2(g) --> 2CO2(g) 17.0 L CO2 x (1 moles O2/2 moles CO2) = 17.0 x (1/2) = 8.5 L did i do this problem …
5. ### #2 chemistry

2CO(g) + O2(g) ==> 2CO2(g) A. If 16.01 L of oxygen is reacted at STP, how many moles of carbon dioxide is produced?
6. ### ap chemistry

Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction: 2CO2 + O2 yields 2CO2 Delta H for this reaction is -566 kJ/mol run. What is the delta H for CO?
7. ### ap chemistry

Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction: 2CO + O2 yields 2CO2 Delta H for this reaction is -135.28 kcal. If 811.7 kcal is released, how many moles of CO must have reacted?
8. ### Chemistry

Just having some trouble with this chemistry problem.. Thanks for help! Toxic carbon monoxide (CO) gas is produced when fossil fuels such as petroleum burn without enough oxygen. The CO can eventually be converted to CO2 in the atmosphere. …
9. ### Chemistry

An equilibrium mixture contains 0.250 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) + H2O(g) <-> CO2(g)+ H2(g) …
10. ### AP Chemistry

Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction: 2CO(g) + O2(g) --> 2CO2(g) change in H for this reaction is −135.28 kcal. If 811.7 kcal is released, how many moles of CO must have reacted?

More Similar Questions