AP Chemistry

The system CO2(g) + H2(g)<->H2O(g) + CO(g) is at equilibrium at some temperature. At equilibrium a 4.00 L vessel contains 1.00 mole CO2, 1.00 mole H2, 2.40 moles H2O, and 2.40
moles CO. How many moles of CO2 must be
added to the system to bring the equilibrium CO concentration to 0.679 mol/L?
Answer in units of moles

  1. 👍 0
  2. 👎 0
  3. 👁 290
  1. ........CO2 + H2 ==> H2O + CO
    E.....0.679+x etc.

    Then solve for x = (CO2) in M, and M x L = mols.

    1. 👍 0
    2. 👎 0
  2. The Ksp of Ni(CN)2 is 3.0 × 10−23. What is
    the molar solubility of Ni(CN)2 in a 0.065 M KCN solution?
    Answer in units of mol/L.

    I found that the normal molar solubility is 1.957x10^-8, but I don't know how the KCN solution affects it.
    Sig figs aren't accounted for.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    The equilibrium constant is equal to 5.00 at 1300K for the reaction 2SO2(g) + O2(g) 2SO3(g) if initial concentrations are [SO2] = 6.00M, [O2] = 0.45M, [SO3]= 9.00M, the system is a/. At equilibrium b/. Not at equilibrium and will

  2. AP Chem

    For the following equilibrium system, which of the following changes will form more CaCO3? CO2(g) + Ca(OH)2(s) CaCO3(s) + H2O(l) deltaH(rxn) = -113 kJ My choices are: a) Decrease temperature at a constant pressure (no phase

  3. AP Chemistry

    For the system 2SO2(g) + O2(g) 2SO3 (g), change in enthalpy is negative for the production of SO3. At a particular temperature, 8.00 moles of sulfur dioxide and 10.00 moles of sulfur trioxide are introduced into a 2.00 L

  4. chemistry

    Using dissociation constants from Appendix D in the textbook, determine the value for the equilibrium constant for each of the following reactions. (Remember that when reactions are added, the corresponding equilibrium constants

  1. Chemistry

    Consider the following equilibrium process at 686 C C02(g)+H2(g)=CO(g)+H20(g) The equilibrium concentration of the reacting species are [CO]=0.050M, [H2]=0.045M, [CO2]=0.086M, and [H20]=0.040M. (a)Calculate the Kc for the reaction

  2. Chemistry

    For the reaction: H2(g) + I2(g) 2HI(g) , Kc = 12.3 at some temperature T. If [H2] = [I2] = [HI] = 3.21 x 10-3 M at this temperature, which one of the following statements is true? 1. ) Not enough information is given to answer the

  3. Chemistry

    Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(g) + H2O(g) C2H5OH(g) Kc = 9.0 × 103 [C2H4]eq = 0.015 M

  4. chemistry

    carbon dioxide dissolves in water to form carbonic acid. Estimate the thermodynamic equilibrium constanst (K) for this reaction (delta Gf values: H2CO3= - 616.1, H2O= - 237.1, CO2= - 394.4) . Carbonic acid then ionizes in water

  1. Chemistry (please help me!)

    H2(g) + CO2(g) H20(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured: [H2]=0.20 M [CO2]=0.30 M

  2. science

    1.40g each of CO, H2O, and H2 are sealed in a 1.41−L vessel and brought to equilibrium at 600 K. CO(g)+H2O(g)⇌CO2(g)+H2(g)KC=23.2 How many grams of CO2 will be present in the equilibrium mixture?

  3. chemistry

    A mixture consisting of 1 mol of H2O (g) and 1 mol CO (g) is placed in a 11 L reaction vessel at 800 K. At equilibrium 0.647 mol CO2 (g) is present as a result of the reaction: CO(g) + H2O (g) --> CO2(g) + H2 What is K(equilibrium

  4. Chemistry

    Consider the hypothetical reaction: A + B + heat ⇌ C + D (All species are in the gaseous phase) What will happen to the concentration of A, B, C, and D under each of the following conditions? a) A catalyst is added to the

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